AQA GCSE (9-1) CHEMISTRY QUIZ on TOPIC 3 "QUANTITATIVE CHEMISTRY" (AQA science triology chemistry)

Given the following symbol equation:
2Mg + O₂ ==> 2MgO
Calculate how many g of magnesium oxide is formed by burning 24g of magnesium in air.
(Relative atomic masses, A_r: Mg = 24 and O = 16) [com-1]
1. 40
2. 16
3. 20
4. 80
Given the following symbol equation:
2Mg + O₂ ==> 2MgO
Calculate how many tonne of magnesium is needed to make 80 tonne of magnesium oxide.
(Relative atomic masses, A_r: Mg = 24 and O = 16) [com-2]
1. 96
2. 48
3. 24
4. 16
Given the following symbol equation:
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Calculate how many kg of calcium carbonate is needed to make 56 kg of calcium oxide.
(Relative atomic masses, A_r: Ca = 40, C = 12 and O = 16) [com-3]
1. 50
2. 44
3. 100
4. 40
Given the following symbol equation:
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Calculate how many g of carbon dioxide is formed if 25g of calcium carbonate is decomposed on heating to form 14g of calcium oxide.
(Relative atomic masses, A_r: Ca = 40, C = 12 and O = 16) [com-4]
1. 22
2. 44
3. 10
4. 11
Given the symbol equation to show the formation of iron sulfide:
Fe + S ==> FeS
Calculate the mass in g of iron sulfide formed when 5.6g of iron combines with 3.2g of sulfur.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-5]
1. 8.8
2. 2.4
3. 5.6
4. 3.2
Given the symbol equation to show the formation of iron sulfide:
Fe + S ==> FeS
Calculate the mass in g of iron sulfide formed when 28g of iron combines with 16g of sulfur.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-6]
1. 12
2. 44
3. 28
4. 16
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of calcium chloride formed when 20g of calcium combines with 35.5g of chlorine.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-7]
1. 15.5
2. 70.0
3. 55.5
4. 17.5
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of chlorine needed when 40g of calcium forms 111g of calcium chloride.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-8]
1. 80
2. 100
3. 151
4. 71
Given the symbol equation to show the formation of aluminium sulfide by heating a mixture of aluminium and sulfur:
2Al + 3S ==> Al₂S₃
How many g of sulfur is needed if 54g of aluminium is reacted to form 150g of aluminium sulfide?
(Relative atomic masses, A_r: Al = 27 and S = 32) [com-9]
1. 96
2. 204
3. 64
4. 27
Given the symbol equation to show the formation of aluminium sulfide by heating a mixture of aluminium and sulfur:
2Al + 3S ==> Al₂S₃
How many kg of sulfur is needed if 108kg of aluminium is reacted to form 300kg of aluminium sulfide?
(Relative atomic masses, A_r: Al = 27 and S = 32) [com-10]
1. 408
2. 192
3. 96
4. 32
Given the symbol equation to show the formation of iron sulfide by heating a mixture of iron and sulfur:
Fe + S ==> FeS
Calculate the mass in g of iron unreacted when 60g of iron reacts with 32g of sulfur to form 88g of iron sulfide.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-11]
1. 8
2. 32
3. 4
4. 56
Given the symbol equation to show the formation of iron sulfide by heating a mixture of iron and sulfur:
Fe + S ==> FeS
Calculate the mass in g of sulfur unreacted when 28g of iron reacts with 22g of sulfur to form 44g of iron sulfide.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-12]
1. 22
2. 16
3. 12
4. 6
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of calcium left unreacted when 25g of calcium reacts with 35.5g of chlorine.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-13]
1. 10.5
2. 5.0
3. 7.1
4. 12.5
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of chlorine left unreacted when 80g of calcium reacts with 150g of chlorine to form 222g of calcium chloride.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-14]
1. 70
2. 8
3. 16
4. 72
Given the following relative atomic masses: Cu = 64, S = 32 and O = 16; calculate the relative formula mass of copper sulfate, CuSO₄ [rfm-1]
1. 160
2. 112
3. 96
4. 336
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of ethane, C₂H₆ [rfm-2]
1. 13
2. 30
3. 18
4. 25
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of octane, C₈H₁₈ [rfm-3]
1. 13
2. 96
3. 114
4. 112
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of nitric acid, HNO₃ [rfm-4]
1. 31
2. 93
3. 62
4. 63
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of ammonium nitrate, NH₄NO₃ [rfm-5]
1. 80
2. 31
3. 90
4. 180
Given the following relative atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the relative formula mass of ammonium sulfate, (NH₄)₂SO₄ [rfm-6]
1. 63
2. 132
3. 216
4. 100
Given the following relative atomic masses: H = 1, O = 16 and S = 32; calculate the relative formula mass of sulfuric acid, H₂SO₄ [rfm-7]
1. 49
2. 194
3. 98
4. 66
Given the following relative atomic masses: O = 16, Al = 27 and S = 32; calculate the relative formula mass of aluminium sulfate, Al₂(SO₄)₃ [rfm-8]
1. 75
2. 315
3. 171
4. 342
Given the following relative atomic masses: H = 1 and Cl = 35.5, calculate the relative formula mass of hydrochloric acid, HCl [rfm-9]
1. 36.5
2. 18
3. 35.5
4. 37.5
Given the following relative atomic masses: Na = 23 and Cl = 35.5, calculate the relative formula mass of sodium chloride, NaCl [rfm-10]
1. 40
2. 58.5
3. 49.5
4. 35
Given the following relative atomic masses: Ca = 40 and Cl = 35.5, calculate the relative formula mass of calcium chloride, CaCl₂ [rfm-11]
1. 75.5
2. 151
3. 111
4. 146.5
Given the following relative atomic masses: H = 1, O = 16 and Mg = 24, calculate the relative formula mass of magnesium hydroxide, Mg(OH)₂ [rfm-12]
1. 41
2. 82
3. 42
4. 58
Given the following relative atomic masses: Al = 27 and Cl = 35.5, calculate the relative formula mass of aluminium chloride, AlCl₃ [rfm-13]
1. 133.5
2. 62.5
3. 187.5
4. 98
Given the following relative atomic masses: H = 1, O = 16 and Al = 27, calculate the relative formula mass of aluminium hydroxide, Al(OH)₃ [rfm-14]
1. 44
2. 78
3. 132
4. 46
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of glucose, C₆H₁₂O₆ [rfm-5]
1. 29
2. 40
3. 180
4. 90
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanol ('alcohol'), C₂H₅OH [rfm-16]
