it chem f5 topical test 1 (e)

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PAPER 1

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TOPICAL TEST 1: RATE OF REACTION

1 Which of the following changes can

be used to determine the rate of reaction?A pH and sizeB pH and colourC Pressure and sizeD Concentration and shape

2 Which of the rate of reaction is matched correctly?

Reaction Rate of reaction

A Photosynthesis Fast

B Formation of stalagmites

Fast

C Silver nitrate mixed with sodium chloride

Slow

D Combustion of magnesium and oxygen

Fast

3 The following chemical equation shows the reaction between excess marble and dilute nitric acid to produce carbon dioxide gas.

Which of the following graphs does not show the correct plot for the reaction?A

B

C

D

4 The following chemical equation shows the reaction between sodium carbonate and hydrochloric acid.

Which of the following changes is the most appropriate manner to determine the rate of reaction of the reaction?A The decrease in concentration of

hydrochloric acid per unit time.B The change of the temperature

per unit time.C The increase of water per unit

time.D The increase in volume of carbon

dioxide.

5 When excess sulphuric acid is used to react with 5 g of granulated zinc, the residue of zinc after 1.5 minutes is 1.25 g. The average rate of reaction is[Relative atomic mass = Zn : 65]A 0.0006 mol s–1 C 0.06 mol s–1

B 0.004 mol s–1 D 0.4 mol s–1

6 The graph in Diagram 1 shows the volume of carbon dioxide released when bromine reacts with some methanoic acid against time.

Diagram 1

Which of the following statements about the graph is true?A Carbon dioxide is produced at a

constant rate at t3.B The methanoic acid is used up at

t3.C The rate of reaction of methanoic

acid is the highest at t3.D There are more carbon dioxide

produced between t2 and t3

compared to the volume produced between t1 and t2.

7 Diagram 2 shows the graph of hydrogen gas liberated against time when zinc is reacted with hydrochloric acid.

Diagram 2

Which of the positions, A, B, C and D in the graph represents the instantaneous rate of reaction in 0.0 cm3 s–1?

8 The gradient of the curve at a given time in a graph of concentration of product against time tells us the information aboutA the average rate of the reaction.B the initial rate of the reaction.C the constant rate of the reaction.D the instantaneous rate of the

reaction.

9 Table 1 shows the volume of gas liberated when sodium carbonate reacts with hydrochloric acid.

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Time / s Volume of gas / cm3

0 0.0

30 1.8

60 4.6

90 7.7

120 10.8

150 13.6

180 15.6

210 17.5

240 18.7Table 1

What is the average rate of reaction from the 3rd minute to the 4th minute?A 0.10 cm3/sB 0.04 cm3/sC 0.05 cm3/sD 0.06 cm3/s

10 The combustion of carbon in excess oxygen produces carbon dioxide. 40 cm3 of gas is produced after the reaction is completed in 2 minutes. What is the average rate of the reaction?A 0.20 cm3 s–1 C 0.66 cm3 s–1

B 0.33 cm3 s–1 D 0.72 cm3 s–1

11 The initial rate of reaction for 1 g of small marble chip is higher than 1 g of large marble chip when reacting with 30 cm3 of 0.1 mol dm–3

hydrochloric acid. This is becauseA the large marble chip is tougher

than the small marble chip.B the total surface area of large

marble chip is larger than small marble chip.

C the total surface area of small marble chip is larger than large marble chip.

D the large marble chip is too heavy.

12 Curve P in the graph in Diagram 3 is generated when 5 g (excess) of zinc powder is added to 70.0 cm3 of 1.0 mol dm–3 hydrochloric acid in conical flask.

Diagram 3 In what condition, the curve Q can be produced?A 5 g of zinc powder + 50.0 cm3 of

1.0 mol dm–3 hydrochloric acidB 5 g of granulated zinc + 70.0 cm3

of 1.0 mol dm–3 hydrochloric acidC 5 g of zinc powder + 70.0 cm3 of

0.5 mol dm–3 hydrochloric acidD 5 g of zinc powder + 70.0 cm3 of

1.5 mol dm–3 hydrochloric acid

13 In an experiment, 40 cm3 of 0.5 mol dm–3 sodium thiosulphate solution is mixed with 5 cm3 of 1 mol dm–3 sulphuric acid at 28 C in a conical flask. Which of the following alterations will increase the rate of reaction?A Increase the temperature to 40 C.B Add 20 cm3 of water to the

mixture.C Use 40 cm3 of 0.2 mol dm–3

sodium thiosulphate.D Use a bigger conical flask.

