Download C. 3.5 g

F.5 Revision - Mole Calculation(Ch 13,20,21,22,29)
5. Which of the following isotopes is used nowadays to compare atomic masses?
I. Multiple Choice
A.
Carbon-14
Choose the best option and write the correct answer in the box provided.
B.
Carbon-12
1. 1 mole of calcium chloride contains
C.
Carbon-13
D.
Hydrogen-1
A.
1 mole of calcium chloride molecules
B.
6.02  1023 calcium atoms and 2 x 6.02  1023 chlorine atoms
C.
1/2  6.02  10 calcium ions and 6.02  10 chloride ions
D.
6.02  1023 calcium ions and 2  6.02  1023 chloride ions
23
□
23
6. What is the molar mass of CCl4? (Relative atomic masses: C = 12.0; Cl = 35.5)
A.
1 mol
2. What is the relative molecular mass of carbon dioxide? (Relative atomic masses: C =
B.
1 g mol1
12.0; O = 16.0)
C.
154 mol
A.
28
D.
154 g mol1
B.
44
C.
60
D.
74
□
7. Which of the following substances contains the least number of ions?
A.
0.7 mole of Na2O
B.
0.9 mole of CaO
3. What is the formula mass of calcium sulphate? (Relative atomic masses: Ca = 40.1; S =
C.
0.5 mole of Al2O3
32.1; O = 16.0)
D.
0.8 mole of MgCl2
□
□
A.
136.2
B.
120.2
C.
88.2
A.
There are 0.4 mole of Al2+ ions and 0.4 mole of O2 ions.
D.
68.1
B.
There are 0.8 mole of Al+ ions and 0.4 mole of O2 ions.
C.
There are 0.8 mole of Al3+ ions and 1.2 moles of O2 ions.
D.
There are 1.2 moles of Al3+ ions and 0.8 mole if O2 ions.
8. Which of the following statements is correct about 0.4 mole aluminium oxide?
□
4. Which of the following is the unit for formula mass?
□
A.
Gram
B.
Mole
9. A mixture of copper(II) sulphate and copper(II) bromide contains 0.3 mole of sulphate
C.
No unit
ions and 0.6 mole of bromide ions. How many moles of copper(II) ions are in the mixture?
D.
Mass unit
□
F.5 Revision – Mole
A.
0.6
B.
0.8
page 1 of 16
C.
0.9
A.
19
D.
1.1
B.
23
C.
27
D.
31
□
10. In electrolysis, how many number of electrons are required to change all iron(III) ions
□
to iron atoms in 0.7 mole of iron(III) oxide?
A.
4.21  1023
14. Which of the following substances has the smallest mass? (Relative atomic masses: H =
B.
1.26  10
1.0; C = 12.0; O = 16.0; K = 39.1; Ca = 40.1; Fe = 55.8; Br = 80.0)
C.
2.28  1024
A.
0.8 mole of CaBr2
D.
2.53  1024
B.
1 mole of C4H10
C.
1.5 moles of Fe2O3
D.
1.9 moles of K
24
□
11. Which of the following statements is correct?
A.
B.
C.
D.
□
1 mole of oxygen gas contains the same number of atoms as 1 mole of neon gas
at room conditions.
15. What is the number of shared electrons in 35.5 g of chlorine gas at room conditions?
1 mole of magnesium contains the same number of atoms as 1 mole of iodine
(Relative atomic mass: Cl = 35.5)
at room conditions.
A.
1.51  1023
1 mole of chlorine gas and 1 mole of bromine gas have the same number of
B.
3.01  1023
molecules and atoms.
C.
6.02  1023
1 mole of sodium has the same mass as 1 mole of potassium.
D.
1.20  1024
□
□
12. What is the mass of 2.3 moles of aluminum oxide? (Relative atomic masses: O = 16.0;
16. How many moles of aluminium ions are present in 17.12 g of aluminium sulphate?
Al = 27.0)
(Relative atomic masses: Al = 27.0; S = 32.1; O = 16.0)
A.
124.8g
A.
0.005
B.
234.6g
B.
0.01
C.
367.5g
C.
0.05
D.
417.4g
D.
