Name: _______________________________________________
IAL Edexcel Chemistry
Topic 1 Formulae, Equations and Amount of
Substance
Date:
Time:
Total marks available:
Total marks achieved: ______
AK Powell-Young
Questions
Q1.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
A sample of seawater contains 3.54% sodium chloride by mass.
What is the concentration of sodium chloride in parts per million?
A
3.54 × 10–6
B
3.54 × 10–4
C
3.54 × 104
D
3.54 × 106
(Total for question = 1 mark)
Q2.
Consider the following data.
What is the relationship between a, b, c and d?
A
B
C
D
a=b+c−d
a=d−b−c
a=b−c−d
a=d+c−b
(Total for question = 1 mark)
Q3.
The value of the Avogadro constant is equal to the number of
(1)
A
B
C
D
grams of carbon in one mole of carbon.
atoms in one mole of oxygen gas.
atoms in one mole of helium gas.
ions in one mole of sodium chloride.
(Total for question = 1 mark)
Q4.
Bioethanol can be made by the fermentation of glucose.
The atom economy by mass for the production of ethanol in this reaction is
(1)
A
B
C
D
67%.
51%.
50%.
40%.
(Total for question = 1 mark)
Q5.
A compound has the composition by mass of 54.5% C, 9.1% H and 36.4% O. What is its empirical
formula?
A
C2H2O
B
C2H4O
C
C4H9O
D
C6HO4
(Total for question = 1 mark)
Q6.
Sodium hydrogencarbonate decomposes on heating.
2NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(l)
What is the maximum volume of carbon dioxide, in dm3, which could be obtained by heating 0.25 mol
sodium hydrogencarbonate?
The gas volume is measured at room temperature and pressure when the molar volume of a gas = 24
dm3 mol–1.
A
3
B
6
C
12
D
24
(Total for question = 1 mark)
Q7.
50 cm3 of hydrogen is mixed with 25 cm3 of chlorine. The gases react as shown in the equation below.
H2(g) + Cl2(g) → 2HCl(g)
What is the total volume of gas present at the end of the reaction?
[All gas volumes are measured at the same temperature and pressure.]
A
75 cm3
B
100 cm3
C
125 cm3
D
150 cm3
(Total for question = 1 mark)
Q8.
Which of the following gas samples has the same volume as 7.0 g of carbon monoxide?
All volumes are measured at the same temperature and pressure.
A
B
C
1.0 g of hydrogen
3.5 g of nitrogen
10.0 g of argon
D
35.5 g of chlorine
(Total for question = 1 mark)
Q9.
How many moles of ions are present in 30 cm3 of 0.025 mol dm–3 barium hydroxide solution,
Ba(OH)2(aq)?
A
B
C
D
0.00075
0.00150
0.00225
0.00450
(Total for question = 1 mark)
Q10.
Which of the following aqueous solutions contains the greatest number of negative ions?
A
B
C
D
500 cm3 of 0.10 mol dm−3 Na2SO4(aq)
250 cm3 of 0.12 mol dm−3 BaCl2(aq)
250 cm3 of 0.15 mol dm−3 KI(aq)
500 cm3 of 0.10 mol dm−3 Zn(NO3)2(aq)
(Total for question = 1 mark)
Q11.
In the synthesis of ammonia, 56.0 g nitrogen was reacted with excess hydrogen.
N2(g) + 3H2(g) → 2NH3(g)
The mass of ammonia produced was 6.00 g.
What is the percentage yield of ammonia?
A
5.66
B
8.82
C
9.10
D
10.7
(Total for question = 1 mark)
Q12.
Calculate the empirical formula of the compound with the percentage composition by mass:
Li = 17.9%; P = 26.8%; O = 55.3%
Molar masses / g mol–1
Li = 6.9, P = 31.0, O = 16.0
(1)
A
Li2P3O6
B
Li3PO3
C
LiPO3
D
Li3PO4
(Total for question = 1 mark)
Q13.
In an experiment carried out at 200°C and 1 atm pressure, 20 cm3 of ammonia gas reacted with an
excess of heated copper(II) oxide.
If all measurements were made at 200°C and 1 atm pressure, what would be the total volume, in cm3, of
gaseous products?
A
B
C
D
10
20
30
40
(Total for question = 1 mark)
Q14.
How many electrons are in 10.1 g of neon?
