Kinetics MCQ

HKDSE Chemistry A Modern View Part IX Rate of Reaction

1

Section 38.1

1

Which of the following reactions is the fastest?

A. 6CO2(g) + 6H2O(l) C6H12O6(aq) + 6O2(g)

B. 4Fe(s) + 3O2(g) + 2H2O(l) 2Fe2O3 • H2O(s)

C. C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g)

D. 2C2H6(g) + 7O2(g) 4CO2(g) + 6H2O(l)

2

Which of the following reactions has the slowest rate?

A Reaction between hydrochloric acid and copper(II) carbonate

B. Reaction between dilute sulphuric acid and barium nitrate solution

C. Reaction between methane and chlorine in sunlight

D. Decay of fruit

3

Which of the following reactions is the slowest?

A. Neutralization of HCl(aq) and NaOH(aq)

B. Reaction of potassium and water

C. Corrosion of iron

D. Displacement reaction of Mg in CuSO4(aq)

Section 38.2

4

When 50 cm3 of 0.20 M hydrochloric acid was mixed with excess sodium

thiosulphate solution, the following reaction occurred.

S2O32(aq) + 2H+(aq) SO2(aq) + H2O(l) + S(s)

0.161 g of S was produced in 2 minutes. What is the average rate of production of S?

A. 8.05 × 102 g s1

B. 1.34 × 103 g s1

C. 0.417 cm3 s1

D. 1.67 × 103 M s1

5

The following graph shows the volume of hydrogen gas produced against time.


2

Which of the following statements about the above graph is INCORRECT?

A. The average rate of the reaction is about 7.25 cm3 min1.

B. The average rate between t = 1 min and t = 3 min is about 13.5 cm3 min1.

C. The instantaneous rate at t = 1 min is about 23.0 cm3 min1.

D. The instantaneous rate at t = 2 min is about 21.0 cm3 min1.

6

Which of the following can be shown by a rate curve?

(1) Instantaneous rate of a reaction

(2) Average rate of a reaction

(3) Amount of reactants/products at a particular time

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

7

Which of the following statements concerning a rate curve is/are true?

(1) The initial rate must be the fastest.

(2) If the slope of the tangent equals zero, then the reaction stops.

(3) The slope of the tangent must decrease from the largest value to zero.

A. (1) only

B. (2) only

Vol

ume

of h

ydro

gen

gas

(cm

3 )

Time of reaction (min)


3

C. (1) and (3) only

D. (2) and (3) only

8

5 g of calcium carbonate takes 250 s to react with the solution of hydrochloric acid

completely. What is the average reaction rate of the reaction?

A. 0.16 mol s1

B. 0.020 mol s1

C. 2.0 × 104 mol s1

D. 2.0 × 105 mol s1

9

When 10 cm3 of 1.0 M acidified potassium permanganate is mixed with excess

ethanedioate, the purple colour of the solution disappears after 40 s. Calculate the

average reaction rate of the reaction.

A. 0 M s1

B. 0.025 M s1

C. 0.050 M s1

D. 40 M s1

10

The rate curve of the amount of carbon dioxide produced when an acid reacts with a

carbonate is plotted. When is the rate of the reaction the fastest?

A. The graph is the steepest.

B. The graph is at 45 to the horizontal.

C. The graph is half finished.

D. The graph is horizontal.

11

Instantaneous rate can be obtained from a concentration-time graph. Which of the

following methods is correct?

A. Multiplying the concentration by time

B. Measuring the slope of the graph at that instant

C. Measuring the area under the graph

D. Dividing the concentration by time

12

A chemical reaction completed in 10 minutes and released 0.16 g of oxygen gas. What


4

is the average rate of this reaction?

A. 8.33 × 106 mol s1

B. 9.33 × 105 mol s1

C. 5.00 × 104 mol s1

D. 8.00 × 103 mol s1

13

Which of the following methods are possible to quench a reaction?

(1) Cooling the reaction mixture with an ice bath

(2) Removing one or more of the reactant(s)

(3) Diluting the reaction mixture

(4) Adding a catalyst

A. (1), (2) and (3)

B. (1), (2) and (4)

C. (1), (3) and (4)

D. (2), (3) and (4)

14

The rate of formation of O3(g) is 2.0 × 107 mol dm3 s1 for the reaction:

3O2(g) 2O3(g)

What is the rate of disappearance of O2(g) in mol dm3 s1?

A. 1.3 × 107

B. 2.0 × 107

C. 3.0 × 107

D. 4.5 × 107

15

A reaction follows the concentration-time diagram. Which of the following values is

closest to the instantaneous rate for this reaction at the 20th second?


5

A. 5 × 103 M s1

B. 5 × 103 M s1

C. 2 × 103 M s1

D. 2 × 103 M s1

16

Which of the following can be used to determine the rate of reaction at a specific time

from a graph of concentration against time?

A. Concentration at that time divided by the time

B. Logarithm of the concentration divided by the time

C. Slope of the graph at that time

D. Logarithm of the slope divided by the time

17

What is the initial rate of the reaction (in mol dm3 s1) represented by this graph?

A. 0.08

B. 0.08

Time (s)

Con

cent

rati

on (

M)

Time (s)

Con

cent

rati

on (

M)


6

C. 0.02

D. 0.02

18

Based on the definition for rate of reaction, which of the following is a unit of

reaction rate?

A. mol dm3

B. mol s2

C. dm3 min3

D. mol dm3 min1

19

Which of the following statements is correct for the reaction below?

4P + Q 2R + 2S

A. The rate of formation of R is one half the rate of disappearance of Q.

B. The rate of decrease of Q is one quarter of the rate of disappearance of P.

C. The rates of formation of R and S are not equal.

D. The rate of formation of S is double the rate of disappearance of P.

20

Consider the esterification between ethanol and ethanoic acid in the presence of an

acid catalyst. The concentration of ethyl ethanoate builds up to 0.68 mol dm3 in 2

minutes. Calculate the average rate of the reaction.

A. 0.68 mol dm3 min1

B. 0.34 mol dm3 min1

C. 0.68 mol min1

D. 0.34 mol min1

21

Combustion of methane gives carbon dioxide as one of the products. CH4(g) + 2O2(g)

CO2(g) + 2H2O(l) The concentration of carbon dioxide increases from 0 to 2 ×

102 mol dm3 in 0.01 seconds. What is the average rate of decrease of O2(g)

concentration?

A. 0.02 mol dm3 s1

B. 0.04 mol dm3 s1

C. 2 mol dm3 s1

D. 4 mol dm3 s1


7

22

Copper(II) ion reacts with ammonia molecules to form a deep blue complex: Cu2+(aq)

+ 4NH3(aq) [Cu(NH3)4]2+(aq) The average rate of decrease of ammonia is 1.6 ×

102 mol dm3 s1. Calculate the average rate of increase of the complex

concentration.

A. 6.4 × 102 mol dm3 s1

B. 3.2 × 102 mol dm3 s1

C. 4.0 × 103 mol dm3 s1

D. 2.0 × 103 mol dm3 s1

23

The average reaction rate of the complete reaction A B + C was 0.15 mol dm3 s1.

If the time taken for the reaction to complete was 30 seconds, what was the total

change in concentration of A?

A. 0.0050 mol dm3

B. 0.75 mol dm3

C. 4.5 mol dm3

D. 20 mol dm3

24

Which of the following statements concerning the tangents to the rate curve is

INCORRECT?

A. The slope of the tangent represents the rate of the reaction.

B. The tangent at time zero is usually the steepest.

C. The slope of the tangent is equal to 0 when t = 0.

D. The steepness of the tangents will decrease as the reaction proceeds.

25

5 g of magnesium ribbon of 70% purity was added to 200 cm3 of 0.050 M

hydrochloric acid. The reaction took 50 seconds to complete and volume of gas

collected was 4800 cm3. Which of the following statements is correct?