1. 29
2. 23
3. 41
4. 46
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanoic acid ('acetic acid'), CH₃COOH [rfm-17]
1. 60
2. 29
3. 84
4. 58
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(II) oxide, FeO [rfm-18]
1. 40
2. 72
3. 56
4. 16
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(III) oxide, Fe₂O₃ [rfm-19]
1. 72
2. 200
3. 160
4. 216
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of the iron oxide, Fe₃O₄ [rfm-20]
1. 72
2. 272
3. 174
4. 232
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of methane, CH₄ [rfm-21]
1. 16
2. 13
3. 52
4. 10
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of propane, C₃H₈ [rfm-22]
1. 13
2. 44
3. 99
4. 40
Given the following relative atomic masses: C = 12 and O = 16; calculate the relative molecular mass of carbon dioxide, CO₂ [rfm-23]
1. 28
2. 56
3. 44
4. 14
Given the following relative atomic masses: C = 12, O = 16 and Cu = 64; calculate the relative formula mass of copper carbonate, CuCO₃ [rfm-24]
1. 92
2. 276
3. 148
4. 124
Given the following relative atomic masses: C = 12, O = 16 and Ca = 40; calculate the relative formula mass of calcium carbonate, CaCO₃ [rfm-25]
1. 100
2. 68
3. 204
4. 124
How many moles of iron are there in 2.8g? (atomic mass Fe = 56) [mam-1]
1. 0.05
2. 156.8
3. 20.0
4. 2.0
How many moles of sulfur are there in 64g? (atomic mass S = 32) [mam-2]
1. 2048
2. 2.0
3. 0.5
4. 0.05
How many moles of sodium are there in 115g? (atomic mass Na = 23) [mam-3]
1. 2645
2. 0.2
3. 5
4. 4
How many moles of carbon are there in 3g? (atomic mass C = 12 ) [mam-4]
1. 36
2. 4
3. 0.5
4. 0.25
How many moles of zinc are there in 1.625g? (atomic mass Zn = 65) [mam-5]
1. 0.025
2. 105.6
3. 40.0
4. 100.0
How many moles of iodine are there in 12.7g of I₂? (atomic mass I = 127) [mam-6]
1. 10.0
2. 0.05
3. 0.10
4. 5.0
How many moles of chlorine are there in 213g of Cl₂? (atomic mass Cl = 35.5) [mam-7]
1. 0.17
2. 0.33
3. 3.0
4. 6.0
How many moles of bromine are there in 6.4g of Br₂? (atomic mass Br = 80) [mam-8]
1. 512
2. 1024
3. 0.08
4. 0.04
How many moles of phosphorus are there in 24.8g of P₄? (atomic mass P = 31) [mam-9]
1. 0.2
2. 0.8
3. 7688
4. 1922
How many moles of oxygen are there in 128g of O₂? (atomic mass O = 16) [mam-10]
1. 8
2. 4
3. 2048
4. 1032
How many moles of water are there in 4.5g of H₂O? (atomic masses: H = 1, O = 16) [mam-11]
1. 81
2. 0.26
3. 0.25
4. 72
How many moles of methane are there in 112g of CH₄? (atomic masses: C = 12, H = 1) [mam-12]
1. 8.6
2. 1792
3. 0.14
4. 7.0
How many moles of sodium sulfate are there in 7.1g of Na₂SO₄? (atomic masses: Na = 23, S = 32, O = 16) [mam-13]
1. 0.05
2. 10082
3. 20
4. 5
How many moles of sulfuric acid are there in 2.45g of H₂SO₄? (atomic masses: H = 1, S = 32, O = 16) [mam-14]
1. 240.1
2. 0.025
3. 40.0
4. 3.0
How many moles of calcium hydroxide are there in 25.9g of Ca(OH)₂? (atomic masses: Ca = 40, O = 16, H = 1) [mam-15]
1. 2.86
2. 1916
3. 0.35
4. 45.0
How many g are there in 1.5 moles of aluminium? (atomic mass Al = 27) [mam-16]
1. 0.056
2. 18.0
3. 9.0
4. 40.5
How many g are there in 0.02 moles of uranium? (atomic mass U = 238) [mam-17]
1. 4.76
2. 11900
3. 0.00008
4. 2.58
How many g are there in 0.65 moles of magnesium? (atomic mass Mg = 24) [mam-18]
1. 0.027
2. 15.6
3. 36.9
4. 7.8
How many g are there in 0.23 moles of silicon? (atomic mass Si = 28) [mam-19]
1. 0.0082
2. 121.7
3. 6.44
4. 0.82
How many g are there in 7.3 moles of boron? (atomic mass B = 10.8) [mam-20]
1. 0.68
2. 1.48
3. 70.0
4. 78.84
How many g are there in 0.05 moles of nitrogen, N ₂? (atomic mass N = 14) [mam-21]
1. 1.4
2. 2.4
3. 0.0035
4. 280
How many g are there in 0.75 moles of ozone, O₃? (atomic mass O = 16) [mam-22]
1. 0.047
2. 36.0
3. 12.0
4. 0.016
How many g are there in 2.5 moles of oxygen, O₂? (atomic mass O = 16) [mam-23]
1. 4.0
2. 6.4
3. 80.0
4. 40.0
How many g are there in 0.16 moles of chlorine, Cl₂? (atomic mass Cl = 35.5) [mam-24]
1. 5.68
2. 221.8
3. 443.8
4. 11.36
How many g are there in 1.65 moles of iodine, I₂? (atomic mass I = 127) [mam-25]
1. 419.1
2. 77.0
3. 154.0
4. 209.6
How many g are there in 3.6 moles of sodium hydroxide, NaOH? (atomic masses: Na = 23, O = 16, H = 1) [mam-26]
1. 0.09
2. 144
3. 11.1
4. 7.2
How many g are there in 1.5 moles of nitric acid, HNO₃? (atomic masses: H = 1, N = 14, O = 16) [mam-27]
1. 42.0
2. 0.024
3. 94.5
4. 46.5
How many g are there in 0.15 moles of ammonium sulfate, (NH₄)₂SO₄? (atomic masses: N = 14, H = 1, S = 32, O = 16) [mam-28]
1. 0.0011
2. 880.0
3. 17.1
4. 19.8
How many g are there in 0.8 moles of aluminium hydroxide, Al(OH)₃? (atomic masses: Al = 27, O = 16, H = 1) [mam-29]
1. 62.4
2. 97.5
3. 0.01
4. 10.0
How many g are there in 0.005 moles of sodium thiosulfate, Na₂S₂O₃? (atomic masses: Na = 23, S = 32, O =16) [mam-30]
1. 0.71
2. 0.79
3. 0.63
4. 0.55
It was found that 0.2 moles of atoms of an element had a mass of 3.2g. What is the relative atomic mass of the element? [mam-31]
1. 6.4
2. 8.0
3. 16.0
4. 15.0
It was found that 0.005 moles of atoms of an element had a mass of 0.295g. What is the relative atomic mass of the element? [mam-32]
1. 15
2. 60
3. 16
4. 59
It was found that 0.15 moles of atoms of an element had a mass of 10.95g. What is the relative atomic mass of the element? [mam-33]
1. 73
2. 164
3. 82
4. 146
It was found that 0.4 moles of atoms of an element had a mass of 56.2g. What is the relative atomic mass of the element? [mam-34]
1. 22.5
2. 140.5
3. 224.0
4. 25.0
It was found that 0.015 moles of atoms of an element had a mass of 2.88g. What is the relative atomic mass of the element? [mam-35]
1. 432
2. 450
3. 192
4. 200
It was found that 0.25 moles of atoms of an element had a mass of 40.65g. What is the relative atomic mass of the element? [mam-36]
1. 10.2
2. 102.0
3. 16.0
4. 162.6
It was found that 0.002 moles of a compound had a mass of 0.24g. What is the relative formula mass of the compound? [mam-37]
1. 120
2. 12
3. 48
4. 480
It was found that 0.005 moles of a compound had a mass of 0.2025g. What is the relative formula mass of the compound? [mam-38]
1. 101.3
2. 40.5
3. 24.7
4. 247