[Avogadro constant = 6.0 × 1023 mol−1]
(1)
A
B
C
D
6.0 × 10
3.0 × 1024
6.0 × 1023
3.0 × 1023
24
(Total for question = 1 mark)
Q15.
What is the concentration, in mol dm–3, of a solution of 10.6 g of sodium carbonate, Na2CO3, in 250 cm3 of
solution?
A
0.40
B
0.25
C
0.10
D
0.025
(Total for question = 1 marks)
Q16.
In which of the following pairs does each gas occupy the same volume?
All volumes are measured at the same temperature and pressure.
A
2 g of hydrogen and 14 g of nitrogen.
B
32 g of methane and 88 g of carbon dioxide.
C
Calcium carbonate is in excess by 0.01 mol.
D
Nitric acid is in excess by 0.03 mol.
(Total for question = 1 mark)
Q17.
Consider the reaction below.
2NO(g) + O2(g) → 2NO2(g)
What is the maximum volume, in dm3, of nitrogen dioxide that could be obtained in the reaction occurring
when 1 dm3 of nitrogen monoxide is mixed with 2 dm3 of oxygen, under suitable conditions?
All measurements are made at the same temperature and pressure.
A
1
B
2
C
3
D
4
(Total for question = 1 mark)
Q18.
When 1.270 g of copper (Ar = 63.5) is added to excess silver nitrate solution, 4.316 g of silver (Ar = 107.9)
forms.
The ionic equation for the reaction is:
A
B
C
D
Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)
2Cu(s) + Ag2+(aq) → 2Cu+(aq) + Ag(s)
Cu(s) + Ag2+(aq) → Cu2+(aq) + Ag(s)
Cu(s) + Ag+(aq) → Cu+(aq) + Ag(s)
(Total for question = 1 mark)
Q19.
Sea water contains 2.7 mg of sulfate ions per kilogram.
What is the concentration of sulfate ions in parts per million by mass?
(1)
A
2.7 × 10–6
B
2.7 × 10–3
C
2.7
D
2.7 × 103
(Total for question = 1 mark)
Q20.
What is the empirical formula of the oxide formed when 2.6 g of chromium produces 3.8 g of chromium
oxide?
Molar masses / g mol–1 Cr = 52.0, O = 16.0
(1)
A
CrO
B
CrO2
C
Cr2O3
D
Cr3O4
(Total for question = 1 mark)
Q21.
The empirical formula of poly(ethene) is
A
CH
B
CH2
C
C2H4
D
CnH2n
(Total for question = 1 mark)
Q22.
Alstonite is a rare salt with the formula, BaCa(CO3)2. It reacts with hydrochloric acid.
Data:
molar mass of alstonite = 297.4 g mol−1
L = 6.02 × 1023 mol−1
(a) The percentage by mass of oxygen in alstonite is
(1)
A
B
C
D
16.1%
26.9%
32.3%
34.3%
(b) What is the total number of ions in one mole of alstonite?
(1)
A
B
C
D
6.02 × 1023
1.20 × 1024
1.81 × 1024
2.41 × 1024
(c) What is the number of moles of hydrochloric acid required for complete reaction with one mole of
alstonite?
(1)
A
B
C
D
one
two
three
four
(Total for question = 3 marks)
Q23.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
How many atoms are there in 120 cm3 of ammonia gas at room temperature and pressure (r.t.p.)?
[Molar volume of gas at r.t.p. = 24 000 cm3 mol–1 Avogadro constant = 6.0 × 1023 mol–1]
A
B
C
D
3.0 × 1021
1.2 × 1022
1.5 × 1022
1.2 × 1025
(Total for question = 1 mark)
Q24.
Answer the question with a cross in the box you think is correct (
). If you change your mind
about an answer, put a line through the box (
( ).
) and then mark your new answer with a cross
A sample of blood plasma contains 3.10 mg of sodium ions in 1 cm3.
The concentration, in mol dm–3, of sodium ions in the plasma is
A
B
C
D
1.35 × 10–1
2.82 × 10–1
1.35 × 10–4
2.82 × 10–4
(Total for question = 1 mark)
Q25.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
A compound contains 31.25% Ca, 18.75% C and 50.00% O.
Its empirical formula is
A
CaC2O4
B
Ca2CO3
C
Ca2CO2
D
CaCO3
(Total for question = 1 mark)
Q26.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
The European Union limit for nitrogen dioxide in the atmosphere is 0.0209 cm3 in 1 m3.