A. Magnesium ribbon is the limiting reagent.

B. Hydrochloric acid is the limiting reagent.

C. The rate of reaction of first 30 seconds is 100 cm3 s1.

D. The average rate of mass decrease of magnesium is 0.07 g s1.

26

Which of the following is NOT a unit of chemical reaction rate?


8

A. s mol1

B. cm3 s1

C. g min1

D. mol dm3 s1

27

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 min1

B. The average rate of decrease in concentration of the acid was 0.0125 mol

dm3 s1

C. The average rate of increase in volume of carbon dioxide was 60 cm3 s1

D. Sodium carbonate and sulphuric acid just reacted completely.

28

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?

29

Which of the following diagrams shows a correct rate curve for a chemical reaction?

Pressure of gas

Time

A

C B

D


9

A.

B.

C.

D.

30

When excess dilute nitric acid reacts with magnesium carbonate, the reaction

gradually becomes slower and finally stops. Which of the following statements

correctly explains this 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.

31

The experiment shown in the diagram was set up and the syringe reading was noted at

intervals.

Amount of p

in the reaction

roduct

Time

Amount of p

in the reaction

roduct

Time

Amount of p

in the reaction

roduct

Time

Amount of p

in the reaction

roduct

Time


10

A graph of the syringe readings against time was plotted. Which of the following

curves would be obtained?

32

When steam is passed through a red-hot magnesium ribbon inside a combustion tube,

a reaction occurs and the temperature of the magnesium ribbon increases. What does

this indicate?

A. The reaction is reversible.

B. Steam contains impurities.

C. The reaction is exothermic.

D. Magnesium is an oxidizing agent.

33

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.

gas syringe

rubber connecting tubing

dilute HCl MgCO3(s)

A B C

D

Volume of gas

Time


11

Which of the following statements about section PQ of the curve is correct?

A. The speed of reaction is at maximum.

B. All calcium carbonate has reacted.

C. No more carbon dioxide is being produced.

D. The concentration of the acid is increasing.

34

Which of the following methods of obtaining the instantaneous rate from a

concentration-time graph is correct?

A. By equating the reaction rate with the concentration of reactant at that

instant.

B. By measuring the slope of the tangent to the curve at that instant.

C. By measuring the area under the graph from time zero to that instant.

D. The instantaneous rate cannot be obtained from a concentration-time graph.

35

A chemical reaction releases 0.16 g of oxygen gas in 10 minutes and reaches

completion. What is the average rate of this reaction?

A. 8.33 × 106 mol s1

B. 1.67 × 105 mol s1

C. 5.00 × 104 mol s1

D. 1.00 × 103 mol s1

Section 38.3

36

Which of the following methods can be used to quench a reaction?

(1) Cooling the reaction mixture rapidly in ice

(2) Removing the catalyst by adding another reagent

(3) Diluting the reaction mixture with a large amount of ice water

A. (1) and (2) only

P Q

Total volume of carbon

dioxide produced

Time


12

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

37

Which of the following statements about the reaction between ethyl ethanoate and

dilute sodium hydroxide solution is INCORRECT?

A. The concentration of a reactant at regular time intervals can be determined

by titrimetric analysis.

B. Ethanol is formed in the reaction.

C. The reaction can be quenched with ice water.

D. This reaction is regarded as esterification.

38

2MnO4(aq) + 5H2O2(aq) + 6H+(aq) 2Mn2+(aq) + 8H2O(l) + 5O2(g)

Which of the following methods is/are possible for monitoring the progress of the

above reaction?

(1) Titrimetric analysis

(2) Measuring the change in colour intensity by colorimetry

(3) Measuring the change in volume of gas

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

39


(1) Cooling the reaction mixture slowly

(2) Removing one of the reactants

(3) Diluting the reaction mixture with cold water

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

40

What is/are the advantage(s) of using titrimetric analysis to follow the progress of a

reaction?


13

(1) Only simple apparatus like pipette is required.

(2) The reaction does not need to be quenched.

(3) There is a continuous monitoring of the progress of reaction.

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

41

Which of the following reactions CANNOT be followed by using the method of

measuring the change in pressure of a gas?

A. Na2CO3 + HCl

B. Zn + CH3COOH

C. Na2SO3 + CH3COOH

D. Zn + HCl

42

Concerning the method used to study the progress of a chemical reaction between

sodium thiosulphate and hydrochloric acid by measuring the change in transmittance

of light through the reaction mixture, which of the following statements is correct?

A. The transmittance of light through the solution is affected by the formation

of sulphur dioxide.

B. A data-logger is required in this method.

C. The rate of the reaction is directly proportional to the time taken for the

‘blot out’ of the cross.

D. The cross should be seen from a position immediately above it.

43

Which of the following methods can be used to determine the reaction rate of the

following reaction?

Cr2O72(aq) + 14H+(aq) + 3C2O4

2(aq) 6CO2(g) + 7H2O(l) + 2Cr3+(aq)

(1) Measuring volume of CO2 formed

(2) Measuring time for pH change

(3) Measuring time for the colour of the solution to change from orange to green

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)


14

44

Some marble chips are mixed with excess dilute hydrochloric acid in a stoppered

conical flask. The flask is placed on an electronic balance to determine its mass. The

mass of the reaction mixture is measured at regular time intervals. Which of the

following graphs represents the rate of the reaction?

A.

B.

C.

D.

45

Which of the following reactions and methods of measuring reaction rate is

INCORRECTLY matched?

Reaction Method of measuring reaction rate

A. Fe3+(aq) + SCN(aq) Measure the change in colour

intensity of the reaction mixture

B. C4H6O4(aq) + NaHCO3(aq) Measure the change in pressure of

reaction system by pressure sensor

and data-logger

C. H2O2(aq) + I(aq) + H+(aq) Measure the change in mass of

reaction mixture by electronic

balance

D. CH3COCH3(aq) + I2(aq) +

H+(aq)

Measure the change in

concentration of I2(aq) by titration

with sodium thiosulphate solution

46

In order to follow the progress of the reaction,

Br2(aq) + HCOOH(aq) 2Br(aq) + 2H+(aq) + CO2(g)

Which of the following techniques can be used?

Time

Reading of

the balance

Time

Reading of

the balance

Time

Reading of

the balance

Time

Reading of

the balance


15

(1) Measuring the volume of gas produced

(2) Measuring the loss of mass of the reaction mixture

(3) Colorimetry

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

47


HCOOCH3(aq) + NaOH(aq) HCOONa+(aq) + CH3OH(aq)

Which of the following techniques can be used?


(2) Colorimetric analysis


A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

48


S2O32(aq) + 2H+(aq) SO2(g) + S(s) + H2O(l)

a paper with a black cross marked on it was placed below the beaker containing the

reaction mixture. The cross gradually disappeared as the reaction proceeded. Which of

the following is NOT a disadvantage of this technique?

A. There is a significant error in determining whether the cross disappeared.

B. The gas produced would affect the transmittance of light through the

solution.

C. The rate of reaction at a particular instant cannot be found.

D. The value of cross theof ncedisappearafor taken time

1 is just proportional

to the average rate of reaction.

49

Hydrogen ion is used as a catalyst in esterification. Which of the following can be

used to quench the reaction?

A. Potassium permanganate


16

B. Hydrochloric acid

C. Carbon dioxide

D. Sodium hydroxide

50

A student is monitoring the progress of a chemical reaction by measuring the change

in mass of the reaction mixture. The set-up is shown below:

Which of the following combinations is correct?

X Y

A. Cotton wool plug Magnesium carbonate

B. Rubber plug Magnesium chloride

C. Cotton wool plug Magnesium sulphate

D. Rubber plug Magnesium hydroxide

51



(2) Cooling the reaction mixture

(3) Removing the reactant

(4) Removing the product

A. (1), (2) and (3)

B. (1), (2) and (4)

C. (1), (3) and (4)

D. (2), (3) and (4)

52

Which of the following methods can monitor the rate of the reaction between Mg

ribbon and HCl?