0.1
□
□
13. M is a metal in Group I. 0.5 mole of the metal sulphate weighs 71.05g. Find the relative
17. What mass of sulphur contains the same number of atoms as 8.1 g of magnesium?
atomic mass of M. (Relative atomic masses: O = 16.0; S = 32.1)
(Relative atomic masses: Mg = 24.3; S = 32.1;)
F.5 Revision – Mole
page 2 of 16
A.
5.35 g
relative atomic mass of X? (Relative atomic masses: H = 1.0; O = 16.0)
B.
10.70 g
A.
72
C.
16.05 g
B.
86
D.
21.40 g
C.
90
D.
102
□
□
18. Which of the following substances contains the same number of ions as 2.34 g of
sodium chloride? (Relative atomic masses: O = 16.0; Na = 23.0 Mg = 24.3; S = 32.1; Cl =
22. What is the percentage by mass of C in C6H12O6? (Relative atomic masses: C = 12.0; H
35.5; K = 39.1; Ca = 40.1; Zn = 65.4; Br = 80.0)
= 1.0; O = 16.0)
A.
2.984 g of potassium chloride
A.
40%
B.
3.125 g of zinc chloride
B.
25%
C.
3.598 g of calcium sulphate
C.
53%
D.
5.529 g of magnesium bromide
D.
50%
□
□
19. 2.4 g of oxygen contains x atoms at room conditions. How many atoms are present in
23. What is the mass of iron in 15 g of FeSO4˙7H2O? (Relative atomic masses: Fe = 55.8;
12 g of helium? (Relative atomic masses: He = 4.0; O = 16.0)
S = 32.1; O = 16.0; H = 1.0)
A.
5x
A.
0.2 g
B.
10x
B.
3.0 g
C.
20x
C.
6.2 g
D.
30x
D.
20.0 g
□
□
20. What is the percentage by mass of chlorine in 11.8 g of aluminum chloride?
24. The chloride of a metal X has the formula XCl3 and contains 65.6% by mass of Cl. Find
(Relative atomic masses: Al = 27.0; Cl = 35.5)
the relative atomic mass of X. (Relative atomic mass: Cl = 35.5)
A.
47%
A.
12.2
B.
68%
B.
18.6
C.
72%
C.
34.4
D.
80%
D.
55.8
□
21. If 1 mole of XO3 contains the same number of atoms as 72 g of XH4, What is the
F.5 Revision – Mole
□
25. Which of the following is a molecular formula?
page 3 of 16
A.
Mg
equal to 62, what is the molecular formula of Y? (Relative atomic masses: C = 12.0; H =
B.
CH4
1.0; O = 16.0)
C.
NaCl
A.
C2H6O2
D.
NH4Cl
B.
CH3O
C.
CHO
D.
C3H9O3
□
26. Which of the following is the structural formula of a molecule?
+

□
A.
K Cl
B.
O=C=O
30. 20.7 g of lead metal reacts with excess oxygen gas to form lead(II) oxide on strong
C.
CH2O
heating. What is the mass of the solid product formed? (Relative atomic masses: Pb = 207;
D.
CCl4
O =16.0)
□
A.
11.1 g
27. What is the empirical formula for a compound having the following composition by
B.
22.3 g
mass? (Relative atomic masses: Al = 27.0; S = 32.1; O = 16)
C.
33.4 g
D.
44.6 g
15.79% aluminium
28.07% sulphur
56.14% oxygen
□
A.
Al2S3O9
B.
Al2S3O12
31. What mass of zinc oxide is required to obtain 0.8 mole of zinc by carbon reduction?
C.
AlSO4
(Relative atomic masses: Zn = 65.4; O = 16.0; C = 12.0)
D.
Al2SO4
A.
3.256 g
B.
6.512 g
28. What is the empirical formula for a compound having 92.3% by mass of carbon and
C.
32.56 g
7.7% by mass of hydrogen? (Relative atomic masses: H = 1.0; C = 12.0)
D.
65.12 g
□
□
A.
CH2
B.
C2H
32. 3.9 g of potassium reacts with excess water. What is the mass of the gaseous product
C.
C2H2
formed? (Relative atomic masses: K = 39.1; O = 16.0; H=1.0)
D.
