HOD: __________

AD/Coordinator: __________

REVISION WS

Chemistry
Subject: Class and Section: IX G Date:

Name: _________________________________________________ Topic: Rate of reaction

1 Hydrogen peroxide decomposes to form water and oxygen. This reaction is catalysed by
manganese(IV) oxide.

2H2O2(aq) → 2H2O(l) + O2(g)

The rate of this reaction can be investigated using the following apparatus.

oxygen gas

aqueous hydrogen peroxide

and manganese(IV) oxide

40 cm3 of aqueous hydrogen peroxide was put in the flask and 0.1 g of small lumps of manganese(IV)
oxide was added. The volume of oxygen collected was measured every 30 seconds. The results
were plotted to give the graph shown below.

volume of
oxygen

0
0 t t2 t3
1
time

CSI_AY_2024-25_IGCSE IX G_ Chemistry _WS

 (a)
a) How do the rates at times t1, t2 and t3 differ?

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....................................................................................................................................... [2]

(ii) Explain the trend in reaction rate that you described in (a)(i).

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....................................................................................................................................... [2]

(b) The experiment was repeated using 0.1 g of finely powdered manganese(IV) oxide. All the
other variables were kept the same.

(i) On the axes opposite, sketch the graph that would be expected. [2]

(ii) Explain the shape of this graph. ..........................................................................................

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....................................................................................................................................... [2]

(c) Describe how you could show that the catalyst, manganese(IV) oxide, was not used up in the
reaction. Manganese(IV) oxide is insoluble in water.

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.............................................................................................................................................. [4]

[Total: 12]

CSI_AY_2024-25_IGCSE IX G_ Chemistry _WS

 2 One of the factors which determine the reaction rate of solids is particle size.

(a) A mixture of finely powdered aluminium and air may explode when ignited.
An explosion is a very fast exothermic reaction. This causes a large and sudden increase
in temperature.

Explain each of the following in terms of collisions between reacting particles.

(i) Why is the reaction between finely powdered aluminium and air very fast?

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.............................................................................................................................. [2]

(ii) Explain why for most reactions the rate of reaction decreases with time.

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(iii) Suggest an explanation why the rate of reaction in an explosion could increase
rather than decrease with time.

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.............................................................................................................................. [3]

(b) (i) Give another example of a substance other than a metal which, when finely
powdered, might explode when ignited in air.

.............................................................................................................................. [1]

(ii) Describe a simple test-tube reaction which shows the effect of particle size on the
rate at which a solid reacts with a solution.

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....................................................................................................................................

.............................................................................................................................. [3]

[Total: 11]

CSI_AY_2024-25_IGCSE IX G_ Chemistry _WS

3 The speed (rate) of a chemical reaction depends on a number of factors which include
temperature and the presence of a catalyst.

(a) Reaction speed increases as the temperature increases.

(i) Explain why reaction speed increases with temperature.

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.............................................................................................................................. [3]

(ii) Reactions involving enzymes do not follow the above pattern.

The following graph shows how the speed of such a reaction varies with temperature.

speed

temperature

Suggest an explanation why initially the reaction speed increases then above a
certain temperature the speed decreases.

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.............................................................................................................................. [2]

(b) An organic compound decomposes to give off nitrogen.

C6H5N2Cl (aq) → C6H5Cl (l) + N2(g)

The speed of this reaction can be determined by measuring the volume of nitrogen
formed at regular intervals. Typical results are shown in the graph below.

volume of
nitrogen

0
0 time

(i) The reaction is catalysed by copper.

Sketch the graph for the catalysed reaction on the diagram above. [2]
 (ii) How does the speed of this reaction vary with time?

.............................................................................................................................. [1]

(iii) Why does the speed of reaction vary with time?

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.............................................................................................................................. [2]

(c) Catalytic converters reduce the pollution from motor vehicles.

oxides of nitrogen less harmful gases

and carbon monoxide to atmosphere

catalysts: rhodium,
platinum, palladium

(i) Describe how carbon monoxide and the oxides of nitrogen are formed in car engines.

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.............................................................................................................................. [4]

(ii) Describe the reaction(s) inside the catalytic converter which change these pollutants
into less harmful gases. Include at least one equation in your description.

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.............................................................................................................................. [3]

[Total: 17]

CSI_AY_2024-25_IGCSE IX G_ Chemistry _WS

 (c) The speed (rate) of reaction between an organic halide and water can be measured by
the following method.

A mixture of 10 cm3 of aqueous silver nitrate and 10 cm3 of ethanol is warmed to 60 °C.
Drops of the organic halide are added and the time taken for a precipitate to form is
measured.

Silver ions react with the halide ions to form a precipitate of the silver halide.

Ag+(aq) + X–(aq) → AgX(s)

Typical results for four experiments, A, B, C and D, are given in the table.

experiment organic halide number of drops time / min

A bromobutane 4 6
B bromobutane 8 3
C chlorobutane 4 80
D iodobutane 4 0.1

(i) Explain why it takes longer to produce a precipitate in experiment A than in B.

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.............................................................................................................................. [2]

(ii) How does the order of reactivity of the organic halides compare with the order of
reactivity of the halogens?

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(iii) Explain why the time taken to produce a precipitate would increase if the experiments
were repeated at 50 °C.

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.............................................................................................................................. [3]

[Total: 15]

CSI_AY_2024-25_IGCSE IX G_ Chemistry _WS

5 Hydriodic acid, HI(aq), is a strong acid. Its salts are iodides.

(a) It has the reactions of a typical strong acid. Complete the following equations.

(i) ............Li + ............HI → ........................ + ................... [1]

(ii) zinc hydriodic .......................... ..........................

+ → + + .........................
carbonate acid .......................... ..........................
[1]

(iii) MgO + ............HI → ................... + ................... [1]

(b) Two of the reactions in (a) are acid / base and one is redox. Which one is redox? Explain
your choice.

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...........................................................................................................................................

..................................................................................................................................... [2]

(c) Describe how you could distinguish between hydriodic, HI(aq), and hydrobromic, HBr(aq)
acids, by bubbling chlorine through these two acids.

result with hydriodic acid ..................................................................................................

result with hydrobromic acid ....................................................................................... [2]

CSI_AY_2024-25_IGCSE IX G_ Chemistry _WS

 (d) 20.0 cm3 of aqueous sodium hydroxide, 2.00 mol / dm3, was placed in a beaker. The
temperature of the alkali was measured and 1.0 cm3 portions of hydriodic acid were
added. After each addition, the temperature of the mixture was measured. Typical results
are shown on the graph.

temperature

18.0 cm3 volume of

acid added

NaOH(aq) + HI(aq) → NaI(aq) + H2O(l)

(i) Explain why the temperature increases rapidly at first then stops increasing.

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.............................................................................................................................. [2]

(ii) Suggest why the temperature drops after the addition of 18.0 cm3 of acid.

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(iii) In another experiment, it was shown that 15.0 cm3 of the acid neutralised 20.0 cm3 of
aqueous sodium hydroxide, 1.00 mol / dm3. Calculate the concentration of the acid.

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.............................................................................................................................. [2]

[Total: 12]

CSI_AY_2024-25_IGCSE IX G_ Chemistry _WS