It was found that 0.25 moles of a compound had a mass of 14.05g. What is the relative formula mass of the compound? [mam-39]
1. 177.8
2. 35.1
3. 56.2
4. 28.1
It was found that 0.025 moles of a compound had a mass of 0.70g. What is the relative formula mass of the compound? [mam-40]
1. 175
2. 280
3. 140
4. 28
If 54g of aluminium combines with oxygen to form 102g of aluminium oxide, work out the formula of aluminium oxide. (Relative atomic masses: Al = 27 and O = 16) [emp-1]
1. Al₂O₃
2. Al₂O
3. AlO₂
4. AlO₃
In an experiment, 56g of iron combined with exactly 64g of sulfur. Work out the formula of the iron sulfide formed. (Relative atomic masses: Fe = 56 and S = 32) [emp-2]
1. FeS
2. FeS₂
3. Fe₂S
4. FeS₃
In an experiment, 21g of lithium combined with exactly 14g of nitrogen. Work out the formula of lithium nitride. (Relative atomic masses: Li = 7 and N = 14) [emp-3]
1. LiN₂
2. Li₂N
3. Li₃N
4. LiN₃
If 168g of iron combined with oxygen to form 232g of an iron oxide, work out the formula of the iron oxide. (Relative atomic masses: Fe = 56 and O = 16) [emp-4]
1. FeO
2. FeO₂
3. Fe₂O₃
4. Fe₃O₄
If 28g of silicon combined with oxygen to form 60g of silicon oxide, work out the formula of silicon oxide. (Relative atomic masses: Si = 28 and O = 16) [emp-5]
1. SiO₂
2. SiO
3. Si₂O
4. SiO₃
In an experiment, heating 128g of copper combined with exactly 32g of sulfur. Work out the formula of the copper sulfide formed. (Relative atomic masses: Cu = 64 and S = 32) [emp-6]
1. CuS
2. Cu₂S
3. CuS₂
4. CuS₄
In an experiment, excess chlorine was passed over 24g of heated magnesium metal until all the metal had reacted. If 95g of white magnesium chloride solid was formed, work out the formula of magnesium chloride. (Relative atomic masses: Mg = 24 and Cl = 35.5) [emp-7]
1. MgCl
2. Mg₂Cl
3. MgCl₂
4. MgCl₃
In an experiment, excess chlorine was passed over 27g of heated aluminium metal until all the metal had reacted. If 133.5g of white aluminium chloride was formed work out the formula of aluminium chloride. (Relative atomic masses: Al = 27 and Cl = 35.5) [emp-8]
1. Al₃Cl
2. AlCl₂
3. AlCl₄
4. AlCl₃
In an experiment, excess chlorine was passed over 28g of heated silicon until all of it had reacted. If 170g of liquid silicon chloride was formed work out the formula of silicon chloride. (Relative atomic masses: Si = 28 and Cl = 35.5) [emp-9]
1. SiCl₄
2. SiCl₂
3. Si₂Cl
4. Si₄Cl
In an experiment, excess chlorine was passed over 31g of hot phosphorus until all of it had reacted. If 208.5g of white phosphorus chloride was formed work out the formula of phosphorus chloride. (Relative atomic masses: P = 31 and Cl = 35.5) [emp-10]
1. PCl₃
2. PCl₅
3. PCl₆
4. PCl₇
If 8g of sulfur combines with 12g of oxygen, what is the formula of the sulfur oxide formed? (Relative atomic masses: S = 32 and O = 16) [emp-11]
1. SO
2. SO₂
3. SO₃
4. SO₄
If 16g of sulfur combines with 103.5g of lead, what is the formula of the lead sulfide formed? (Relative atomic masses: S = 32 and Pb = 207) [emp-12]
1. Pb₂S
2. PbS₂
3. PbS₆
4. PbS
If 40g of calcium combines with 160g of bromine, what is the formula of calcium bromide? (Relative atomic masses: Ca = 40 and Br = 80) [emp-13]
1. CaBr₂
2. CaBr
3. CaBr₃
4. Ca₂Br
78g of potassium combines with 160g of bromine. What is the simplest formula of potassium bromide? (Relative atomic masses: K = 39 and Br = 80) [emp-14]
1. KBr₂
2. KBr
3. K₂Br
4. KBr₄
48g of magnesium combines with 320g of bromine, what is the formula of magnesium bromide? (Relative atomic masses: Mg = 24 and Br = 80) [emp-15]
1. MgBr
2. Mg₂Br
3. MgBr₂
4. MgBr₃
160g of calcium combines with 64g of oxygen, what is the formula of calcium oxide? (Relative atomic masses: Ca = 40 and O = 16) [emp-16]
1. CaO₂
2. Ca₂O
3. Ca₄O₄
4. CaO
What is the formula of the phosphorus oxide formed when 62g of phosphorus combines with 80g of oxygen? (Relative atomic masses: P = 31 and O = 16) [emp-17]
1. P₂O₅
2. PO
3. P₂O
4. PO₅
72g of magnesium combines with 48g of oxygen, what is the formula of magnesium oxide? (Relative atomic masses: Mg = 24 and O = 16) [emp-18]
1. MgO₂
2. MgO
3. Mg₃O₃
4. Mg₂O
46g of sodium combined with 16g of oxygen. What is the formula of the sodium oxide formed? (Relative atomic masses: Na = 23 and O = 16) [emp-19]
1. NaO
2. NaO₂
3. Na₂O
4. Na₂O₂
78g of potassium combined with 32g of sulfur. What is the formula of potassium sulfide formed? (Relative atomic masses: K = 39 and S = 32) [emp-20]
1. KS
2. KS₂
3. K₂S₂
4. K₂S
56g of iron combined with 240g of bromine. What is the formula of the iron bromide formed? (Relative atomic masses: Fe = 56 and Br = 80) [emp-21]
1. FeBr₃
2. FeBr₂
3. Fe₃Br
4. FeBr
If 20.9g of bismuth combines with 24.0g of bromine, what is the formula of the bismuth bromide formed? (Relative atomic masses: Bi = 209 and Br = 80) [emp-22]
1. BiBr
2. BiBr₃
3. Bi₃Br
4. BiBr₂
If 54g of aluminium combines with 96g of sulfur, what is the formula of aluminium sulfide? (Relative atomic masses: Al = 27 and S = 32) [emp-23]
1. AlS
2. AlS₃
3. Al₂S₃
4. Al₂S
When 117g of potassium combines with 31g of phosphorus, what is the formula of the potassium phosphide formed? (Relative atomic masses: K = 39 and P = 31) [emp-24]
1. KP
2. KP₃
3. KP₂
4. K₃P
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, how many g of magnesium is needed to make 10g of magnesium oxide? [rmc-1]
1. 6.0
2. 3.0
3. 1.2
4. 2.4
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, how many tonne of magnesium oxide can be made from 3 tonne of magnesium? [rmc-2]
1. 2.4
2. 5.0
3. 8.0
4. 4.8
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, what mass of oxygen in g, combines with 240g of magnesium? [rmc-3]
1. 64
2. 80
3. 160
4. 32
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of iron sulfide can be made from 14g of iron? [rmc-4]
1. 44
2. 28
3. 16
4. 22
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of sulfur reacts with 224g of iron? [rmc-5]
1. 128
2. 32
3. 64
4. 112
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of iron is needed to make 440g of iron sulfide? [rmc-6]
1. 56
2. 280
3. 220
4. 168