(1) Measuring the change in mass of the reaction mixture

electronic balance

Y

X

hydrochloric acid


17

(2) Measuring the change in colour intensity of the reaction mixture

(3) Measuring the change in pressure of the reaction system

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

53

Which of the following reactions can be followed by measuring the change in mass?

A. The reaction of vinegar and sodium hydroxide solution

B. The decomposition of hydrogen peroxide into hydrogen and oxygen

C. The reaction of magnesium ribbon and hydrochloric acid

D. The reaction of acidified silver nitrate solution and sodium chloride solution

54

Which of the following reactions and methods of measuring reaction rate are NOT

correctly matched?

Reaction Method of measuring reaction rate

A. Hydrochloric acid and

sodium thiosulphate solution

Measuring the time taken for the

‘blot out’ of a cross

B. Methyl ethanoate and sodium

hydroxide

Measuring the change in

concentration of sodium hydroxide

by titration with standard acid

C. Magnesium ribbon and

sulphuric acid

Measuring the change in pressure of

reaction system by pressure sensor

and data-logger

D. Decomposition of hydrogen

peroxide into hydrogen and

oxygen

Measuring the change in volume of

gas produced

55

The reaction rate of which of the following reactions can be measured using a

colorimeter?

A. Dissolving eggshells in sulphuric acid solution

B. The reaction of sulphur dioxide and bromine water

C. The reaction of ethyl propanoate and sodium hydroxide

D. The reaction of silver and nitric acid


18

56

After the addition of marble chips to an excess of dilute hydrochloric acid in a conical

flask, each of the following was measured and plotted against time on a graph.

If the reaction was complete in 2.5 minutes, which of the following, when plotted

against time, would give a graph like the one shown above?

A. Total mass of the conical flask and its contents

B. Volume of carbon dioxide produced

C. pH of the solution

D. Temperature of the solution

57

In which of the following reactions the rate CANNOT be measured by the set-up

shown?

A. ZnCO3 + HCl

B. Zn + H2SO4

C. ZnO + HNO3

D. Zn + CH3COOH

58

Which of the following shows the correct sequence of results of measuring rate of

reaction between sodium thiosulphate solution and dilute hydrochloric acid? (The

diagrams show the top view of the solution in a beaker putting on top of a marked

collected gas gas syringe

dilute hydrochloric acidmagnesium ribbon

Time (min)


19

cross.)

A.

B.

C.

D.

59

Which of the following sets of apparatus could be used to measure the speed of the

reaction between marble chips and dilute nitric acid?

(1)

(2)

dilute nitric acid marble chips

boiling tube

water

dilute nitric acid

electronic balance


20

(3)

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

60

A test tube containing dilute sulphuric acid was placed in a flask containing excess

zinc 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?

A.

B.

dilute sulphuric acid

zinc granules

Mass of flask

Time

Mass of flask

Time

rubber connecting tubing

gas syringe

dilute nitric acid marble chips


21

C.

D.

61

Which of the following methods is most suitable for measuring the reaction rate of the

following chemical reaction?

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.

B. Measuring the change in volume of H2O(l) with time.

C. Measuring the change in volume of SO2(g) formed with time.

D. Measuring the change in pressure of the reaction system with time.

62


Br2(aq) + HCOOH(aq) 2Br(aq) + 2H+(aq) + CO2(g)

Which of the following techniques can be adopted?

(1) Measuring the volume of gas produced



A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

63


HCOOCH3(aq) + NaOH(aq) HCOONa(aq) + CH3OH(aq)

Which of the following techniques can be adopted?




A. (1) only

Mass of flask

Time

Mass of flask

Time


22

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

64

Which of the following methods are possible to quench a reaction mixture?

(1) Cooling the reaction mixture in ice

(2) Removing one of the reactants


A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

65

In order to follow the progress of the following reaction:

S2O32(aq) + 2H+(aq) SO2(g) + S(s) + H2O(l),

a white tile with a cross marked on it was placed below the beaker of reaction mixture.

The cross gradually disappeared as the reaction went on. Which of the following is

NOT a disadvantage of this technique?

A. There is a significant error in determining whether the cross has

disappeared.

B. It is inconvenient to set up the apparatus.

C. The rate of reaction at a particular instant cannot be found.

D. The value of cross theof ncedisappearafor taken time

1 is just proportional

to the average rate.

Each question below consists of two separate statements. Decide whether each of

the two statements is true or false; if both are true, then decide whether or not

the second statement is a correct explanation of the first statement. Then select

one option from A to D according to the following table:

A. Both statements are true and the 2nd statement is a correct explanation

of the 1st statement.

B. Both statements are true and the 2nd statement is NOT a correct

explanation of the 1st statement.

C. The 1st statement is false but the 2nd statement is true.

D. Both statements are false.


23

Section 38.1

66

Zn reacts with water faster than Cu. Zn is more reactive than Cu.

67

There is no air inside a refrigerator. Food will go bad slower in a

refrigerator.

Section 38.2

68

The initial rates of most reactions are

the highest.

The initial rate of a reaction is the

instantaneous rate at t = 0.

69

The instantaneous rate of a reaction is

calculated from the slope of the tangent

to the rate curve at t = 0.

The rate curve of most reactions is the

steepest at first and becomes less steep

with time.

70

Instantaneous rate of reaction is always

higher than the average rate of

reaction.

Average rate of reaction can be

calculated from a rate curve.

Section 38.3

71

Ice water is usually used to quench a

reaction.

Ice water dilutes the reaction mixture.

72

The rate of reaction between sodium

thiosulphate and dilute hydrochloric

acid is measured by the time taken for

the ‘blot out’ of the cross marked on

the white tile.

The time taken for the ‘blot out’ of the

cross is inversely proportional to the

average rate of formation of sulphur.


24

73

Sodium carbonate can be used to

quench the reaction between

propanone and iodine.

An acid is used as the catalyst in the

reaction between propanone and iodine.

Chemistry: Chapter 39 Factors affecting rate of reaction

Sections 39.139.2

74

Which of the following statements concerning the collision theory are correct?

(1) Reactant particles must collide to trigger a reaction.

(2) Products can only be formed if the collision is in the right orientation, regardless

of the speed of the reactant particles.

(3) Only a small fraction of collisions is classified as effective collisions.

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

75

According to the collision theory, which of the following is/are essential for a

chemical reaction to occur?

(1) Collision of reactant particles.

(2) Possession of adequate kinetic energy by reactant particles.

(3) Possession of adequate kinetic energy by product particles.

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

76

An increase in the number of effective collisions per unit time implies

A. an increase in concentration of reactants.

B. an increase in temperature.

C. an increase in surface area of reactants.

D. an increase in reaction rate.

77


25

Which of the following is/are important in determining whether a reaction occurs?

(1) Size of the molecules

(2) Energy of the molecules

(3) Orientation of the molecules

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

Section 39.3

78

A fixed mass of magnesium strips reacts with excess dilute sulphuric acid of different

concentrations. Which of the following statements is/are correct?

(1) For the most concentrated acid, the rate curve of production of H2 gas gives the

largest slope initially.

(2) For the most concentrated acid, the reaction takes the longest time to complete.

(3) For the most concentrated acid, the volume of H2 gas produced is the largest.

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

79

In the graphs below, curve (i) was obtained when 3 g of zinc granules was reacted

with excess 2.0 M hydrochloric acid. Curves (ii) and (iii) were obtained after making

changes to the acid.

Curve (ii): Excess 1.0 M nitric acid

Curve (iii): Excess 1.5 M sulphuric acid

Which of the following graphs matches the rate curves (i), (ii) and (iii) correctly?

A.

Volume

of H2(g) ii

Time

i iii


26

B.

C.

D.