In units of parts per million (ppm) this is
A
B
C
D
2.09 × 10–5
2.09 × 10–2
20.9
2.09 × 104
(Total for question = 1 mark)
Q27.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
Hydrogen is manufactured using the reaction
CH4 + H2O → CO + 3H2
The percentage yield of hydrogen in this process is 90%.
The mass of hydrogen, in tonnes, which can be produced from 160 tonnes of methane is
A
27
B
54
C
60
D
67
(Total for question = 1 mark)
Q28.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
When 0.127 g of copper is added to excess silver nitrate solution, the following reaction occurs.
Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)
What mass of silver is formed?
[Molar masses / g mol–1: Cu = 63.5 Ag = 107.9]
A
B
C
D
0.216 g
0.254 g
0.432 g
0.863 g
(Total for question = 1 mark)
Q29.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
Aluminium reacts with hydrochloric acid.
2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)
What is the maximum volume of hydrogen at room temperature and pressure (r.t.p.)
that can be formed from 0.135 g of aluminium?
[Molar volume of gas at r.t.p. = 24 000 cm3 mol–1 Molar mass Al = 27.0 g mol–1]
A
B
C
D
60 cm3
80 cm3
120 cm3
180 cm3
(Total for question = 1 mark)
Q30.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
Silicon dioxide reacts with hydrogen fluoride to form water and a compound with the formula H2SiF6.
SiO2 + .................... HF → H2SiF6 + .................... H2O
The mole ratio of HF to H2O in the balanced equation is
A
1:2
B
3:1
C
2:1
D
6:1
(Total for question = 1 mark)
Q31.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
The Avogadro constant is 6.0 × 1023 mol−1.
The number of atoms in 15 g of nitrogen monoxide, NO, is
A
3.0 × 1023
B
6.0 × 1023
C
2.4 × 1024
D
9.0 × 1024
(Total for question = 1 mark)
Q32.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
Phosphoric(V) acid, H3PO4, can be made from phosphorus in two stages.
P4 + 5O2 → P4O10
P4O10 + 6H2O → 4H3PO4
Data
The percentage atom economy, by mass, for the production of phosphoric(V) acid from phosphorus is
A
58.0
B
69.0
C
72.4
D
100
(Total for question = 1 mark)
Q33.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
The reaction of magnesium chloride with silver nitrate gives a precipitate of silver chloride.
MgCl2(aq) + 2AgNO3(aq) → Mg(NO3)2(aq) + 2AgCl(s)
A solution containing 0.001 mol of magnesium chloride reacts with excess silver nitrate.
What is the mass of the precipitate formed?
[Molar mass / g mol–1: AgCl = 143.4]
A
B
C
D
0.072 g
0.143 g
0.287 g
0.574 g
(Total for question = 1 mark)
Q34.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
Dilute sulfuric acid is mixed with a solution of barium chloride.
The reaction that occurs is
A
B
C
D
displacement.
neutralisation.
precipitation.
redox.
(Total for question = 1 mark)
Q35.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
(
).
The solution containing the greatest number of chloride ions is
A
10 cm3 of 1.00 × 10−2 mol dm−3 AlCl3
B
20 cm3 of 1.50 × 10−2 mol dm−3 MgCl2
C
30 cm3 of 1.50 × 10−2 mol dm−3 HCl
D
10 cm3 of 2.50 × 10−2 mol dm−3 CaCl2
(Total for question = 1 mark)
Q36.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
150 cm3 of ethane is mixed with 700 cm3 of oxygen. The equation for the reaction is
C2H6(g) + 31⁄2O2(g) → 2CO2(g) + 3H2O(l)
What is the total volume of gas when the reaction is complete?
All gas volumes are measured at the same temperature and pressure.
A
B
C
D
150 cm3
300 cm3
325 cm3
475 cm3
(Total for question = 1 mark)
Q37.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
Nitrogen monoxide reacts with oxygen to form nitrogen dioxide.
2NO(g) + O2(g) → 2NO2(g)
200 cm3 of nitrogen monoxide is mixed with 350 cm3 of oxygen.
What is the total volume, in cm3, of the gaseous mixture when the reaction is complete?
All volumes are measured at the same temperature and pressure.