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many tonne of iron can be made from 40 tonnes of haematite ore? [rmc-7]
1. 56
2. 14
3. 28
4. 7
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many tonne of haematite ore are needed to make 224 tonne of iron? [rmc-8]
1. 160
2. 480
3. 640
4. 320
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how g of carbon monoxide are needed to reduce 32g of iron oxide to iron? [rmc-9]
1. 16.8
2. 33.6
3. 8.4
4. 28.0
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many g of carbon dioxide are formed when 80 g of haematite is reduced to iron? [rmc-10]
1. 44
2. 66
3. 33
4. 40
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, how many tonne of limestone is needed to make 112 tonne of lime? [rmc-11]
1. 224
2. 400
3. 200
4. 300
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, what mass in g of lime is made from 20g of limestone? [rmc-12]
1. 8.8
2. 5.6
3. 4.4
4. 11.2
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, how many tonne of carbon dioxide is formed by decomposing 400 tonne of calcium carbonate? [rmc-13]
1. 176
2. 44
3. 88
4. 132
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of zinc carbonate are needed to make 68g of zinc chloride?? [rmc-14]
1. 125.0
2. 62.5
3. 68.0
4. 136.0
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of HCl are needed to make 408g of zinc chloride? [rmc-15]
1. 109.5
2. 36.5
3. 219.0
4. 71.0
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, what mass of zinc chloride in g can be made from 25g of zinc carbonate? [rmc-16]
1. 54.4
2. 12.5
3. 13.6
4. 27.2
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of water are formed when 250g of zinc carbonate reacts? [rmc-17]
1. 36
2. 18
3. 9
4. 27
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of carbon dioxide are formed when 3.65g of hydrochloric acid reacts? [rmc-18]
1. 4.4
2. 2.2
3. 1.1
4. 8.8
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of sodium hydroxide is needed to make 213g of sodium sulfate? [rmc-19]
1. 40
2. 80
3. 120
4. 160
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, what mass in g of sulfuric acid is needed to make 7.1g of sodium sulfate? [rmc-20]
1. 9.8
2. 14.7
3. 19.6
4. 4.9
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of sodium sulfate is formed when 8g of sodium hydroxide reacts? [rmc-21]
1. 14.2
2. 28.4
3. 7.1
4. 21.3
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of water are formed when 49g of sulfuric acid reacts? [rmc-22]
1. 9
2. 18
3. 36
4. 23
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many g of copper can be made from 320g of the copper ore?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-23]
1. 128
2. 64
3. 256
4. 192
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of oxygen are needed to convert 40 tonnes of ore to copper?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-24]
1. 16
2. 32
3. 12
4. 8
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of sulfur dioxide are produced for every 1280 tonnes of ore processed?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-25]
1. 512
2. 128
3. 256
4. 64
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of ore are needed to make 25.6 tonnes of copper?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-26]
1. 64
2. 32
3. 48
4. 56
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the hydrogen chloride reaction is:
2Al_(s) + 6HCl_(g) ==> 2AlCl_3(s) + 3H_2(g)
How many kg of aluminium chloride can be made from 27 kg of aluminium?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1.0) [rmc-27]
1. 267.0
2. 400.5
3. 133.5
4. 66.75
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the hydrogen chloride reaction is:
2Al_(s) + 6HCl_(g) ==> 2AlCl_3(s) + 3H_2(g)
How many tonnes of hydrogen would be produced by reacting 108 tonnes of aluminium?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1.0) [rmc-28]
1. 2
2. 3
3. 6
4. 12
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the chlorine reaction is:
2Al_(s) + 3Cl_2(g) ==> 2AlCl_3(s)
How much aluminium is needed to make 89 g of aluminium chloride?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H =1) [rmc-29]
1. 18
2. 27
3. 54
4. 9
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the chlorine reaction is:
2Al_(s) + 3Cl_2(g) ==> 2AlCl_3(s)
How many tonne of chlorine is needed to make 1068 tonne of aluminium chloride?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1) [rmc-30]
1. 71
2. 852
3. 426
4. 213
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many tonne of lead can be made from 223 tonne of ore?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-31]
1. 414.0
2. 103.5
3. 207.0
4. 310.5
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many tonne of ore is needed to make 828 tonne of lead?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-32]
1. 223
2. 446
3. 1784
4. 892
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many kg of carbon is needed to make 828 kg of lead?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-33]
1. 24
2. 12
3. 6
4. 48
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many g of carbon dioxide are formed when 207 g of lead are produced?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-34]
1. 44
2. 22
3. 11
4. 33
What is the molarity of the solution formed by dissolving 20 g of sodium hydroxide (NaOH) in 1000 cm³ of water? (A_r's: Na=23, O=16, H=1) [msc-1]
1. 0.50
2. 0.25
3. 1.00
4. 2.00
What is the molarity of the solution formed by dissolving 10 g of sodium hydroxide (NaOH) in 500 cm³ of water? (A_r's: Na=23, O=16, H=1) [msc-2]
1. 1.00
2. 0.50
3. 0.25
4. 2.00
What is the molarity of the solution formed by dissolving 80 g of sodium hydroxide (NaOH) in 500 cm³ of water? (A_r's: Na=23, O=16, H=1) [msc-3]
1. 2
2. 1
3. 4
4. 8
What is the molarity of the solution formed by dissolving 9.8 g of sulfuric acid (H₂SO₄) in 1000 cm³ of water? (A_r's: H=1, S=32, O=16) [msc-4]
1. 10.0
2. 0.01
3. 1.0
4. 0.1
What is the molarity of the solution formed by dissolving 196 g of sulfuric acid (H₂SO₄) in 1000 cm³ of water? (A_r's: H=1, S=32, O=16) [msc-5]
1. 2.0
2. 0.5
3. 3.0
4. 1.5