80

Consider the following equation of rusting of iron:

4Fe(s) + 3O2(g) + 2nH2O(l) 2Fe2O3 • nH2O(s)

Which of the following statements correctly explains that a coating of oil can slow

down the rusting of iron gears of a bicycle?

A. The oil cools down the iron gears.

B. The oil prevents oxygen from reaching the iron gears, so the concentration

of oxygen in the rusting reaction is decreased.

C. The oil decreases the surface area of iron gears.

D. The oil is an ‘anti-catalyst’.

81

When the concentration of a reactant is increased, which of the following concerning

the reactant particles will NOT occur?

Volume

of H2(g) ii i iii

Time

Volume

of H2(g) iii

i

ii

Time

iii

i

ii

Volume

of H2(g)

Time


27

(1) There will be a larger number of collisions.

(2) Reactant particles will have a greater amount of average kinetic energy.

(3) There will be a larger fraction of effective collisions.

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

82

An experiment was carried out to investigate the relationship between temperature

and rate of reaction for the following reaction.

S2O32(aq) + 2H+(aq) S(s) + SO2(g) + H2O(l)

The resultant solution became cloudy as sulphur was formed in the reaction. A paper

with a black cross marked on it was placed below the beaker containing the reaction

mixture. At 298 K, time taken for the ‘blot out’ of the cross was 130 seconds. At 308

K, the time was 66 seconds. Which of the following conclusions can be obtained?

A. Rate increases by around two times when the temperature increases by 10

K.

B. Rate increases by around four times as the temperature increases by 10 K.

C. Rate decreases by roughly a half as the temperature increases by 10 K.

D. Rate decreases by roughly one fourth as the temperature increases by 10 K.

83

Zinc metal reacts with excess 1.0 M HCl according to the following equation:

Zn(s) + 2H+(aq) Zn2+(aq) + H2(g)

Which of the following changes will increase the rate of evolution of H2(g)?

(1) Using zinc dust instead of chunks.

(2) Using 200 cm3 of 1.0 M HCl in place of 100 cm3.

(3) Using 2.0 M HCl instead of 1.0 M HCl.

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

84

For a given reaction, why does the rate of reaction increase when the concentrations

of the reactants are increased?

A. The frequency of the molecular collisions increases.


28

B. The surface area of molecules increases.

C. The average kinetic energy of the molecules increases.

D. The amount of the reactants increases.

85

Consider the reaction of excess dilute hydrochloric acid and magnesium ribbon,

which of the following parameters is/are NOT changed upon changes in the

concentration of the hydrochloric acid, given other factors are kept constant?

(1) The total heat energy released from the reaction mixture

(2) The time taken for the reaction to complete

(3) The total volume of gas collected

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

86

Which of the following reactants will give the highest reaction rate when reacting

with 1 g of NaOH(s)?

A. 90 cm3 of 0.2 M H2SO4

B. 80 cm3 of 0.3 M H2SO4

C. 60 cm3 of 0.4 M HCl

D. 40 cm3 of 0.5 M HCl

87

Arrange the following reaction rates in descending order.

(1) Reaction between 3.0 g of magnesium granules and 1.0 M of CH3COOH at

room temperature.

ture.

(2) Reaction between 3.0 g of magnesium powder and 1.0 M of HCl at a warm water

bath.

(3) Reaction between 3.0 g of magnesium powder and 0.6 M of H2SO4 at a warm

water bath.

(4) Reaction between 2.0 g of magnesium granules and 0.9 M of CH3COOH at

room tempera

A. (1) > (3) > (4) > (2)

B. (2) > (3) > (4) > (1)

C. (2) > (4) > (1) > (3)

D. (3) > (2) > (1) > (4)


29

Section 39.4

88

Consider the following reaction:

S2O32(aq) + 2H+(aq) SO2(g) + H2O(l) + S(s)

A white tile with a black cross marked on it was placed under a beaker. 50.0 cm3 of

0.10 M sodium thiosulphate solution and 10.0 cm3 of 1.0 M hydrochloric acid were

mixed in the beaker. Sulphur was produced and the cross was blocked. Which of the

following changes can make the cross disappear in a shorter time?

(1) Warm the reagents before the reaction.

(2) Use 100 cm3 of 0.10 M sodium thiosulphate solution instead.

(3) Use 20.0 cm3 of 2.0 M hydrochloric acid instead.

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

89

An increase in temperature of the reactants increases the rate of reaction. Which of the

following statements explains this situation correctly?

A. Heat energy causes an increase in concentration of the reactants.

B. Heat energy causes an increase in size of the molecules.

C. Heat energy causes a decrease in energy required for the reaction to occur. D. Heat energy causes the reactant particles to move faster.

90

Sodium hydroxide reacts with acids. Which of the following solutions would give the

highest initial rate?

A. 60 cm3 of 1.5 M NaOH(aq) and 60 cm3 of 1.5 M HCl(aq) at 30C.

B. 50 cm3 of 2.0 M NaOH(aq) and 50 cm3 of 2.0 M HCl(aq) at 20C.

C. 20 cm3 of 2.0 M NaOH(aq) and 20 cm3 of 1.5 M H2SO4(aq) at 30C.

D. 40 cm3 of 1.5 M NaOH(aq) and 40 cm3 of 2.0 M CH3COOH(aq) at 25C.

91

Na2S2O3(aq) + H2SO4(aq) Na2SO4(aq) + H2O(l) + SO2(g) + S(s)

Which of the following reactions has the shortest time for ‘blot out’ at room

temperature and pressure?

Na2S2O3 H2SO4 H2O


30

Volume

(cm3)

Concentration

(mol dm3)

Volume

(cm3)

Concentration

(mol dm3)

Volume

(cm3)

A. 5 0.15 10 0.15 0

B. 5 0.20 10 0.10 5

C. 10 0.10 10 0.10 0

D. 5 0.20 5 0.20 10

92

When temperature is increased, which of the following concerning collisions of

reactant particles will occur?

(1) There will be a larger number of effective collisions.

(2) There will be a larger number of ineffective collisions.

(3) Reactant particles will have a higher average kinetic energy.

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

93

When the surface area of a solid reactant is increased, which of the following

concerning the reactant particles will NOT occur?

(1) There will be a larger number of collisions.

(2) Reactant particles will have a greater amount of average kinetic energy.

(3) There will be a larger fraction of effective collisions.

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

94

Powdering a solid reactant can

A. increase the chance of collision between reactant particles.

B. reduce the energy required for reaction to occur.

C. increase the concentration of the reactant.

D. convert the reactant into a catalyst.

95

A small increase in temperature often produces a large increase in the rate of a


31

chemical reaction because it

A. decreases the size of the reactant particles.

B. increases the effectiveness of the collisions between the reactant molecules.

C. decreases the number of collisions per second between the reactant

molecules.

D. decreases the volume of the solution, altering the concentrations of the

reactants.

96

The rates of many chemical reactions double when there is a ten-degree rise in

temperature. Which of the following factors DOES NOT contribute to this change in

rate with increasing temperature?

A. The average kinetic energy of the reactant species.

B. The number of collisions in a given time.

C. The number of very energetic species.

D. The moving path of the reactant particles.

97

Which of the following statements correctly explains the effect of increase in

temperature of reactants on reaction rate?

A. Increase in temperature raises the potential energy of the reactant particles.

B. Increase in temperature reduces the energy difference between the reactants

and products.

C. Increase in temperature raises the average kinetic energy of the reactant

particles.

D. Increase in temperature reduces the contribution from orientation factor.

98

A chemical reaction takes place inside a glow stick. The higher the temperature, the

brighter is the glow stick. Which of the following descriptions about the glowing time

at a higher temperature is correct?

A. Longer

B. Shorter

C. Unchanged

D. Uncertain

99

Superheated water (boiling point > 100C) can make cooking faster. Which of the


32

following methods can be used to prepare the superheated water?