A
200
B
350
C
450
D
550
(Total for question = 1 mark)
Q38.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
For safety reasons, the concentration of lead in paint should not exceed 600 parts per million (ppm) by
mass.
Therefore, the mass of lead in one kilogram of paint should not exceed
A
0.06 g
B
0.60 g
C
6.0 g
D
60 g
(Total for question = 1 mark)
Q39.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
10 cm3 of a 1.00 × 10−2 mol dm−3 solution needs to be diluted to make the concentration 5.00 × 10−4 mol
dm−3.
What volume of water, in cm3, should be added?
A
20
B
40
C
190
D
200
(Total for question = 1 mark)
Q40.
Solutions of barium chloride and silver nitrate are mixed together. The reaction that takes place is an
example of
A
B
C
D
displacement.
neutralization.
oxidation.
precipitation.
(Total for question = 1 mark)
Q41.
10 g of magnesium is added to 1 dm3 of 1 mol dm−3 copper(II) sulfate solution and the mixture is stirred
until no further reaction occurs.
Which of the following is a result of this reaction?
A
B
C
D
The resulting solution is colourless.
10 g of copper is displaced.
63.5 g of copper is displaced.
All the magnesium reacts.
(Total for question = 1 mark)
Q42.
The ionic equation for the reaction between hydrochloric acid and aqueous sodium hydroxide is
A
B
C
D
H+(aq) + OH−(aq) → H2O(l)
Cl−(aq) + Na+(aq) → NaCl(aq)
H+(aq) + Cl−(aq) + Na+(aq) + OH−(aq) → Cl−(aq) + Na+(aq) + H2O(l)
H+(aq) + Cl−(aq) + Na+(aq) + OH−(aq) → NaCl(aq) + H2O(l)
(Total for question = 1 mark)
Q43.
Calcium chloride can be prepared by reacting calcium carbonate with dilute hydrochloric acid.
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)
(a) The ionic equation for the reaction is
(1)
(b) An excess of calcium carbonate is used in the preparation. The sequence of processes needed to
obtain crystals of calcium chloride from the reaction mixture is
(1)
A
filtering, concentrating the solution, slowly evaporating.
B
filtering, slowly evaporating, distilling.
C
concentrating the solution, filtering, distilling.
D
concentrating the solution, slowly evaporating, filtering.
(c) The excess calcium carbonate was added to 100 cm3 of 2.00 mol dm–3 hydrochloric acid. The mass of
calcium chloride crystals obtained was 10.4 g.
Molar mass of calcium chloride crystals, CaCl2.2H2O = 147 g mol–1.
The percentage yield, by mass, of calcium chloride crystals is
(1)
A
71.2
B
70.7
C
35.4
D
17.7
(Total for question = 3 marks)
Q44.
How many ions are in 284 g of sodium sulfate, Na2SO4?
Avogadro constant = 6.0 × 1023 mol–1
Molar mass of sodium sulfate = 142 g mol–1
(1)
A
1.2 × 1024
B
2.4 × 1024
C
3.6 × 1024
D
8.4 × 1024
(Total for question = 1 mark)
Q45.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
The concentration of potassium ions in human blood is in the range 3.5 × 10–3 to 5.0 × 10–3 mol dm–3.
An average person has 5 dm3 of blood.
What is the minimum mass of potassium ions in the blood of an average person?
[Molar mass of potassium = 39.1 g mol–1]
A
0.137 g
B
0.684 g
C
0.978 g
D
684.0 g
(Total for question = 1 mark)
Q46.
Consider the reaction
2SO2(g) + O2(g) → 2SO3(g)
What is the maximum volume, in dm3, of sulfur trioxide that could be obtained when 0.5 dm3 of sulfur
dioxide is mixed with 1 dm3 of oxygen, under suitable conditions?
All measurements are made at the same temperature and pressure.
(1)
A
0.5
B
1.5
C
2.0
D
2.5
(Total for question = 1 mark)
Q47.
Answer the question with a cross in the box you think is correct ( ). If you change your mind
about an answer, put a line through the box ( ) and then mark your new answer with a cross
( ).
What is the number of atoms present in 3.06 dm3 of carbon dioxide, at 373 K?
[Molar volume of a gas at 373 K is 30.6 dm3 mol–1, Avogadro constant = 6.0 × 1023 mol–1]
A
1.8 × 1022
B
6.0 × 1022
C
1.8 × 1023
D
6.0 × 1023
(Total for question = 1 mark)
Q48.