CH
A.
0.1 g
B.
0.2 g
29. Complete combustion of 1.86 g of an organic compound Y gave 2.64 g of carbon
C.
1.0 g
dioxide and 1.62 g of water as the only products. If the relative molecular mass of Y is
D.
2.0 g
□
F.5 Revision – Mole
page 4 of 16
□
□
33. To reduce 7.2 g of iron(III) oxide completely, how many grams of carbon is required?
37. Calculate the number of moles of carbon atoms in 4.7g of ethane, C2H6. (Relative
(Relative atomic masses: C = 12.0; O = 16.0; Fe = 55.8;)
atomic mass: H = 1.0; C = 12.0)
A.
0.52 g
A.
0.182
B.
0.81 g
B.
0.283
C.
1.36 g
C.
0.278
D.
2.20 g
D.
0.314
□
□
3
34. What is the number of atoms in one mole of oxygen gas if two moles of ozone, O 3,
38. What is the concentration of aqueous sodium ions in a 500 cm solution containing
contain y atoms?
0.585 g of pure sodium chloride?
A.
2y/3
(Relative atomic masses: Na = 23.0; Cl = 35.5)
B.
y/3
A.
0.01 mol/dm3
C.
y/2
B.
0.02 mol/dm3
D.
y/6
C.
0.03 mol/dm3
D.
0.04 mol/dm3
□
35. Which of the the following statements are about one mole of propane (C 3H8) and one
39. What is the concentration of bromine in a 200 cm3 solution containing 1.598 g of
mole of propene (C3H6) is correct?
bromine?
A.
They have equal masses.
B.
They have the same number of molecules.
A.
0.02 mol/dm3
C.
They have the same number of atoms.
B.
0.04 mol/dm3
D.
They have the same boiling point.
C.
0.05 mol/dm3
D.
0.06 mol/dm3
(Relative atomic masses: Br = 79.9)
□
36. Calculate the mass of two moles of chlorine molecules. (Relative atomic mass of Cl =
40. A sample of a certain concentrated acid has a density of 1.96 gcm3 and contains 95.0%
35.5)
of the acid by mass. What is the concentration (correct to one decimal place) of the acid in
A.
70g
the sample?
B.
71g
(Relative molecular mass of the acid is 100)
C.
84g
A.
17.4 M
D.
142g
B.
18.2 M
F.5 Revision – Mole
□
page 5 of 16
□
C.
18.6 M
D.
19.3 M
D.
□
6.524 g
□
45. Which
of the following cases has different masses of solutes in the two solutions?
41. A 2.0 M potassium chloride solution is prepared by dissolving 37.3 g of potassium
(Relative atomic masses: H = 1.0; C = 12.0; O = 16.0; Na = 23.0; S = 32.1; Cl = 35.5)
chloride in distilled water. What is the volume of the solution formed?
(Relative atomic masses: K = 39.1, Cl = 35.5)
Solution 1
Solution 2
A.
500 cm3 of 0.50 M Na2SO4
100 cm3 of 2.50 M Na2SO4
A.
75.0 cm3
B.
100.0 cm3
B.
0.25 dm3 of 0.15 M Na2CO3
0.05 dm3 of 0.75 M Na2CO3
C.
250.0 cm3
C.
25 cm3 of 0.10 M NaOH
0.05 dm3 of 0.05 M NaOH
D.
400.0 cm3
D.□ 100 cm3 of 0.05 M NaCl
0.025 dm3 of 0.02 M NaCl
3
□
3
42. In an experiment, 20 cm of 0.5 M nitric acid is added slowly into 10 cm of 1 M
potassium hydroxide solution. Which of the following statements about the experiment is
46. Which of the following statements about a 0.50 M MgCl 2 solution is correct?
correct?
A.
The concentration of nitrate ions in the mixture remains unchanged.
B.
The mixture does not conduct electricity at the end of the experiment.
C.
The pH value of the mixture decreases.
D.
The temperature of the mixture decreases.
43. Which of the following concentrations is INCORRECT if 10 g of sodium carbonate
solid is dissolved in water to give 500 cm3 solution?
A.