A. Overheat the water.

B. Add table salt to the water.

C. Increase the pressure.

D. Use distilled water.

Section 39.5

100

Which of the following factors DOES NOT affect the rate of reaction?

A. Surface area of the solid reactant

B. Molar mass of the reactant

C. Temperature of the reaction system

D. Concentration of the reactant

101

Which of the following factors affect(s) the rate of reaction between a solid reactant

and a liquid reactant?

(1) Molar mass of the solid reactant

(2) Concentration of the liquid reactant

(3) Surface area of the solid reactant

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

102

Which of the following is the reason for the fact that antacids have to be chewed

before swallowing?

A. A catalyst is added by saliva.

B. The temperature of the antacid is increased.

C. The surface area of the antacids is increased.

D. The concentration of the antacids is increased.

103

Which of the following factors can speed up reactions in industrial chemical

production involving gaseous reactants?

(1) Temperature

(2) Pressure


33

(3) Catalyst

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

104

Consider the reaction between solid calcium carbonate and aqueous hydrochloric acid.

Which of the following conditions can be increased to speed up the reaction?

(1) Concentration of HCl

(2) Surface area of the CaCO3 particles

(3) Temperature

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

105

Excess magnesium was added to a beaker of aqueous hydrochloric acid on a balance.

A graph of the mass of the beaker and contents was plotted against time (curve 1).

Which of the following changes in the experiment could give curve 2?

(1) The same mass of magnesium but in smaller pieces

(2) The same volume of a more concentrated solution of hydrochloric acid

(3) A lower temperature

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

Time

Mas

s

1

2


34

106

Which of the following changes CANNOT increase the rate of the reaction of

chlorine gas and a liquid hydrocarbon?

A. Use UV light to dissociate the Cl2.

B. Increase temperature at constant pressure.

C. Use chlorine gas of higher concentration.

D. Increase the pressure by adding helium gas.

107

Which of the following factors determine(s) the rate of a chemical reaction?

(1) Molar mass of reactants added

(2) Average kinetic energy of reactant particles

(3) Surface area of solid reactants

A. (1) only

B. (2) only

C. (1) and (3) only

D. (2) and (3) only

108

Which of the following statements correctly explains the higher reaction rate when

using the same amount of powdered limestone instead of lumps of limestone to react

with hydrochloric acid?

A. Particles on the surface of the limestone are more activated for reactions to

occur, so increase in surface area increases the rate.

B. Particles on the surface of the limestone are more properly orientated so that

increase in surface area increases the rate.

C. The hydrogen ions are less reactive towards the particles inside the solid

reactant so that increase in surface area increases the rate.

D. The hydrogen ions can only collide with the particles on the surface of the

solid reactant so that increase in surface area increases the rate.

109

Which of the following statements explains correctly why antacids should be well

chewed before swallowing?

A. Gritted by teeth makes antacids hotter, so it will be more reactive.

B. The enzyme of the saliva can activate the antacids.

C. Chewing compresses the antacid molecules, so its concentration increases.


35

D. Chewing grinds the tablets into small pieces, so the surface area of antacids

increases.

110

Which of the following processes CANNOT be employed to increase the reaction

rate?

CaCO3(s) + 2HCl(aq) CaCl2(aq) + H2O(l) + CO2(g)

A. Use the same concentration of H2SO4.

B. Heat the reaction mixture.

C. Grind the calcium carbonate.

D. Carry out the reaction in a smaller container.

Section 39.6

111

The following set-up is used to investigate the decomposition of hydrogen peroxide.

2H2O2(aq) 2H2O(l) + O2(g)

xture against time was plotted. Which of the

following curves would be obtained?

A graph of the mass of the reaction mi

A B Cmixture

Time

D

Mass of

reaction

stopwatch

a small amount of

solid MnO 2

2 2

measured volume of standard

H O (aq)

electronic balance

cotton wool


36

hich of ng a catalyst MUST be correct?

unchanged after a reaction.

D. A catalyst can operate under any conditions.

mixed together and they have the following reactions:

hic f atements is correct?

D. The overall reaction is 2Q + R S + T.

n rate greatly. Which of

e f actions and catalysts are matched?

112

W the following statements concerni

A. The rate of reaction is increased.

B. A catalyst remains chemically and physically

C. A catalyst is neither a reactant nor a product.

113

P and Q are

P + Q R

Q + R P + S + T

W h o the following st

A. P is a catalyst.

B. Q is a catalyst.

C. R is a catalyst.

114

Catalyst is an important chemical that can increase the reactio

th ollowing re correctly

Reaction Catalyst

(1) 2SO2(g) + O2(g) 2SO3(g) Pt

(2) N2(g) + 3H2(g) 2NH3(g) Fe

(3 2H 2) 2O l) + O2(g) MnO2 (aq) 2H2O(

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

D. (1), (2) and (3)

B. tration of a solid reactant increases when its surface area

D. f reaction has no relationship with the enthalpy change of

reaction.

115

Which of the following about rate of reaction is correct?

A. The fraction of effective collisions does not depend on temperature.

The concen

increases.

C. The rate of reaction cannot be decreased by a catalyst.

The rate o


37

h the shape shown below are often observed for reactions involving

catalysts.

d to the fact that

formed.

occupied.

D. the catalyst is used up.

of gaseous products, which of the following changes will lower the reaction

te?

ure

D. Using a steam bath

(1) t particles are moving at equal speed under the same temperature and

(3) es collide at high speed and both

eactive sites for reaction.

D. (2) and (3) only

116

Curves wit

The level portion of the curve is best attribute

A. product is no longer being

B. the reaction is complete.

C. all the catalytic sites are

117

For an exothermic reaction in which 2 moles of gaseous reactants are converted to 3

moles

ra

A. Decreasing the volume

B. Adding more reactants

C. Decreasing the press

118

Which of the following statements about the collision theory is/are INCORRECT?

All reactan

pressure.

(2) Only a small fraction of collisions can lead to the formation of products.

Products are formed when the reactant particl

particles have the r

A. (1) only

B. (2) only

C. (1) and (3) only

Concentration of reactant

Rea

ctio

n ra

te


38

hich of alyst is INCORRECT?

C. can increase the frequency of collisions between reactant

D. A catalyst can be regenerated at the end of a reaction.

on 39.7

119

W the following statements concerning a cat

A. A catalyst can increase the reaction rate.

B. A catalyst is neither a reactant nor a product of a reaction.

A catalyst

particles.

Secti

c is/are used in Contact process?

of 450C

) e of 250 atm

D. (2) and (3) only

ents concerning the

) b ced in the reaction makes the bread ‘raise’.

D. (1), (2) and (3)

negar?

B. p the reaction leading to the formation

C. indeed the oxides of iron. Thus, acid neutralizes and

120

Whi h of the following conditions

(1) A high temperature

(2) Iron as the catalyst

(3 A high pressur

A. (1) only

B. (2) only

C. (1) and (3) only

121

Yeast is commonly used in bakery. Which of the following statem

reaction that involves yeast is/are correct?

(1) Yeast contains an enzyme called zymase as the catalyst.

(2) The enzyme breaks down starch into ethanol and carbon dioxide.

(3 Car on dioxide produ

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

122

Why can the browning of fruits be slowed down if they are put in vi

A. Vinegar prevents O2 to come into contact with the fruits.

The enzymes in cells which speed u

of brown substance are denatured.

Brown substances are

dissolves the oxides.


39

D. Brown substances dissolve in vinegar.

e following statements explains why catalysts are often used in chemical

eact ?

eactions.

D. Catalysts decrease the amount of reactants.

g is NOT a proper reason for the application of catalysts in

roducts.

D. To save the use of fuel.

t step in the manufacture of sulphuric acid. What is the

his process?

D. VO3

c requires the presence of a catalyst?

sis of ester

one by iodine

)

D. (2), (3) and (4)

f

123

Which of th

r ions

A. Catalysts increase the rate of reactions.

B. Catalysts increase the yield of products of reactions.

C. Catalysts increase the purity of products of r

124

Which of the followin

chemical industries?