The percentage by mass of hydrogen in heptane, C7H16, is
(1)
A
B
C
D
84.0
69.6
19.0
16.0
(Total for question = 1 mark)
Q49.
Phenol, C6H5OH, is converted into trichlorophenol (known as TCP), C6H2Cl3OH, according to the equation
below.
C6H5OH + 3Cl2 → C6H2Cl3OH + 3HCl
If 50.0 g of phenol produces 97.6 g of TCP, what is the percentage yield of the TCP?
[Molar masses: phenol = 94 g mol−1; TCP = 197.5 g mol−1]
A
47.6%
B
49.4%
C
51.2%
D
92.9%
(Total for question = 1 mark)
Q50.
Phosphorus reacts with iodine to produce phosphorus(III) iodide:
P4 + 6I2 → 4PI3
What is the minimum mass of iodine required to produce 1 kg of phosphorus(III) iodide when the
phosphorus is in excess?
Data: molar mass of phosphorus(III) iodide = 411.7 g mol−1
A
B
C
D
0.616 kg
0.925 kg
2.466 kg
3.700 kg
(Total for question = 1 mark)
Q51.
Sulfur reacts with chlorine to produce disulfur dichloride:
S8 + 4Cl2 → 4S2Cl2
What is the maximum mass of disulfur dichloride that could be produced from the reaction of 0.100 mol of
sulfur, S8, with 0.394 mol of chlorine?
Data: molar mass of disulfur dichloride = 135.2 g mol−1
A
B
C
D
13.32 g
13.52 g
53.27 g
54.08 g
(Total for question = 1 mark)
Q52.
Ammonia is manufactured from hydrogen and nitrogen in the Haber process.
If 60 tonnes of hydrogen produces 80 tonnes of ammonia, what is the percentage yield in the reaction?
A
× 100%
B
× 100%
C
× 100%
D
× 100%
(Total for question = 1 mark)
Q53.
A typical adult human has 5.0 dm3 of blood, which contains a total of 35 cm3 of white blood cells.
What is the concentration of white blood cells, in parts per million, by volume?
(1)
A
B
C
D
142.9
7000
7 000 000
142 900 000
(Total for question = 1 mark)
Q54.
The process with the highest atom economy is the production of
A
B
C
D
propene by cracking eicosane, C20H42.
1-chloropropane from propane and chlorine.
cyclohexene by reforming hexane.
poly(propene) by polymerising propene.
(Total for question = 1 mark)
Q55.
What type of reaction occurs when dilute sulfuric acid reacts with aqueous barium chloride?
(1)
A
B
C
D
Displacement
Neutralisation
Oxidation
Precipitation
(Total for question = 1 mark)
Q56.
The Avogadro constant is numerically equal to the number of
A
B
C
D
ions in 1 mol of sodium chloride, NaCl
atoms in 1 mol of hydrogen gas, H2
electrons in 1 mol of helium gas, He
molecules in 1 mol of oxygen gas, O2
(Total for question = 1 mark)
Q57.
The Avogadro constant is equal to the number of
A
grams of an element which contains 6.02 × 1023 atoms of that element.
B
atoms contained in one mole of any element.
C
atoms contained in one mole of any monatomic element.
D
particles (atoms, ions or molecules) required to make one gram of a substance.
(Total for question = 1 mark)
Q58.
In an experiment, 3.425 g of lead oxide was reduced to form 3.105 g of lead.
The empirical formula of the lead oxide is
A
PbO
B
Pb3O2
C
Pb3O4
D
Pb4O3
(Total for question = 1 mark)
Q59.
A hydrocarbon contains, by mass, 82.7% carbon and 17.3% hydrogen.
The molecular formula of the hydrocarbon is
A
CH3
B
C2H6
C
C2H5
D
C4H10
(Total for question = 1 mark)
Q60.
Which of the following contains one mole of neutrons?
A
1 g of H
B
1 g of
C
2 g of
Mg
D
2 g of
Ne
C
(Total for question = 1 mark)
Q61.
2000 g of a solution contains 0.015 g of solute.
In the solution, the concentration of the solute in parts per million (ppm) is
A
3.0
B
7.5
C
30
D
75
(Total for question = 1 marks)
Q62.
A solution contains 33 ppm of solute. The mass of solute dissolved in 1 kg of this solution is
A
33 g
B
0.33 g
C
0.033 g
D
0.000033 g
(Total for question = 1 mark)
Q63.