There are 0.50 M Mg2+ ions and 0.50 M Cl ions.
B.
There are 0.50 M Mg2+ ions and 1.0 M Cl ions.
C.
There are 1.0 M Mg2+ ions and 0.50 M Cl ions.
D. There are 1.0 M Mg2+ ions and 1.0 M Cl ions.
□
47. Which of the following information about the number of moles of ions present in 25
cm3 of 0.20 M ammonium sulphate solution is correct?
(Relative atomic masses: Na = 23.0; C = 12.0; O = 16.0)
Ammonium ion
Sulphate ion
A.
20 g dm3
A.
5 x 103 mol
5 x 103 mol
B.
0.02 g cm-3
B.
5 x 103 mol
1 x 102 mol
C.
0.19 mol dm3
0.24 mol dm3
C.
□
D.
1 x 102 mol
1 x 102 mol
D.
1 x 102 mol
5 x 103 mol
44. What is the mass of solute in 250.0 cm3 of 0.50 M HCl(aq)?
□
□
(Relative atomic masses: H = 1.0; Cl = 35.5)
A.
2.645 g
48. What volume of water has to be added to 250 cm3 of 0.20 M K2CO3 solution to dilute it
B.
4.562 g
to 0.05 M?
C.
5.246 g
F.5 Revision – Mole
A.
250 cm3
page 6 of 16
B.
500 cm3
C.
750 cm3
D.
1000 cm3
Pressure of gas
□
A
B
49. Which of the following reactions is the slowest?
C
D
A.
Neutralization of HCl(aq) and NaOH(aq)
B.
Reaction of potassium and water.
C.
Corrosion of iron.
53. Which of the following shows the correct sequence of results of measuring rate of
D.
Displacement reaction of Mg in CuSO4(aq)
□ between sodium thiosulphate solution and dilute hydrochloric acid? (The diagrams
reaction
50. Which of the following is NOT a unit of chemical reaction rate?
A.
s mol1
B.
cm3 s1
C.
g min1
D.
mol dm3 s1
Time
□
show the top view of the solution in a beaker putting on top of a marked cross.)
A.
B. □
51. When 10.6 g of anhydrous sodium carbonate was added to 200.0 cm3 of 1.0 M
sulphuric acid at room conditions, the reaction stopped in 40 seconds. At the same time,
2400 cm3 of carbon dioxide was produced. Which of the following statements about the
reaction is INCORRECT?
A.
The average rate of decrease in mass of sodium carbonate was 15.9 g min1
B.
The average rate of decrease in concentration of the acid was 0.0125 mol dm3
s1
C.
D.
C.
The average rate of increase in volume of carbon dioxide was 60 cm3 s1
D.
Sodium carbonate and sulphuric acid just reacted completely.
□
□
52. A rate curve is obtained when anhydrous sodium carbonate reacts with dilute
hydrochloric acid. At which point on the rate curve below is the reaction rate highest?
F.5 Revision – Mole
page 7 of 16
D.
54. Which of the following diagrams shows a correct rate curve for chemical reactions?
A.
B.
□
Increase in volume of HCl(aq)
57. Which of the following sets of apparatus could be used to measure the speed of the
reaction between marble chips and dilute nitric acid?
Amount of
Amount of
product in
product in the
the reaction
reaction
(1)
Time
C.
Time
D.
Amount of
Amount of
product in
product in
the reaction
the reaction
graduated tube
dilute nitric acid
marble chips
water
(2)
marble chips
dilute nitric acid
top pan
balance
Time
Time
55. Which of the following is a factor affecting the reaction rate of the following reaction?
□
(3)
Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g)
A.
Concentration of HCl(aq)
B.
Concentration of Mg(s)
C.
Concentration of MgCl2(aq)
D.
Concentration of H2(g)
56. Which of the following CANNOT increase the reaction rate of the following reaction?
CaCO3(s) + 2HCl(aq)  CaCl2(aq) + H2O(l) + CO2(g)
A.
Increase in concentration of HCl(aq)
B.
Increase in temperature of the reaction mixture
C.
Use powdered CaCO3
F.5 Revision – Mole
gas syringe
dilute nitric acid
marble chips
□
A.
(1) only
B.