A. To save time.

B. To reduce the cost of production.

C. To increase the yield of p

125

Contact process is an importan

catalyst used in t

A. V2O2

B. V2O3

C. V2O5

126

Whi h of the following processes

(1) Alkaline hydroly

(2) Fermentation

(3) Oxidation of propan

(4 Browning of fruits

A. (1), (2) and (3)

B. (1), (2) and (4)

C. (1), (3) and (4)

Each question below consists of two separate statements. Decide whether each o


40


the second statement is a correct explanation of the first statement. Then select

one

A. ue and the 2nd statement is a correct explanation

B. nd statement is NOT a correct

ut the 2nd statement is true.


option from A to D according to the following table:

Both statements are tr


Both statements are true and the 2


C. The 1st statement is false b

Sections 39.139.3

e start of most

reactions is the highest.

start of most reactions are the highest.

127

The rate of reaction at th The concentrations of reactants at the

on of reactants for most

reactions.

e

reaction rate for most reactions.

128

Reaction rate depends on the

concentrati

Increasing the concentration of th

excess reactant will increase the

on 39.4Secti

increased, the reaction rate increases.

netic energy of the reactant

particles.

129

When the temperature of a reaction is An increase in temperature raises the

average ki

f

xcess

cid at a higher

temperature.

ased if the

temperature is raised.

130

Effervescence lasts longer when 3 g o

calcium carbonate is put into e

hydrochloric a

The reaction rate is incre

ons 39.539.6Secti

se the rate of a

chemical reaction.

y unchanged at

the end of a reaction.

131

Catalysts can increa A catalyst is chemicall


41

sed up

on, it is regarded as a

reactant.

ed when a

catalyst is used in a reaction.

132

Although a catalyst will not be u

in a reacti

Reaction time is always reduc

action mixture

of hydrogen peroxide.

he

position of

hydrogen peroxide.

133

Manganese(IV) oxide (MnO2) can be

regenerated from the re

Manganese(IV) oxide (MnO2) is t

catalyst for the decom

n always increase the rate

of reaction.

se the number of

effective collisions.

134

A catalyst ca A catalyst can increa

on 39.7Secti

dered

catalyst to catalyze a reaction.

ed as the catalyst in Haber

process.

135

It is generally better to use pow Iron is us

ss is carried out at 450C

and 1 atm.

moles of hydrogen in Haber process.

136

Haber proce One mole of nitrogen reacts with three

try: Chapter 40 Molar volume of gases at room temperature and pressure

r.t.p.)

on 40.1

Chemis

(

Secti

ases has the highest density at r.t.p.?

D. Carbon dioxide

137

Which of the following g

A. Chlorine

B. Ammonia

C. Propane

138


42

Consider the following chemical reaction:

ture and pressure. What is the molar volume of N2 at that temperature

D. 25.3 dm3 mol1

on 40.2

2NaN3(s) 2Na(s) + 3N2(g)

It was found that 0.524 g of NaN3 decomposes to form 0.290 dm3 of nitrogen gas at a

certain tempera

and pressure?

A. 22.8 dm3 mol1

B. 23.5 dm3 mol1

C. 24.0 dm3 mol1

Secti

gaseous sulphur trioxide,

oduced at this temperature and pressure?

D. 3.0 dm3

nitrogen fertilizers is

m volume of NO that can

.0 dm3 of NH3 and 16.0 dm3 of O2?

D. 20.0 dm3

ded to

.0 dm3 of propane (C3H8) measured at the same conditions?

D. 5.0 dm3

139

3.0 dm3 of sulphur dioxide gas, SO2, and 2.0 dm3 of oxygen gas, O2, are reacted at a

certain temperature and pressure. What is the volume of

SO3, that can be pr

A. 1.0 dm3

B. 1.5 dm3

C. 2.0 dm3

140

An important reaction in the production of

4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)

At constant temperature and pressure, what is the maximu

be produced from 14

A. 12.8 dm3

B. 14.0 dm3

C. 17.5 dm3

141

What volume of oxygen gas (O2), measured at 0C and 1 atm, is nee

completely burn 1

A. 10 dm3

B. 7.0 dm3

C. 6.0 dm3


43

142

Assume that 0.10 dm3 of N2 and 0.18 dm3 of H2, both at 50 atm and 450C, are

reacted to form NH3. If the reaction goes to completion, identify the reagent that is in

volume remained at the same temperature and pressure.

D. N2, 0.04 dm3

sulphur dioxide is reacted with 2.0

e equation below.

me of sulphur trioxide (in dm3) was formed at the same temperature and

D. 2.0

when 0.654 g of zinc was reacted with

chloric acid at r.t.p.?

D. 360 cm3

of oxygen at r.t.p. is required for the complete combustion of 150 cm3

D. 900 cm3

excess and determine the

A. H2, 0.02 dm3

B. H2, 0.08 dm3

C. N2, 0.01 dm3

143

At a certain temperature and pressure, 3.0 dm3 of

dm3 of oxygen according to th

2SO2(g) + O2(g) 2SO3(g)

What volu

pressure?

A. 5.0

B. 4.0

C. 3.0

144

What is the volume of hydrogen evolved

excess dilute hydro

A. 120 cm3

B. 200 cm3

C. 240 cm3

145

What volume

of propane?

A. 751 cm3

B. 802 cm3

C. 857 cm3

146

At a certain temperature and pressure, what is the volume of steam formed from the


44

reaction 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g) when 100 cm3 of ammonia is

oxygen at the same temperature and pressure?

D. 175 cm3

ith

complete

is the total volume of gas at the end of the reaction?

D. 320 cm3

s of gases have the same number of atoms at the same

temp ture and p

reacted with excess

A. 100 cm3

B. 125 cm3

C. 150 cm3

147

Butene reacts with oxygen according to the equation, C4H8(g) + 6O2(g) 4CO2(g)

+ 4H2O(l). At a certain temperature and pressure, 35.0 cm3 of butene was mixed w

300 cm3 of oxygen and the reaction was initiated by a spark. Assuming

combustion, what

A. 90 cm3

B. 140 cm3

C. 230 cm3

148

Which of the following pair

era ressure?

A. 200 cm3 of steam 200 cm3 of ammonia

B. 1 1 dm ide dm3 of carbon dioxide 3 of sulphur triox

C. 100 cm3 of methane 500 cm3 of neon

D. 50 cm3 of hydrogen chloride 50 cm3 of hydrogen sulphide

rogen to give hydrogen chloride. What is the volume

e volumes are measured at r.t.p.)

D. 140 cm3

d to sulphur trioxide by air, what is the

149

30 cm3 of chlorine is mixed with 70 cm3 of hydrogen in a test tube with a stopper.

Then the test tube is allowed to expose to sunlight for half an hour. In the presence of

sunlight, chlorine reacts with hyd

of hydrogen chloride produced?

(Assume that all th

A. 30 cm3

B. 40 cm3

C. 60 cm3

150

If two moles of sulphur dioxide are oxidize


45

minimum volume of air required at r.t.p.?

(Assuming air contains 20% of oxygen by volume and the reaction is forced to

complete, so that all sulphur dioxide and oxygen are converted to SO3; molar volume

= 24.0 dm3 mol1) of any gas at r.t.p.

A. 80 dm3

B. 100 dm3

C. 120 dm3

D. 140 dm3

xygen required for the complete combustion of 50 cm3 of

D. 10 cm3

mixture of

oxide, CO at r.t.p.?

any gas at r.t.p. = 24 dm3 mol1)

3

D. 150 cm3

vog o

B. tain the same number of molecules at the same

D. one mole of gas occupies 24.0 dm3 at room temperature and pressure.

volumes occupied by 1 mol of

er r.t.p. in ascending order?

oxide

151

What is the volume of o

methane, CH4 at r.t.p.?