Cold water fish require a minimum of 8 parts per million by mass (ppm) of oxygen dissolved in water.
The minimum mass of oxygen required in 1 kg of water is
A
8 × 10–6 g
B
8 × 10–3 g
C
8 × 10–2 g
D
8 × 10–1 g
(Total for question = 1 mark)
Q64.
Calcium carbonate reacts with dilute nitric acid as follows:
CaCO3(s) + 2HNO3(aq) → Ca(NO3)2(aq) + H2O(l) + CO2(g)
0.05 mol of calcium carbonate was added to a solution containing 0.08 mol of nitric acid.
Which of the following statements is true?
A
0.05 mol of carbon dioxide is produced.
B
0.08 mol of calcium nitrate is produced.
C
Calcium carbonate is in excess by 0.01 mol.
D
Nitric acid is in excess by 0.03 mol.
(Total for question = 1 mark)
Q65.
If the price of one tonne (1000 kg) of sulfur, S, is £160, what is the cost (to the nearest pound) of the
sulfur needed to make one tonne of sulfuric acid, H2SO4?
A
£52
B
£98
C
£160
D
£490
(Total for question = 1 mark)
Q66.
Calculate the total number of atoms in 8.5 g of CH2Cl2.
DATA:
Molar mass of CH2Cl2 = 85 g mol–1.
Avogadro constant = 6.0 × 1023 mol–1
A
1.8 × 1023
B
2.4 × 1023
C
3.0 × 1023
D
3.0 × 1024
(Total for question = 1 mark)
Q67.
Magnesium chloride crystals were prepared using the following reaction.
2HCl(aq) + MgO(s) → MgCl2(aq) + H2O(l)
(a) The ionic equation for this reaction is
(1)
A
2Cl–(aq) + Mg2+(s) → MgCl2(aq)
B
2Cl–(aq) + MgO(s) → MgCl2(aq) + O2–(l)
C
2H+(aq) + 2Cl–(aq) + MgO(s)→ Mg2+(Cl–)2(aq) + H2O(l)
D
2H+(aq) + MgO(s) → Mg2+(aq) + H2O(l)
(b) The amount of hydrochloric acid used was 0.10 mol. Which of the following solutions of hydrochloric
acid contains this amount of HCl?
(1)
A
100 cm3 of 0.10 mol dm–3
B
40 cm3 of 0.25 mol dm–3
C
25 cm3 of 0.40 mol dm–3
D
20 cm3 of 5.00 mol dm–3
(c) An excess of magnesium oxide was reacted with the 0.10 mol of hydrochloric acid.
Which of the following is the smallest mass which would provide an excess of magnesium oxide?
Molar mass of MgO = 40.3 g mol–1
(1)
A
1.50 g
B
2.50 g
C
3.00 g
D
5.00 g
(d) What is the first step in obtaining pure hydrated crystals of magnesium chloride from the resulting
reaction mixture?
(1)
A
Heating the mixture to concentrate it.
B
Allowing the mixture to evaporate slowly.
C
Filtering the mixture.
D
Distilling the mixture.
(e) Use the data below to calculate the number of moles of water of crystallization in each mole of
hydrated magnesium chloride.
(1)
A
2
B
4
C
6
D
8
(Total for question = 5 marks)
Q68.
(a) The relative atomic masses of elements can be determined using a mass spectrometer.
(i) Define the term relative atomic mass.
(3)
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(ii) Describe fully how positive ions are formed from gaseous atoms in a mass spectrometer.
(2)
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(iii) The following data were obtained from the mass spectrum of a sample of strontium.
Calculate the relative atomic mass of strontium in this sample.
Give your answer to three significant figures.
(2)
(b) In which block of the Periodic Table is strontium found?
(1)
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(c) Draw the dot and cross diagram for strontium chloride.
Show outer electrons only.
(2)
(d) A solution of strontium nitrate was prepared from strontium oxide and dilute nitric acid.
Write the equation for this reaction, including state symbols.
(2)
(e) A compound of strontium contains 49.9% strontium, 13.7% carbon and 36.4% oxygen, by mass.
Calculate the empirical formula for this compound.
[Use relative atomic masses: Sr = 87.6, C = 12.0, O = 16.0]
(3)
(Total for question = 15 marks)