What is the molarity of the solution formed by dissolving 49 g of sulfuric acid (H₂SO₄) in 250 cm³ of water? (A_r's: H=1, S=32, O=16) [msc-6]
1. 0.4
2. 2.0
3. 0.5
4. 1.0
What mass (g) of potassium hydroxide (KOH) is needed to make up 1000cm³ of a solution of concentration 1mol/dm³? (A_r's: K=39, O=16, H=1) [msc-7]
1. 0.056
2. 0.56
3. 56
4. 560
What mass (g) of potassium hydroxide (KOH) is needed to make up 500cm³ of a solution of concentration 0.2mol/dm³? (A_r's: K=39, O=16, H=1) [msc-8]
1. 11.2
2. 2.8
3. 0.56
4. 5.6
What mass (g) of potassium hydroxide (KOH) is needed to make up 500cm³ of a solution of concentration 4.0mol/dm³? (A_r's: K=39, O=16, H=1) [msc-9]
1. 112
2. 56
3. 224
4. 28
What mass (g) of hydrogen chloride (HCl) is needed to make up 1000cm³ of a solution of concentration 1mol/dm³? (A_r's: H=1, Cl=35.5) [msc-10]
1. 73
2. 36.5
3. 0.036
4. 0.073
What mass (g) of hydrogen chloride (HCl) is needed to make up 500cm³ of a solution of concentration 4mol/dm³? (A_r's: H=1, Cl=35.5) [msc-11]
1. 36.5
2. 146
3. 73
4. 292
What mass (g) of hydrogen chloride (HCl) is needed to make up 500cm³ of a solution of concentration 0.2mol/dm³? (A_r's: H=1, Cl=35.5) [msc-12]
1. 7.30
2. 14.6
3. 1.83
4. 3.65
Given the neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
25 cm³ of hydrochloric acid are neutralised by 20 cm³ of 0.05M sodium hydroxide. What is the molarity of the acid? [vct-1]
1. 0.04
2. 0.02
3. 1.25
4. 0.80
Given the neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
15 cm³ of hydrochloric acid are neutralised by 25 cm³ of 0.06M sodium hydroxide. What is the molarity of the acid? [vct-2]
1. 0.40
2. 0.10
3. 0.04
4. 0.01
Given the neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
40 cm³ of 0.05M hydrochloric acid are neutralised by 20 cm³ of a sodium hydroxide solution. What is the molarity of the alkali? [vct-3]
1. 0.20
2. 0.05
3. 0.10
4. 0.50
Given the neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
25 cm³ of 0.16M hydrochloric acid are neutralised by 10 cm³ of a sodium hydroxide solution. What is the molarity of the alkali? [vct-4]
1. 0.2
2. 0.1
3. 0.8
4. 0.4
Given the neutralisation equation:
2KOH_(aq) + H₂SO_4(aq) ==> K₂SO_4(aq) + 2H₂O_(l)
What is the molarity of a sulfuric acid solution, if 15 cm³ of it are neutralised by 20 cm³ of a 0.3 M potassium hydroxide solution? [vct-5]
1. 0.20
2. 0.15
3. 0.40
4. 0.75
Given the neutralisation equation:
2KOH_(aq) + H₂SO_4(aq) ==> K₂SO_4(aq) + 2H₂O_(l)
What is the molarity of a sulfuric acid solution, if 30 cm³ of it are neutralised by 10 cm³ of a 0.6 M potassium hydroxide solution? [vct-6]
1. 0.20
2. 0.10
3. 0.05
4. 0.25
Given the neutralisation equation:
2KOH_(aq) + H₂SO_4(aq) ==> K₂SO_4(aq) +2H₂O_(l)
What is the molarity of a potassium hydroxide solution, if 10 cm³ of it are neutralised by 12 cm³ of a 0.5 M sulfuric acid solution? [vct-7]
1. 2.4
2. 0.6
3. 1.2
4. 0.6
Given the neutralisation equation:
2KOH_(aq) + H₂SO_4(aq) ==> K₂SO_4(aq) + 2H₂O_(l)
What is the molarity of a potassium hydroxide solution, if 5 cm³ of it are neutralised by 20 cm³ of a 1 M sulfuric acid solution? [vct-8]
1. 16
2. 4
3. 5
4. 8
Given the neutralisation equation:
3NaOH_(aq) + H₃PO_4(aq) ==> Na₃PO_4(aq) + 3H₂O_(l)
What is the molarity of a phosphoric acid solution, if 15 cm³ of it are neutralised by 22.5 cm³ of a 0.2 M sodium hydroxide solution? [vct-9]
1. 0.10
2. 0.30
3. 0.03
4. 0.01
Given the neutralisation equation:
3NaOH_(aq) + H₃PO_4(aq) ==> Na₃PO_4(aq) + 3H₂O_(l)
What is the molarity of a phosphoric acid solution, if 40 cm³ of it are neutralised by 15 cm³ of a 0.4 M sodium hydroxide solution? [vct-10]
1. 0.150
2. 0.050
3. 0.017
4. 0.115
Given the neutralisation equation:
3NaOH_(aq) + H₃PO_4(aq) ==> Na₃PO_4(aq) + 3H₂O_(l)
What is the molarity of a sodium hydroxide solution, if 21.6 cm³ of it are neutralised by 18 cm³ of a 0.2 M phosphoric acid solution? [vct-11]
1. 1.50
2. 1.15
3. 0.50
4. 0.17
Given the neutralisation equation:
3NaOH_(aq) + H₃PO_4(aq) ==> Na₃PO_4(aq) + 3H₂O_(l)
What is the molarity of a sodium hydroxide solution, if 15 cm³ of it are neutralised by 20 cm³ of a 0.6 M phosphoric acid solution? [vct-12]
1. 1.2
2. 7.2
3. 0.8
4. 2.4
Given the equation: 2Na_(s) + 2H₂O_(l) ==> 2NaOH_(aq) + H_2(g)
Calculate the volume of hydrogen formed in dm³ when 2.3g of sodium reacts with water. (A_r's Na=23, H=1, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-1]
1. 1.2
2. 2.4
3. 4.8
4. 0.6
Given the equation: 2Na_(s) + 2H₂O_(l) ==> 2NaOH_(aq) + H_2(g)
Calculate the volume of hydrogen formed in dm³ when 9.2g of sodium reacts with water. (A_r's Na=23, H=1, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-2]
1. 2.4
2. 4.8
3. 9.6
4. 1.2
Given the equation: 2Na_(s) + 2H₂O_(l) ==> 2NaOH_(aq) + H_2(g)
What mass of sodium in g will form 600 cm³ of hydrogen gas? (A_r's Na=23, H=1, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-3]
1. 2.30
2. 2.40
3. 1.15
4. 4.60
Given the equation: 2Na_(s) + 2H₂O_(l) ==> 2NaOH_(aq) + H_2(g)
What mass of sodium in g will form 18 dm³ of hydrogen gas? (A_r's Na=23, H=1, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-4]
1. 23.0
2. 46.0
3. 16.5
4. 34.5
Given the equation for the thermal decomposition of calcium carbonate (limestone):
CaCO_3(s) ==> CaO_(s) + CO_2(g)
What volume of carbon dioxide in dm³ is formed when 10g of limestone is heated strongly? (A_r's Ca=40, C=12, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-5]
1. 2.4
2. 4.8
3. 1.2
4. 4.4
Given the equation for the thermal decomposition of calcium carbonate (limestone) ...
CaCO_3(s) ==> CaO_(s) + CO_2(g)
What volume of carbon dioxide in dm³ is formed when 200g of limestone is heated strongly? (A_r's Ca=40, C=12, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-6]
1. 24
2. 48
3. 12
4. 96
Given the equation for the thermal decomposition of calcium carbonate (limestone) ...
CaCO_3(s) ==> CaO_(s) + CO_2(g)
What mass of limestone in g, on strong heating, will form 6 dm³ carbon dioxide? (A_r's Ca=40, C=12, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-7]
1. 50
2. 56
3. 25
4. 12
Given the equation for the thermal decomposition of calcium carbonate (limestone) ...