A. 100 cm3

B. 50 cm3

C. 25 cm3

152

What is the volume of oxygen required for the complete combustion of a

50 cm3 of methane, CH4, and 25 cm3 of carbon mon

(Molar volume of

A. 75 cm3

B. 100 cm3

C. 112.5 cm

153

A adr ’s Law states that

A. one mole of substance contains 6.02 × 1023 units of that substance.

equal volumes of gases con

temperature and pressure.

C. gases occupy the same volume at any temperature and pressure.

154

Which of the following is the correct sequence of the

the following gases und

(1) Sulphur di


46

(2) Oxygen

(3) Carbon dioxide

A. (1), (2), (3)

B. (1), (3), (2)

C. (2), (3), (1)

D. They occupy the same volume.

ical reaction:

155

Consider the following chem

N2(g) + 3H2(g) 2NH3(g)

If the reaction goes to completion, what volume of hydrogen gas (H2) is required to

ammonia (NH3) at r.t.p.?

D. 30.0 cm3

hemical reaction:

hur needed to produce 10.0 cm3 of SO2 at r.t.p.?

D. 2.40 × 102 mol

carbon dioxide

is volume of oxygen unreacted?

) 4CO2(g) + 6H2O(l)

D. 75 cm3

40 cm3 of a gaseous oxide of

produce 20.0 cm3 of

A. 6.67 cm3

B. 10.0 cm3

C. 20.0 cm3

156

Consider the following c

S(s) + O2(g) SO2(g)

What is the amount of sulp

A. 4.17 × 104 mol

B. 4.17 × 102 mol

C. 2.40 × 103 mol

157

20 cm3 of ethane (C2H6) are burned with 95 cm3 of oxygen to give

and water as the only products. What

(All volumes are measured at r.t.p.)

2C2H6(g) + 7O2(g

A. 20 cm3

B. 25 cm3

C. 55 cm3

158

20 cm3 of chlorine reacts with 40 cm3 of oxygen to form


47

chlorine. What is the molecular formula of this oxide?

.t.p.)

D. Cl2O3

to form sulphur dioxide at r.t.p.,

rect?

u ed equals 24.0 dm3.

D. (1), (2) and (3)

4(g) at r.t.p.?

D. 48 000 cm3

les of 300 cm3 of ethane at room temperature and pressure?

D. 0.800 mol

volume of 2.80 moles of hydrogen chloride gas at room temperature and

(All volumes are measured at r

A. ClO

B. Cl2O

C. ClO2

159

When excess sulphur is burnt with 1 mole of O2

which of the following statements are cor

(1) Mole ratio of SO2 : O2 equals 1 : 1.

(2) Volume of SO2 formed equals 24.0 dm3.

(3) Vol me of O2 consum

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

160

What is the volume of 3 moles of CH

A. 7.2 dm3

B. 480 dm3

C. 72 000 cm3

161

What is the number of mo

A. 0.125 mol

B. 0.0125 mol

C. 0.0800 mol

162

What is the

pressure?

A. 67.2 dm3

B. 102 dm3

C. 0.672 dm3


48

D. 8.57 dm3

A. essure, the volume of a gas is determined

B. e of a gas is determined

C. re, different gases with equal volume

D. ure and pressure, 1 mole of gas molecules occupies a

volume of 24.0 dm3.

If

volumes of hyd ere reacted and pressure?

Volume

163

Which of the following statements is correct?

Under stated temperature and pr

by the size of the gas molecules.

Under stated temperature and pressure, the volum

by the quantity of the gas molecules.

Under stated temperature and pressu

have different number of molecules.

Under stated temperat

164

Hydrogen can be ignited in chlorine gas to form a white fume, hydrogen chloride.

250 cm3 of HCl was found to be the only remaining species in the reaction, what

rogen and chlorine w at room temperature

of H2 (cm3) Volume of Cl2 (cm3)

A. 250 250

B. 250 125

C. 125 125

D. 125 250

p. deviates from 24.0 dm3 mol1. Which of

nd?

cule

D. Molar mass of the gas molecule

etical reaction 2NxOy(g) xN2(g) + yO2(g) goes to completion upon

atoms, which of the following can be the molecular formula of the

y?

165

The molar volume of different gases at r.t.

the following is the main reason behi

A. Intermolecular interaction

B. Volume of the gas mole

C. Experimental inability

166

A hypoth

heating.

If originally there is only NxOy which contains 8.4 × 1023 atoms, and finally there are

2.4 × 1023 nitrogen

compound NxO

A. N2O


49

B. NO2

C. N2O4

D. N4O10

as the greatest number of atoms under r.t.p.?

a

D. 8.0 dm3 of sulphur trioxide

ha moles of atoms in 500 cm3 of CH4 at r.t.p.?

D. 10.4 mol

molecules in 305 cm3 of O2(g) at r.t.p.?

D 7.65 × 1021

followin equations represents the calculation of molar volume?

A.

167

Which of the following gases h

A. 18 dm3 of ammoni

B. 32 dm3 of helium

C. 6.0 dm3 of methane

168

W t is the number of

A. 1.04 mol

B. 0.104 mol

C. 0.0104 mol

169

What is the number of

A. 3.83 × 1021

B. 7.64 × 1022

C. 1.53 × 1022

170

Which of the g

massmolar

molarity

B. density

mass

oles

D.

molar

C. concentration × number of m

constant Avogadro

volumetotal

on 40.3Secti

f 4.3 g of ammonia gas at r.t.p.?

171

What is the volume o


50

A. 0.250 dm3

D. 607 dm3

ccupies a volume of 120 cm3 at r.t.p. What is the molar

D. 44.0 g mol1

s a mass of 1.33 g at r.t.p. What is this gas?

D. Methane

of 1.0 M sulphuric acid at r.t.p.

of carbon dioxide produced?

D. 228 cm3

ce

he volume of oxygen

.0 g of potassium chlorate is decomposed?

D. 2.94 cm3

MnO2

B. 6.07 dm3

C. 250 dm3

172

0.22 g of carbon dioxide o

mass of carbon dioxide?

A. 43.4 g mol1

B. 43.6 g mol1

C. 43.8 g mol1

173

1 dm3 of a certain gas ha

A. Nitrogen

B. Oxygen

C. Carbon monoxide

174

0.8 g of magnesium carbonate reacts with 100 cm3

What is the volume

A. 2.28 dm3

B. 4.56 dm3

C. 114 cm3

175

Potassium chlorate (KClO3) is often used in secondary school laboratories to produ

oxygen gas. When it is heated in contact with a catalyst, typically manganese(IV)

dioxide, it will decompose readily to give oxygen gas. What is t

obtained at r.t.p. if 5

A. 1.35 dm3

B. 1.47 dm3

C. 1.96 cm3


51

176

Limestone decomposes upon strong heating. What is the mass of limestone need

produce 6.0 dm

ed to

oxide at r.t.p.? (Assume the percentage by mass of

90%)

D. 30.2 g

2 are reacted according to the equation:

either is in excess.

D. Equal mass of NO is produced.

e reaction is

e volume of gas, in cm3, that is evolved at r.t.p.?

D. 68.5

e the mass of ammonium nitrate needed to produce 15.0 dm3 of laughing gas

D. 50.0 g

s anhydrous

3 of carbon di

CaCO3 in limestone =

A. 22.5 g

B. 25.0 g

C. 27.8 g

177

Equal masses of O2 and N

O2(g) + N2(g) 2NO(g)

Which of the following statements is true?

A. O2 is left at the end of the reaction.

B. N2 is left at the end of the reaction.

C. All of the O2 and N2 react and n

178

A 0.10 g sample of zinc is added to excess hydrochloric acid. When th

complete, what is th

A. 74.0

B. 36.7

C. 34.2

179

Dinitrogen oxide (N2O), which is commonly called laughing gas, can be made by

heating ammonium nitrate (NH4NO3) alone, with water as the only side product.