(2) only
C.
(1) and (3) only
D.
(2) and (3) only
58. When excess dilute nitric acid reacts with magnesium carbonate, the reaction gradually
page 8 of 16
□
becomes slower and finally stops. Which of the following statements correctly explains this
Total volume of carbon dioxide produced
situation?
A.
An insoluble layer of magnesium nitrate is formed.
B.
The magnesium carbonate is gradually used up.
C.
The nitric acid is all used up.
D.
The layer of carbon dioxide bubbles covers the magnesium carbonate.
(i)
(ii)
□
Time
59. The experiment shown in the diagram was set up and the syringe reading was noted at
60.
intervals.
In the graph, curve (i) was obtained when 2 g of marble chips reacted with excess dilute
nitric acid at 20C.
Which of the following changes to the reaction would give curve (ii)?
gas syringe
dilute hydrochloric acid
magnesium carbonate
A.
Using 1.5 g of marble chips
B.
Using 2 g of finely powdered marble
C.
Adding water to dilute the acid
D.
Warming the acid to 30C
A graph of the syringe readings against time was plotted. Which of the following curves
61. When steam is passed through a red-hot magnesium ribbon inside a combustion tube, a
would be obtained?
reaction occurs and the temperature of the magnesium ribbon increases. What does this
indicate?
Syringe
readings
A
B
C
D
Time
A.
The reaction is reversible.
B.
Steam contains impurities.
C.
The reaction is exothermic.
D. Magnesium is an oxidizing agent.
□
62. Hydrogen
peroxide solution is catalytically decomposed by manganese(IV) oxide
according to the following equation:
2H2O2  2H2O + O2
Three experiments were performed using different solutions but a fixed mass of catalyst.
The graph below shows the results.
F.5 Revision – Mole
□
page 9 of 16
□
D.
Total volume of oxygen evolved
Smaller
lower
More concentrated
□
P
64. In the graph, curve P represents the result of the reaction between 2.0 g granulated
Q
magnesium carbonate and excess dilute hydrochloric acid at 40C.
R
Total volume of carbon dioxide produced
P
Time
The solutions used were:
(i)
25 cm3 of 1.0 mol/dm3 hydrogen peroxide
(ii)
50 cm3 of 0.5 mol/dm3 hydrogen peroxide
Q
(iii) 50 cm3 of 1.0 mol/dm3 hydrogen peroxide
Time
Which curves correspond to the three solutions respectively?
Which of the following changes could produce curve Q?
(i)
(ii)
(iii)
A.
2.0 g of powdered magnesium carbonate at 30C.
A.
P
Q
R
B.
2.0 g of granulated magnesium carbonate at 30C.
B.
Q
R
P
C.
1.0 g of granulated magnesium carbonate at 50C.
D.
1.0 g of granulated magnesium carbonate at 30C.
C.
R
Q
P
D.
R
P
Q
65. Which of the following conclusions is INCORRECT according to the following
□ equation. (Relative atomic masses: O = 16.0; S = 32.1; Molar volume of any
chemical
gases at room temperature and pressure = 24 dm3 mol1)
S(s) + O2(g)  SO2(g)
63. A chemical reaction between a metal and an acid is too vigorous to be a safe experiment
for students.
A.
Which set of changes is most likely to make the reaction safer for students?
Size of metal
Temperature
Acid
1 mole of sulphur reacts with 1 mole of oxygen to give 1 mole of sulphur
dioxide
B.
32.1 g of sulphur react with 1 mole of oxygen to give 24 dm 3 of sulphur
dioxide
(the amount is constant)
A.
Smaller
Higher
Less concentrated
B.
Larger
Lower
Less concentrated
C.
Larger
Higher
More concentrated
C.
1 mole of sulphur reacts with 24 dm3 of oxygen to give 64.1 g of sulphur
dioxide
F.5 Revision – Mole
D.
24 dm3 of sulphur reacts with 24 dm3 of oxygen to give 24 dm3 of sulphur
dioxide
page 10 of 16
□
□
A.
30.0 g
66. Which of the following pairs of gases have the same number of atoms at the same
B.
40.0 g
temperature and pressure?
C.
50.0 g
D.
