1
1 mark
1 markThe rate of a reaction was monitored by recording the volume of gas produced every 5 seconds.
What is the mean rate of reaction in the first 10 seconds of the reaction, in cm3/s?
2.9
3.0
3.5
2.5
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Rate of Reaction (Cambridge O Level Chemistry)
Exam Questions
10 hours75 questions21 mark
A student was measuring the rate of reaction using the apparatus in the diagram.
What reaction is the student studying?
CaO + H2SO4 → CaSO4 + H2O
Mg(OH)2 + 2HCl → MgCl2 + 2H2O
Fe + H2SO4 → FeSO4 + H2
KCl + AgNO3 → KNO3 + AgCl
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31 mark
A student was investigating the rate of reaction between iron and a solution of sulfuric acid. Two experiments were performed, P and Q, in which the volume of hydrogen was recorded at regular intervals.
Which change could explain the difference in results between P and Q?
The student added a catalyst in P.
Larger pieces of iron were used in P.
Less concentrated acid was used in P.
Larger quantities of both reactants are used P.
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11 mark
A student was investigating the rate of reaction between a solid base and a solution of sulfuric acid. Two experiments were performed, S and T, in which the mass of the reaction flask was recorded as shown in the graph.
Which of the following changes could explain the difference in results between S and T?
The sulfuric acid is less concentrated in T.
The sulfuric acid is more concentrated in T.
A higher temperature is used in S.
Larger sized particles are used in T.
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21 mark
Which graph correctly shows the effect of increasing the temperature on the rate of reaction between magnesium and sulfuric acid in which neither reactant runs out?
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31 mark
A student reacts a metal carbonate with nitric acid and measures the volume of carbon dioxide gas released at regular intervals. The results of the experiment are shown in the graph.
Between which two measurements was the reaction the fastest?
0 and 2 minutes
2 and 4 minutes
4 and 6 minutes
10 and 12 minutes
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41 mark
1 markMagnesium metal reacts with an excess of hydrochloric acid solution to form magnesium chloride and hydrogen:
Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g)
Which of the following will not increase the rate of this reaction?
Increase the temperature of the acid
Increase the surface area to volume ratio of the pieces of magnesium
Increase the concentration of the hydrochloric acid
Increase the volume of hydrochloric acid solution used
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51 mark
Catalysts are often used in chemical reactions.
Which letter represents two correct features of catalysts?
| Feature 1 | Feature 2 | |
| A | Lower activation energy for the reaction | More products made in total |
| B | Alternative pathway for the reaction is provided | Not used up over the course of the reaction |
| C | Makes industrial processes cheaper | Metal catalysts are cheap to buy |
| D | Reduce the overall energy change of the reaction | Can be present in biological systems as enzymes |
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61 mark
Which changes will speed up a chemical reaction?
| 1 | decreasing the pressure in a reaction between gases |
| 2 | increasing the size of the solid particles in a reaction involving solids |
| 3 | increasing the temperature of any reaction |
| 4 | increasing the concentration of a solution |
1 and 3
2, 3 and 4
3 and 4 only
4 only
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71 mark
Magnesium reacts with dilute sulfuric acid.
Mg(s) + H2SO4(aq) MgSO4(aq) + H2(g)
Two experiments are carried out at 25°C.
experiment 1 24.0 g of powdered magnesium is reacted with 100 cm3 of 1.0 mol / dm3 sulfuric acid.
experiment 2 24.0 g of powdered magnesium is reacted with 50 cm3 of 2.0 mol / dm3 sulfuric acid.
During each experiment the volume of hydrogen produced is measured. The results are plotted on a graph.
Which graph is correct?
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81 mark
In four separate experiments, 1, 2, 3 and 4, nitric acid is added to an excess of marble pieces and the volume of carbon dioxide gas formed is measured.
In all four experiments the same volume of nitric acid is used.
The concentration, or temperature, or both concentration and temperature of the nitric acid, are changed.
The results of the experiments are shown on the graph.
Which statement is correct?
A lower concentration of acid is used in experiment 3 than in experiment 1.
Experiment 4 is faster than experiment 3.
The acid used in experiment 2 is of a lower concentration than in experiment 1.
The temperature of the acid is the same in experiments 1 and 2.
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11 mark
A student was investigating the rate of reaction between acid and metals. The experimental set-up is shown below.
Which test tube would give the quickest reaction?
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21 mark
The graph shows the results of two separate reaction rate investigations using excess calcium carbonate and sulfuric acid.
Which statement explains the difference between the results?
The temperature was higher in experiment 2.
Experiment 2 was allowed more time to react.
Same volume of a more concentrated acid was used in experiment 2.
More calcium carbonate was used in experiment 2.
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31 mark
Which of the following statements explains how increasing temperature increases the rate of a reaction?
Increasing the temperature increases the kinetic energy of the particles so there are a smaller number of successful collisions.
Increasing the temperature increases the kinetic energy of the particles so there are a larger number of unsuccessful collisions.
Increasing the temperature decreases the kinetic energy of the particles so there are a larger number of successful collisions.
Increasing the temperature increases the kinetic energy of the particles so there are a larger number of successful collisions.
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41 mark
Which of the following statements best describes the activation energy of a reaction?
The minimum energy released when colliding particles react.
The minimum energy required for particles to react when they collide.
The maximum energy required for particles to react when they collide.
The maximum energy released when colliding particles react.
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51 mark
Which of the following statements correctly describes the effects of increasing concentration on the rate of a reaction?
Increasing the concentration increases the rate of reaction as there are more successful collisions between particles per unit time.
Increasing the concentration increases the rate of reaction as there is more space between particles.
Increasing the concentration increases the rate of reaction as there are more collisions between particles per unit time.
Increasing the concentration increases the rate of reaction as there are more collisions between particles at the beginning of the reaction.
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