CaCO_3(s) ==> CaO_(s) + CO_2(g)
What mass of limestone in g, on strong heating, will form 120 cm³ carbon dioxide? (A_r's Ca=40, C=12, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-8]
1. 0.3
2. 1.0
3. 2.0
4. 0.5
5 g of a gas had a volume of 60 dm³. What is its molecular mass? (1 mol gas = 24 dm³ at room temp./press.) [mvg-9]
1. 2
2. 6
3. 4
4. 12
What is the volume in dm³ of 8 g of a gas of molecular mass 16? (1 mol gas = 24 dm³ at room temp./press.) [mvg-10]
1. 6
2. 12
3. 0.5
4. 2
What mass of gas, of molecular mass 36.5, is present in 4.8 dm³ of the gas? (1 mol gas = 24 dm³ at room temp./press.) [mvg-11]
1. 14.6
2. 3.65
3. 7.30
4. 0.76
0.145 g of a gas had a volume of 60 cm³. What is its molecular mass? (1 mol gas = 24 dm³ at room temp./press.) [mvg-12]
1. 29
2. 30
3. 116
4. 58
What is the volume in dm³ of 0.85 g of a gas of molecular mass 17? (1 mol gas = 24 dm³ at room temp./press.) [mvg-13]
1. 1.2
2. 0.6
3. 2.4
4. 3.4
What mass of gas, of molecular mass 71, is present in 1.2 dm³ of the gas? (1 mol gas = 24 dm³ at room temp./press.) [mvg-14]
1. 14.2
2. 3.55
3. 7.10
4. 8.52
2.55g of a gas had a volume of 0.6 dm³. What is its molecular mass? (1 mol gas = 24 dm³ at room temp./press.) [mvg-15]
1. 17
2. 51
3. 102
4. 34
What is the volume in dm³ of 1 g of a gas of molecular mass 96? (1 mol gas = 24 dm³ at room temp./press.) [mvg-16]
1. 4.00
2. 0.50
3. 1.92
4. 0.25
What mass of gas, of molecular mass 44, is present in 0.15 dm³ of the gas? (1 mol gas = 24 dm³ at room temp./press.) [mvg-17]
1. 0.275
2. 6.600
3. 3.600
4. 0.003
What is the volume in dm³ of 0.8 g of a gas of molecular mass 32? (1 mol gas = 24 dm³ at room temp./press.) [mvg-18]
1. 0.025
2. 0.6
3. 19.2
4. 1.33
Given the equation for magnesium dissolving in hydrochloric acid:
Mg_(s) + 2HCl_(aq) ==> MgCl_2(aq) + H_2(g)
What mass of magnesium in g, will form 1.2 dm³ of hydrogen gas? (A_r's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-19]
1. 28.8
2. 0.6
3. 1.2
4. 2.4
Given the equation for magnesium dissolving in hydrochloric acid:
Mg_(s) + 2HCl_(aq) ==> MgCl_2(aq) + H_2(g)
What mass of magnesium in g, will form 36 dm³ of hydrogen gas? (A_r's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-20]
1. 24
2. 12
3. 72
4. 36
Given the equation for magnesium dissolving in hydrochloric acid:
Mg_(s) + 2HCl_(aq) ==> MgCl_2(aq) + H_2(g)
What volume of hydrogen gas, in dm³, is formed when 4g of magnesium dissolves in the acid? (A_r's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-21]
1. 4
2. 2
3. 6
4. 3
Given the equation for magnesium dissolving in hydrochloric acid:
Mg_(s) + 2HCl_(aq) ==> MgCl_2(aq) + H_2(g)
What volume of hydrogen gas, in dm³, is formed when 72g of magnesium dissolves in the acid? (A_r's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-22]
1. 36
2. 72
3. 48
4. 24
Given the equation for aluminium dissolving in dilute sulfuric acid:
2Al_(s) + 3H₂SO_4(aq) ==> Al₂(SO₄)_3(aq) + 3H_2(g)
What mass of aluminium (g) dissolves when 7.2 dm³ of hydrogen is formed? (A_r's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-23]
1. 2.7
2. 0.3
3. 5.4
4. 16.2
Given the equation for aluminium dissolving in dilute sulfuric acid:
2Al_(s) + 3H₂SO_4(aq) ==> Al₂(SO₄)_3(aq) + 3H_2(g)
What mass of aluminium in g, dissolves when 48 dm³ of hydrogen is formed? (A_r's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-24]
1. 18
2. 6
3. 18
4. 36
Given the equation for aluminium dissolving in dilute sulfuric acid:
2Al_(s) + 3H₂SO_4(aq) ==> Al₂(SO₄)_3(aq) + 3H_2(g)
What volume of hydrogen, in dm³, is formed, when 54g of aluminium dissolves? (A_r's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-25]
1. 72
2. 24
3. 48
4. 36
Given the equation for aluminium dissolving in dilute sulfuric acid:
2Al_(s) + 3H₂SO_4(aq) ==> Al₂(SO₄)_3(aq) + 3H_2(g)
What volume of hydrogen, in dm³, when 27g of aluminium dissolves? (A_r's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-26]
1. 12
2. 36
3. 18
4. 24
Given the equation for calcium carbonate dissolving in hydrochloric acid:
CaCO_3(s) + 2HCl_(aq) ==> CaCl_2(aq) + H₂O_(l) + CO_2(g)
Calculate the volume of carbon dioxide, in dm³, when 5 g of calcium carbonate dissolves in the acid. (A_r's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-27]
1. 2.4
2. 0.6
3. 1.2
4. 1.8
Given the equation for calcium carbonate dissolving in hydrochloric acid:
CaCO_3(s) + 2HCl_(aq) ==> CaCl_2(aq) + H₂O_(l) + CO_2(g)
Calculate the volume of carbon dioxide, in dm³, when 400 g of calcium carbonate dissolves in the acid. (A_r's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-28]
1. 48
2. 6
3. 24
4. 96
Given the equation for calcium carbonate dissolving in hydrochloric acid:
CaCO_3(s) + 2HCl_(aq) ==> CaCl_2(aq) + H₂O_(l) + CO_2(g)
Calculate the mass of calcium carbonate (in g) that dissolves when 6 dm³ of carbon dioxide is formed. (A_r's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-29]
1. 25.0
2. 12.5
3. 6.0
4. 100.0
Given the equation for calcium carbonate dissolving in hydrochloric acid:
CaCO_3(s) + 2HCl_(aq) ==> CaCl_2(aq) + H₂O_(l) + CO_2(g)
Calculate the mass of calcium carbonate (in g) that dissolves when 36 dm³ of carbon dioxide is formed. (A_r's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-30]
1. 66
2. 150
3. 100
4. 44
Given the reaction between hydrogen and chlorine to form hydrogen chloride:
H_2(g) + Cl_2(g) ==> 2HCl_(g)
What volume of hydrogen in cm³ is needed to make 100cm³ of hydrogen chloride? [rgv-1]
1. 50
2. 100
3. 200
4. 150
Given the reaction between hydrogen and chlorine to form hydrogen chloride:
H_2(g) + Cl_2(g) ==> 2HCl_(g)
What volume of chlorine in dm³ is needed to make 40dm³ of hydrogen chloride? [rgv-2]
1. 40
2. 20
3. 10
4. 30
Given the reaction between hydrogen and chlorine to form hydrogen chloride:
H_2(g) + Cl_2(g) ==> 2HCl_(g)
What volume of hydrogen chloride in dm³ is made by reacting 20dm³ of hydrogen? [rgv-3]
1. 20
2. 30
3. 40
4. 10
Given the reaction between hydrogen and chlorine to form hydrogen chloride:
H_2(g) + Cl_2(g) ==> 2HCl_(g)
What volume of hydrogen chloride in cm³ is made by reacting 300cm³ of chlorine? [rgv-4]
1. 300
2. 450
3. 150
4. 600
Given the reaction between nitrogen and hydrogen to form ammonia:
N_2(g) + 3H_2(g) ==> 2NH_3(g)
What volume of ammonia in cm³ is formed if 180cm³ of hydrogen reacts? [rgv-5]
1. 120
2. 180
3. 90
4. 60
Given the reaction between nitrogen and hydrogen to form ammonia:
N_2(g) + 3H_2(g) ==> 2NH_3(g)
What volume of ammonia in dm³ is formed if 40dm³ of nitrogen reacts? [rgv-6]
1. 120
2. 80
3. 40
4. 160
Given the reaction between nitrogen and hydrogen to form ammonia:
N_2(g) + 3H_2(g) ==> 2NH_3(g)
What volume of hydrogen in dm³ is needed to make 60dm³ of ammonia? [rgv-7]
1. 45
2. 60
3. 90
4. 30
Given the reaction between nitrogen and hydrogen to form ammonia:
N_2(g) + 3H_2(g) ==> 2NH_3(g)
What volume of nitrogen in cm³ is needed to make 640cm³ of ammonia? [rgv-8]
1. 640
2. 960
3. 160
4. 320
The combustion of methane is given by the equation:
CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(l)
What volume of oxygen in cm³ is needed to burn 200cm³ of methane? [rgv-9]
1. 400
2. 200
3. 300
4. 800
The combustion of methane is given by the equation:
CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(l)
What volume of carbon dioxide in cm³ is formed on burning 10cm³ of methane? [rgv-10]
1. 20
2. 10
3. 40
4. 30
The combustion of methane is given by the equation:
CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(g)
What is the total volume of gases produced in cm³ when 30cm³ of methane burns? [rgv-11]
1. 30
2. 60
3. 90
4. 120
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(l)
What volume of oxygen in cm³ is needed to burn 20cm³ of propane? [rgv-12]
1. 50
2. 70
3. 200
4. 100
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(l)
What volume of propane in cm³ can be completely burned by 200cm³ of oxygen? [rgv-13]
1. 40
2. 50
3. 80
4. 20
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(l)
What volume of carbon dioxide in dm³ is formed by burning 30dm³ of propane? [rgv-14]
1. 60
2. 90
3. 150
4. 50
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(g)
What total volume of gases in cm³ is formed by burning 40cm³ of propane? [rgv-15]
1. 120
2. 160
3. 280
4. 200
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(g)
What volume of steam in cm³ is formed by burning 20cm³ of propane? [rgv-16]
1. 100
2. 160
3. 40
4. 80
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(l)
What volume of carbon dioxide in cm³ is formed by burning 20cm³ of ethane? [rgv-17]
1. 40
2. 20
3. 80
4. 70
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(l)
What volume of oxygen in cm³ is needed to completely burn 60cm³ of ethane? [rgv-18]
1. 420
2. 210
3. 105
4. 120
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(g)
What volume of steam in dm³ is formed when 40dm³ of ethane burns? [rgv-19]
1. 240
2. 60
3. 120
4. 80
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(g)
What total volume of gases in dm³ are formed when 15dm³ of ethane burns? [rgv-20]
1. 150
2. 30
3. 45
4. 75
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(g)
What volume of ethane in cm³ can be burned completely using 175cm³ of oxygen? [rgv-21]
1. 50
2. 100
3. 25
4. 75
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below.