60.0 g
A.
200 cm3 of steam
200 cm3 of ammonia
B.
1 dm3 of carbon dioxide
1 dm3 of sulphur trioxide
C.
100 cm3 of methane
500 cm3 of neon
D.
50 cm3 of hydrogen chloride
50 cm3 of hydrogen sulphide
□
mixture of
Cl2 and H2
sunlight
□
67. When 0.2 g of calcium is treated with excess dilute hydrochloric acid, what volume of
gas at room temperature and pressure will be produced?
(Relative atomic mass: Ca = 40.0; molar volume of gases at r.t.p. is 24 dm3 mol1)
A.
20 cm3
B.
60 cm3
C.
100 cm3
D.
3
water
70.
A 100 cm3 tube is filled with 30 cm3 of chlorine and 70 cm3 of hydrogen. The tube is then
120 cm
□
exposed to sunlight for half an hour and then inverted over water. The volume of gas
remained in the tube will be about
68. When 0.01 mole of metal Y reacts with excess dilute acid, 240 cm3 of hydrogen is
given off at room temperature and pressure. Which of the following is the correct equation
A.
30 cm3
for the reaction?
B.
40 cm3
A.
Y + 2H+  Y2+ + 2H
C.
50 cm3
B.
Y + 2H+  Y2+ + H2
D.
60 cm3
C.
2Y + 2H+  2Y + H2
D.
2Y + 6H+  2Y3+ + 3H2
□
71. If two moles of sulphur dioxide are oxidized to sulphur trioxide by air, what is the
□
minimum volume of air required at room temperature and pressure?
69. If 7.0 g of nitrogen and 15.0 g of gas Y have the same number of moles. What is the
(Assuming air contains 20% of oxygen by volume and the reaction is forced to complete,
relative atomic mass of Y?
so that all sulphur dioxide and oxygen are converted to SO 3)
(Relative atomic mass: N = 14.0)
F.5 Revision – Mole
A.
80 dm3
page 11 of 16
B.
100 dm3
A.
a solution with highest concentration.
C.
120 dm3
B.
a solution with lowest concentration.
D.
3
C.
a solution with known concentration.
D.
a solution with concentration of 1 mol dm3.
140 dm
□
□
3
72. Compound Y contains 50% sulphur and 50% oxygen by mass. What is the empirical
76. Which of the following apparatus can transfer 28.7 cm of solution most accurately?
formula of compound Y? (Relative atomic masses: O = 16.0; S = 32.1)
A.
Measuring cylinder
A.
SO
B.
Burette
B.
SO2
C.
Pipette
C.
SO3
D.
Conical flask
D.
SO4
□
77. Which of the following apparatus should be cleaned with the solution to be held just
□
73. What is the volume of oxygen required for the complete combustion of 50 cm3 of
methane, CH4? (Molar volume of any gases at room temperature and pressure = 24 dm
3
mol1)
3
before using it/them?
(1)
Burette
(2)
Conical flask
(3)
Pipette
A.
100 cm
A.
(1) only
B.
50 cm3
B.
(2) only
C.
3
25 cm
C.
(1) and (3) only
D.
10 cm3
D.
(2) and (3) only
□
74. What is the volume of oxygen required for the complete combustion of a mixture of 50
3
3
cm of methane, CH4, and 25 cm of carbon monoxide, CO? (Molar volume of any gases at
78. Which of the following is a correct procedure to prepare a standard solution starting
with a pure solid?
A.
3
75 cm
B.
100 cm3
Weigh the solid  Put into volumetric flask  Dissolve the solid
 Add water to the mark of volumetric flask
room temperature and pressure = 24 dm3 mol1)
A.
□
B.
Weigh the solid  Dissolve the solid  Put into volumetric flask
 Add water to the mark of volumetric flask
3
C.
112.5 cm
D.
150 cm3
C.
 Dissolve the solid  Put into volumetric flask
□
75. A standard solution is
F.5 Revision – Mole
Add water to the mark of volumetric flask  Weigh the solid
D.
Add water to the mark of volumetric flask  Weigh the solid
 Put into volumetric flask  Dissolve the solid
page 12 of 16
□
79. Which of the following substances CANNOT be used to prepare a standard solution
hydrochloric acid?
directly?