Calculat

at r.t.p.

A. 20.0 g

B. 30.0 g

C. 40.0 g

180

What volume of 0.5 M hydrochloric acid is required to neutralize exces


52

sodium carbonate, with 1200 cm3 of carbon dioxide produced at r.t.p.?

D. 300 cm3

) +

of aluminum carbide with excess water?

D. 0.420 dm3

ed by burning sulphur in oxygen.

ve reaction is INCORRECT?

A. r reacts with 1 mole of oxygen to give 1 mole of sulphur

B. react with 1 mole of oxygen to give 24.0 dm3 of sulphur

C. r reacts with 24.0 dm3 of oxygen to give 64.1 g of sulphur

D. 3 of oxygen to give 24.0 dm3 of

sulphur dioxide at r.t.p..

to excess dilute hydrochloric acid at .r.t.p.. What is the

any gas at r.t.p. is 24.0 dm3 mol1)

D. 120 cm3

A. 100 cm3

B. 200 cm3

C. 250 cm3

181

Methane can be synthesized from the hydrolysis of aluminium carbide, Al4C3(s

12H2O(l) 3CH4(g) + 4Al(OH)3(s). What volume of methane at r.t.p. can be

obtained from 0.48 g

A. 0.240 dm3

B. 0.300 dm3

C. 0.360 dm3

182

Sulphur dioxide is form

S(s) + O2(g) SO2(g)

Which of the following statements concerning the abo

(Molar volume of any gas at r.t.p. = 24.0 dm3 mol1)

1 mole of sulphu

dioxide at r.t.p..

32.1 g of sulphur

dioxide at r.t.p..

1 mole of sulphu

dioxide at r.t.p..

24.0 dm3 of sulphur reacts with 24.0 dm

183

0.2 g of calcium was added

volume of gas produced?

(Molar volume of

A. 20 cm3

B. 60 cm3

C. 100 cm3


53

184

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

. = 24.0 dm3 mol1)

D. 2Y + 6H+ 2Y3+ + 3H2

s Y have the same number of moles. What is the

(Molar volume of any gas at r.t.p. = 24.0 dm3 mol1)

as produced when 24.3 g of magnesium reacts with

acid at r.t.p.?

D. 48.0 dm3

s

itrogen and nitrogen gas exist as N2. What is the

nitrogen gas?

D. 2.78 dm3

r of moles of a gas at r.t.p. is given, which of the following can be

u

equation for the reaction?

(Molar volume of any gas at r.t.p

A. Y + 2H+ Y2+ + 2H

B. Y + 2H+ Y2+ + H2

C. 2Y + 2H+ 2Y + H2

185

If 7.0 g of nitrogen and 15.0 g of ga

volume of 15.0 g of gas Y at r.t.p.?

186

Consider the following chemical reaction:

Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g)

What is the volume of hydrogen g

excess hydrochloric

A. 12.0 dm3

B. 24.0 dm3

C. 36.0 dm3

187

3.25 g of liquid nitrogen is taken out from a freezer and placed at r.t.p. Finally it turn

back to nitrogen gas. Both liquid n

final volume of the

A. 200 dm3

B. 103 dm3

C. 5.57 dm3

188

If the numbe

calc lated?

(1) Mass of the gas


54

(2) Volume of the gas

(3 Number of formula un) its of the gas

D. (1), (2) and (3)

carbon dioxide formed at r.t.p. during the complete combustion

?

D. 16.6 dm3

s the mass of H2O formed in the complete combustion of 240 cm3 of ethane at

D. 0.72 g

number of atoms in 2.80 g of carbon monoxide at room temperature and

ress

D. 6.02 × 1023

ric acid, what

produced at room temperature and pressure?

3

D. 48 cm3

A. (1) and (2) only

B. (1) and (3) only

C. (2) and (3) only

189

What is the volume of

of 5.5 g of methane

A. 826 cm3

B. 166 cm3

C. 8.26 dm3

190

What i

r.t.p.?

A. 0.35 g

B. 0.54 g

C. 0.63 g

191

What is the

p ure?

A. 1.20 × 1023

B. 2.01 × 1023

C. 6.02 × 1022

192

When 0.2 g of magnesium carbonate is treated with excess dilute nit

volume of gas will be

A. 0.029 dm3

B. 0.057 dm

C. 5.7 cm3


55

at r.t.p. when 5.4 g of aluminium

dilute sulphuric acid?

D. 2.4 dm3

e of carbon dioxide can be 3 of 1.0 M hydrochloric acid?

D. 2.4 dm3

CO2(g) and H2O(l) at r.t.p.

e of O2 required in this combustion.

D. 3.27 dm3

as evolved when dissolving 0.5 g of magnesium ribbon in

id?

D. 6.74 dm3

occupies a volume of 498 cm3 at r.t.p. Calculate the molar volume

193

2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) + 3H2(g)

What is the volume of hydrogen gas formed

dissolves in excess

A. 7.2 dm3

B. 4.8 dm3

C. 3.6 dm3

194

A student uses hydrochloric acid to react with sodium carbonate at r.t.p. If

hydrochloric acid is the limiting reagent, what volum

produced from 50 cm

A. 0.60 dm3

B. 1.2 dm3

C. 1.8 dm3

195

C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l)

2.0 g of C3H8(g) undergoes complete combustion to give

Calculate the volum

A. 24.0 dm3

B. 5.47 dm3

C. 12.0 dm3

196

What is the volume of g

excess sulphuric ac

A. 494 cm3

B. 674 cm3

C. 4.94 dm3

197

0.623 g of ethane


56

of ethane at r.t.p.

A. 24.2 cm3

B. 22.7 cm3

C. 23.9 dm3

D. 24.5 dm3

f

tatement. Then select

one

A. ue and the 2nd statement is a correct explanation

B. nd statement is NOT a correct

ut the 2nd statement is true.


Each question below consists of two separate statements. Decide whether each o


the second statement is a correct explanation of the first s

option from A to D according to the following table:

Both statements are tr


Both statements are true and the 2


C. The 1st statement is false b

Section 40.1

volume of any gas

must be the same.

s and

ame


198

Under the same temperature and

pressure, the molar

Molar volumes of different solid

liquids are unequal at the s

The unit of molar volume is mol dm3. occupied

by one mole of a substance.

199

Molar volume is the volume

ds DO NOT have

molar volume.

ficant effect on molar volume

of gases.

200

Solids and liqui Changes in temperature and pressure

have signi

on 40.2Secti

mole of iron at room

conditions.

l

t the same

201

1 mole of magnesium has equal

volume as 1

According to the Avogadro’s Law, equa

volumes of any substances contain the

same number of particles a


57


reacts with excess

carbon to give 1 mole of carbon

de at r.t.p..

en reacts with excess

carbon to give 100 cm3 of carbon

dioxide at r.t.p.

202

1 mole of oxygen

dioxi

100 cm3 of oxyg

According to the Avogadro’s Law, e

volumes of all gases contai

203

1 dm3 of H2 and 1 dm3 of O2 DO NOT

contain the same number of molecules

at 100C and 2 atm.

qual

n the same

number of molecules only at room


Section 40.3

204

A gas with greater molar mass

occupies a greater volume.

ined by measuring the volume of

one mole of the gas and its density at

r.t.p.

The molar mass of a gas can be

determ

The volume occupied by 1 mol of

is 24.0 dm3.

The molar volume of any gas is about

24.0 dm3 mol1 at r.t.p.

205

steam

The molar volume of water is 0.018

m3 mol1 if its density is 1 g cm3.

Molar mass of water is 18.0 g mol1.

206

d

Kinetics MCQ

Documents

rate of reaction

average reaction rate

instantaneous rate

reaction of potassium

displacement reaction

chemical reaction

slowest rate

cm3 s1