C₁₈H_38(g) ==> C₆H_14(g) + 2C₃H_6(g) + 3C₂H_4(g)
What total volume in dm³ of hydrocarbon gases are formed when 20dm³ of the large hydrocarbon are broken down? [rgv-22]
1. 60
2. 120
3. 40
4. 80
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below.
C₁₈H_38(g) ==> C₆H_14(g) + 2C₃H_6(g) + 3C₂H_4(g)
What volume in cm³ of propene gas is formed when 120cm³ of the large hydrocarbon are broken down? [rgv-23]
1. 120
2. 360
3. 240
4. 20
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below.
C₁₈H_38(g) ==> C₆H_14(g) + 2C₃H_6(g) + 3C₂H_4(g)
What volume in cm³ of ethene gas is formed when 40cm³ of the large hydrocarbon are broken down? [rgv-24]
1. 40
2. 80
3. 240
4. 120
Which four quantities a, b, c and d are required to balance the equation ...
aCH_4(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-1]
1. 1 2 1 2
2. 1 1 1 2
3. 1 2 2 1
4. 1 1 1 1
Which four quantities a, b, c and d are required to balance the equation ...
aC₂H_6(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-2]
1. 1 2 1 3
2. 2 7 4 6
3. 2 4 4 6
4. 1 7 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₃H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-3]
1. 1 3 3 4
2. 2 10 4 6
3. 1 5 3 4
4. 2 5 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₄H_10(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-4]
1. 1 13 8 4
2. 2 7 4 10
3. 1 5 3 4
4. 2 13 8 10
Which four quantities a, b, c and d are required to balance the equation ...
aC₅H_12(l) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-5]
1. 1 8 5 6
2. 1 4 4 6
3. 2 4 5 12
4. 2 8 10 12
Which four quantities a, b, c and d are required to balance the equation ...
aC₆H_14(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-6]
1. 2 9 6 14
2. 2 19 12 14
3. 1 9 6 7
4. 1 10 12 7
Which four quantities a, b, c and d are required to balance the equation ...
aC₇H_16(l) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-7]
1. 1 5 7 8
2. 2 12 14 16
3. 1 11 7 8
4. 2 11 14 16
Which four quantities a, b, c and d are required to balance the equation ...
aC₈H_18(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-8]
1. 1 13 8 18
2. 1 13 8 9
3. 2 13 16 18
4. 2 25 16 18
Which four quantities a, b, c and d are required to balance the equation ...
aC₂H_4(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-9]
1. 1 3 2 2
2. 1 2 2 2
3. 2 3 4 4
4. 2 6 4 4
Which four quantities a, b, c and d are required to balance the equation ...
aC₃H_6(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-10]
1. 2 5 6 6
2. 2 9 6 6
3. 1 5 3 3
4. 1 9 3 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₄H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-11]
1. 2 12 8 8
2. 2 6 8 8
3. 1 6 4 4
4. 1 3 4 4
Which four quantities a, b, c and d are required to balance the equation ...
aC₇H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-12]
1. 2 9 4 8
2. 2 10 14 8
3. 1 5 7 4
4. 1 9 7 4
Which three quantities a, b and c are required to balance the equation ...
aFe_(s) + bO_2(g) ==> cFe₃O_4(s) ? [eq-13]
1. 3 2 1
2. 3 4 1
3. 6 4 2
4. 6 2 2
Which three quantities a, b and c are required to balance the equation ...
aLi_(s) + bO_2(g) ==> cLi₂O_(s) ? [eq-14]
1. 2 1 2
2. 4 1 2
3. 4 2 1
4. 2 2 1
Which three quantities a, b and c are required to balance the equation ...
aAl_(s) + bO_2(g) ==> cAl₂O_3(s) ? [eq-15]
1. 1 3 2
2. 4 6 4
3. 4 3 2
4. 2 3 2
Which three quantities a, b and c are required to balance the equation ...
aMg_(s) + bO_2(g) ==> cMgO_(s) ? [eq-16]
1. 1 1 2
2. 4 2 2
3. 2 1 1
4. 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aZn_(s) + bHCl_(aq) ==> cZnCl_2(aq) + dH_2(g) ? [eq-17]
1. 1 2 1 1
2. 2 2 2 1
3. 2 1 1 2
4. 1 1 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe_(s) + bH₂SO_4(aq) ==> cFeSO_4(aq) + dH_2(g) ? [eq-18]
1. 1 1 1 2
2. 1 1 1 1
3. 2 2 2 1
4. 2 1 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bHCl_(aq) ==> cAlCl_3(aq) + dH_2(g) ? [eq-19]
1. 1 6 3 2
2. 2 3 2 3
3. 2 6 2 3
4. 1 3 3 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bH₂SO_4(aq) ==> cAl₂(SO₄)_3(aq) + dH_2(g) ? [eq-20]
1. 1 3 1 3
2. 2 3 2 3
3. 1 2 2 2
4. 2 3 1 3
Which four quantities a, b, c and d are required to balance the equation ...
aNa_(s) + bH₂O_(l) ==> cNaOH_(aq) + dH_2(g) ? [eq-21]
1. 2 2 2 1
2. 2 1 2 1
3. 1 2 1 2
4. 1 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCa_(s) + bH₂O_(l) ==> cCa(OH)_2(aq) + dH_2(g) ? [eq-22]
1. 2 2 2 1
2. 1 2 1 1
3. 1 2 1 2
4. 2 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe_(s) + bH₂O_(g) ==> cFe₃O_4(s) + dH_2(g) ? [eq-23]
1. 3 4 1 2
2. 2 3 1 4
3. 3 4 1 4
4. 2 3 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bH₂O_(g) ==> cAl₂O_3(s) + dH_2(g) ? [eq-24]
1. 3 4 1 6
2. 1 3 1 3
3. 2 4 2 6
4. 2 3 1 3
Which four quantities a, b, c and d are required to balance the equation ...