A.
Wash the burette with hydrochloric acid only.
(1)
Concentrated H2SO4
B.
Wash the burette with distilled water only.
(2)
Solid NaOH
C.
Wash the burette with distilled water and then hydrochloric acid.
(3)
Liquid NH3
D.
Wash the burette with hydrochloric acid and then distilled water.
□
A.
(1) and (2) only
84. What volume of 0.25 mol dm3 sulphuric acid is required to neutralize 40.0 cm3 of 0.2
B.
(1) and (3) only
mol dm3 sodium carbonate?
C.
(2) and (3) only
Na2CO3 + H2SO4  Na2SO4 + H2O + CO2
D.
(1), (2) and (3)
□A.
80. Which of the following indicators can be used in the titration of HCl(aq) with NH 3(aq)?
(0.25  40)/ 0.2 cm3
B.
(0.25  40  2)/ 0.2 cm3
A.
Phenolphthalein
C.
(0.2  40)/ 0.25 cm3
B.
Methyl orange
D.
(0.2  40)/ (0.25  2) cm3
C.
Universal indicator
D.
No suitable indicator
□
85. Which of the following are correct procedures just before using a conical flask in
□
titration?
3
81. In a titration experiment, 25.0 cm of ammonia solution is titrated against a standard
(1)
It is washed with the solution which is going to be delivered by the pipette.
solution of hydrochloric acid with methyl orange as indicator. Which of the following
(2)
It is washed with the distilled water.
colour change is correct at the end point?
(3)
A piece of white tile is placed under it during titration.
A.
Yellow to orange
A.
(1) and (2) only
B.
Red to orange
B.
(1) and (3) only
C.
Red to colourless
C.
(2) and (3) only
D.
Colourless to orange
□D.
□
(1), (2) and (3)
82. Which of the following solutions would neutralize 50 cm3 of 0.1 M H2SO4 completely
86. The following table shows the results of a titration. What is the average volume of acid
when mixed?
added in this titration?
A.
50 cm3 of 0.1 M KOH
B.
100 cm3 of 0.1 M NaOH
3
C.
50 cm of 0.1 M NH3
D.
100 cm3 of 0.1 M Ca(OH)2
83. Which of the following is a correct procedure before filling the burette with dilute
F.5 Revision – Mole
Titration
1
2
3
4
Final reading (cm3)
□
24.6
26.1
25.4
26.6
Initial reading (cm3)
1.1
1.4
0.6
2.1
Burette reading
page 13 of 16
Volume of acid added (cm3)
A.
24.4 cm3
B.
24.7 cm3
C.
24.8 cm3
D.
24.5 cm3
23.5
24.7
24.8
24.5
are mixed in a polystyrene cup. In which of the following combinations would the
temperature rise be the greatest?
Volume of 1.0 M NaOH(aq)/cm3
Volume of 1.0 M HCl(aq)/cm3
A.
20
100
B. □
40
80
C.
60
60
D.
80
40
3
87. The concentration of an aqueous solution of an acid is 2.0 M. 20.0 cm of this acid
solution requires 80.0 cm3 of 1.0 M sodium hydroxide solution for complete neutralization.
What is the basicity of the acid?
A.
1
B.
2
91. 0.57 g of a sample of hydrated sodium carbonate Na 2CO3  nH2O required 20.0 cm3 of
C.
3
0.20 M hydrochloric acid for complete neutralization. What is the number of crystallization,
D.
4
n, in□
the formula?
88. In an experiment, 2.0 M sodium hydroxide solution was added to 20.0 cm3 of 1.0 M
(Relative atomic masses: H = 1.0; C = 12.0; O = 16.0; Na = 23.0; Cl = 35.5)
sulphuric acid until the acid was completely neutralized. What is the concentration of
A.
1
sodium sulphate (correct to two decimal places) in the resulting solution?
B.
5
A.
0.25 M
C.
9
B.
0.33 M
D.
10
C.
0.50 M
92. 1.05 g of a mixture of anhydrous sodium carbonate and sodium chloride was dissolved
D.