aMg_(s) + bCuSO_4(aq) ==> cMgSO_4(aq) + dCu_(s) ? [eq-25]
1. 1 1 1 1
2. 2 1 2 2
3. 1 2 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCu_(s) + bAgNO_3(aq) ==> cCu(NO₃)_2(aq) + dAg_(s) ? [eq-26]
1. 1 1 2 1
2. 1 2 1 2
3. 2 2 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aZn_(s) + bFe₂(SO₄)_3(aq) ==> cZnSO_4(aq) + dFe_(s) ? [eq-27]
1. 3 2 6 2
2. 3 1 3 3
3. 3 1 3 2
4. 2 2 6 3
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bFe₂O_3(s)) ==> cAl₂O_3(s) + dFe_(s) ? [eq-28]
1. 1 2 2 1
2. 3 1 1 3
3. 2 3 2 3
4. 2 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCl_2(aq) + bKBr_(aq) ==> cKCl_(aq) + dBr_2(aq) ? [eq-29]
1. 1 2 2 1
2. 2 1 1 1
3. 1 1 2 2
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aBr_2(aq) + bNaI_(aq) ==> cNaBr_(aq) + dI_2(aq) ? [eq-30]
1. 1 2 1 2
2. 1 2 2 1
3. 1 1 2 2
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCl_2(aq) + bCaI_2(aq) ==> cCaCl_2(aq) + dI_2(s) ? [eq-31]
1. 2 1 2 1
2. 1 2 2 2
3. 1 1 1 1
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aAlBr_3(aq) + bCl_2(aq) ==> cAlCl_3(aq) + dBr_2(s) ? [eq-32]
1. 1 3 2 2
2. 1 3 1 3
3. 3 2 2 2
4. 2 3 2 3
Which five quantities a, b, c, d and e are required to balance the equation ...
aCaCO_3(s) + bHCl_(aq) ==> cCaCl_2(aq) + dH₂O_(l) + eCO_2(g) ? [eq-33]
1. 1 2 1 1 1
2. 2 2 1 2 1
3. 1 1 1 1 1
4. 2 1 2 2 2
Which five quantities a, b, c, d and e are required to balance the equation ...
aNa₂CO_3(s) + bHCl_(aq) ==> cNaCl_(aq) + dH₂O_(l) + eCO_2(g) ? [eq-34]
1. 1 4 4 2 2
2. 1 2 2 1 1
3. 2 2 4 2 2
4. 2 2 2 1 1
Which five quantities a, b, c, d and e are required to balance the equation ...
aTl₂(CO₃)_3(s) + bHCl_(aq) ==> cTlCl_3(aq) + dH₂O_(l) + eCO_2(g) ? [eq-35]
1. 2 6 4 3 6
2. 1 3 2 6 2
3. 1 6 2 3 3
4. 2 3 4 3 6
Which five quantities a, b, c, d and e are required to balance the equation ...
aTl₂(CO₃)_3(s) + bH₂SO_4(aq) ==> cTl₂(SO₄)_3(aq) + dH₂O_(l) + eCO_2(g) ? [eq-36]
1. 2 6 4 3 6
2. 1 3 2 6 6
3. 1 6 2 6 3
4. 1 3 1 3 3
Which three quantities a, b and c are required to balance the equation ...
aNa_(s) + bCl_2(g) ==> cNaCl_(s) ? [eq-37]
1. 2 1 2
2. 1 1 1
3. 1 2 1
4. 2 1 1
Which three quantities a, b and c are required to balance the equation ...
aAl_(s) + bCl_2(g) ==> cAlCl_3(s) ? [eq-38]
1. 1 3 1
2. 2 3 2
3. 2 2 3
4. 1 3 2
Which three quantities a, b and c are required to balance the equation ...
aCa_(s) + bCl_2(g) ==> cCaCl_2(s) ? [eq-39]
1. 1 2 1
2. 1 1 2
3. 1 1 1
4. 2 2 1
Which three quantities a, b and c are required to balance the equation ...
aP_(s) + bCl_2(g) ==> cPCl_5(s) ? [eq-40]
1. 1 5 1
2. 1 5 2
3. 2 5 4
4. 2 5 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe₂O_3(s) + bCO_(g) ==> cFe_(l) + dCO_2(g) ? eq-41]
1. 1 3 2 3
2. 1 6 2 6
3. 2 6 4 3
4. 2 3 4 6
Which four quantities a, b, c and d are required to balance the equation ...
aCuO_(s) + bH_2(g) ==> cCu_(l) + dH₂O_(g) ? [eq-42]
1. 2 1 1 1
2. 1 1 1 1
3. 1 2 2 1
4. 2 1 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCuO_(s) + bC_(s) ==> cCu_(s) + dCO_2(g) ? [eq-43]
1. 1 2 1 2
2. 2 2 2 1
3. 2 1 2 1
4. 1 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe₃O_4(s) + bC_(s) ==> cFe_(l) + dCO_2(g) ? [eq-44]
1. 2 1 3 2
2. 1 3 2 1
3. 2 1 2 1
4. 1 2 3 2
Which four quantities a, b, c and d are required to balance the equation ...
aNaOH_(aq) + bHCl_(aq) ==> cNaCl_(aq) + dH₂O_(l) ? [eq-45]
1. 1 1 1 1
2. 1 2 2 1
3. 2 1 1 2
4. 1 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCa(OH)_2(aq) + bHCl_(aq) ==> cCaCl_2(aq) + dH₂O_(l) ? [eq-46]
1. 1 2 1 1
2. 1 2 1 2
3. 2 1 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aAl(OH)_3(s) + bHCl_(aq) ==> cAlCl_3(aq) + dH₂O_(l) ? [eq-47]
1. 2 6 2 3
2. 1 6 2 6
3. 1 3 1 3
4. 2 3 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aFe₂O_3(s) + bHCl_(aq) ==> cFeCl_3(aq) + dH₂O_(l) ? [eq-48]
1. 2 6 2 3
2. 1 6 2 6
3. 1 3 1 3
4. 1 6 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aMgO_(s) + bHCl_(aq) ==> cMgCl_2(aq) + dH₂O_(l) ? [eq-49]
1. 1 2 1 1
2. 1 1 1 1
3. 2 2 1 2
4. 1 4 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aMg(OH)_2(s) + bH₂SO_4(aq) ==> cMgSO_4(aq) + dH₂O_(l) ? [eq-50]
1. 1 2 1 1
2. 1 1 1 2
3. 2 2 1 2
4. 1 4 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aLi₂O_(s) + bHCl_(aq) ==> cLiCl_(aq) + dH₂O_(l) ? [eq-51]
1. 1 2 1 1
2. 1 1 1 1
3. 1 2 2 1
4. 1 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aKOH_(aq) + bH₂SO_4(aq) ==> cK₂SO_4(aq) + dH₂O_(l) ? [eq-52]
1. 1 2 1 1
2. 1 1 1 1
3. 2 2 1 2
4. 2 1 1 2

AQA GCSE (9-1) CHEMISTRY QUIZ on TOPIC 3 "QUANTITATIVE CHEMISTRY" (AQA science trilogy chemistry)

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