1.00 M
in 50□cm3 of deionized water. The resulting solution required 28.5 cm3 of 0.15 M sulphuric
89. The formula of a metal carbonate is X2CO3. 50 cm3 of a solution containing 0.53 g of
acid for complete reaction. What is the percentage purity of the anhydrous sodium
the carbonate requires 25 cm3 of 0.2 M sulphuric acid for complete neutralization. What is
carbonate sample?
the relative atomic mass of metal X?
(Relative atomic masses: C = 12.0; O = 16.0; Na = 23.0)
A.
19.0
A.
21.4 %
B.
21.0
B.
42.9 %
C.
23.0
C.
64.3 %
D.
25.0
□D.
85.6 %
90. Different volumes of 1.0 M sodium hydroxide solutions and 1.0 M of hydrochloric acid
93. 8.5 g of sodium carbonate can neutralize 25.0 cm3 of 1 M sulphuric acid. What is the
mass of carbon dioxide liberated at room temperature and pressure?
F.5 Revision – Mole
□
page 14 of 16
□
□
(Relative atomic masses: C = 12.0; O = 16.0; Na = 23.0)
A.
Increasing the temperature
A.
1.1 g
B.
Using another catalyst
B.
1.8 g
C.
Using more manganese(IV) oxide
C.
3.5 g
D.
Adding some 1 M aqueous hydrogen peroxide
D.
4.5 g
□
□
97. Sodium
carbonate was added to excess dilute sulphuric acid at 30C. A student repeated
94. What mass of magnesium will react completely with 25.0 cm3 of 0.20 M hydrochloric
this experiment at 50C. The volumes of carbon dioxide produced were measured at room
acid?
temperature and pressure. Which of the following diagrams shows the correct result?
(Relative atomic mass: Mg = 24.3)
A.
A.
0.06 g
Volume of carbon dioxide
B.
0.12 g
o
At 30 C
C.
0.18 g
D.
0.24 g
□
Volume of carbon dioxide
At 50oC
At 50oC
95. 3.65 g of HCl(g) is dissolved in 100 cm3 of distilled water. What volume of 0.2 M
NaOH can neutralize the resulting solution?
B.
At 30oC
Time
C.
A.
250 cm3
Volume of carbon dioxide
B.
500 cm3
o
At 50 C
C.
3
750 cm
D.
1000 cm3
□
Time
D.
Volume of carbon dioxide
At 30oC
o
At 30 C
96. Curve I was obtained by observing the decomposition of 200 cm3 of 2 M aqueous
o
At 50 C
Time
hydrogen peroxide, catalyzed by manganese(IV) oxide.
Time
□
2H2O2(aq)  2H2O(l) + O2(g)
98. A test tube containing dilute sulphuric acid was placed in a flask containing excess zinc
Volume of oxygen formed
II
I
granules. The flask was then tilted so that the acid was poured out of the test tube and
completely covered the zinc granules. The flask was re-weighed at intervals from the start
of the reaction. Which of the following diagrams is correct?
Time
Which of the following changes could produce curve II?
F.5 Revision – Mole
page 15 of 16
Which of the following statements about section PQ of the curve is correct?
dilute sulphuric acid
zinc granules
A.
A.
The speed of reaction is at maximum.
B.
All the calcium carbonate has reacted.
C.
No more carbon dioxide is being produced.
D.
The concentration of the acid is increasing.
□
100. Which of the following methods is most suitable for measuring the reaction rate of the
B.
Mass of flask
following chemical reaction?
Mass of flask
S2O32(aq) + 2H+(aq)  SO2(g) + H2O(l) + S(s)
A.
Measuring the time taken to reach an easily seen stage. e.g. to blot out a
marked cross.
Time
C.
B.
Measuring the change in volume of H2O(l) with time.
C.
Measuring the change in volume of SO 2(g) formed with time.
D.
Measuring the change in pressure of the reaction system with time.
Time
D.
Mass of flask
Mass of flask
Time
Time
□
99. The graph shows how the total volume of carbon dioxide produced by the reaction
between dilute nitric acid and excess calcium carbonate varied with time.
Total volume of carbon dioxide produced
P
Q
Time
F.5 Revision – Mole
page 16 of 16
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