14 In the following sets of experiment, the highest initial rate can be obtained fromA 4 g of magnesium ribbon + 50

cm3 of 0.1 mol dm–3 sulphuric acid at 25 C

B 4 g of granulated magnesium + 50 cm3 of 0.1 mol dm–3 sulphuric acid at 35 C

C 4 g of magnesium ribbon + 40 cm3 of 0.5 mol dm–3 sulphuric acid at 35 C

D 4 g of granulated magnesium + 40 cm3 of 0.5 mol dm–3 sulphuric acid at 35 C

15 Which of the following statements about catalyst is not true?A Catalyst is only needed in a small

amount to achieve a huge increase in reaction rate.

B Catalyst helps to increase the activation energy of the reaction.

C Positive catalyst plays a role in increasing the rate of a reaction.

D Negative catalyst is also known as inhibitor.

16 The following chemical equation shows the composition of hydrogen peroxide solution.

The rate of reaction decreases against time becauseA the pressure of the solution

decreases.B the concentration of oxygen

increases.C the production of water decreases

the concentration of solution.D the production of the products

increases the volume.

17 Diagram 4 shows the apparatus set-up to study the effect of concentration on the rate of reaction.

Diagram 4 Which of the following is the most appropriate method to determine the rate of reaction?A Record the time when the

solution starts changing colour.B Record the time when bubble is

formed in the solution.C Record the time taken for the

cross mark to disappear from view.

D Record the time taken for the solution to achieve 40 C.

18 The following chemical reaction shows the reaction of iron(II) sulphate solution with bromine water.

The change of colour from green to brown is faster when the mixture is heated. Which of the following do not contribute to the changes?A The frequency of effective

collisions increases.B The activation energy decreases.



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C The kinetic energy of the reactant’s molecules increases.

D The size of the molecules decreases.

19 Which of the following methods can help 25 kg of potatoes to be cooked faster?A Cook the potatoes in microwave.B Add salt to the potatoes.C Cook the potatoes in a pressure

cooker.D Steam the potatoes using hot

water.

20 The following chemical equation shows the reaction between magnesium ribbon and dilute sulphuric acid.

The liberation of hydrogen gas can be slowed down by

I using magnesium powder.II reducing the temperature of

sulphuric acid.III reducing the pressure on the

reaction.IV decreasing the concentration of

sulphuric acid.A I and II onlyB I and III onlyC II and IV onlyD II, III and IV only

21 Which of the following sets of reactants for the reaction between sodium thiosulphate and sulphuric acid will result in the maximum rate of reaction?

Sulphuric acid Sodium thiosulphate

Volume/cm3

Concentration/mol dm–3

Volume/cm3

Concentration/mol dm–3

A 30 0.4 25 0.5

B 25 0.6 30 0.5

C 30 0.6 25 0.5

D 25 0.8 30 0.5

22 Dilute ethanoic acid was reacted with excess zinc powder at 28 C, 34 C, 39 C and 44 C. The volume of hydrogen gas evolved was shown in Diagram 5.

Diagram 5 Which of the following curves represents the volume of gas measured at 39 C?A R C TB S D U

23 The reacting condition for the reaction between zinc and hydrochloric acid is shown below.

Which of the following factors do not affect the rate of reaction?A The temperature of the reaction.B The concentration of the acid.C The amount of copper(II)

sulphate solution used.D The excess mass of zinc.

24 Which of the following does not explain the meaning of effective collision?A The collision that produce a

chemical reaction.B The collision in correct

orientation.C The collision that successfully

overcome the activation energy.D The collision with the low kinetic

energy.

25 In the reaction between sulphuric acid and sodium thiosulphate, sulphur precipitate will be formed at a faster rate if higher concentration of sulphuric acid is used becauseA the frequency of collisions

increases.B the number of particles per unit

volume decreases.C the ions move faster.D the activation energy decreases.

26 Diagram 6 shows an energy level for the reaction between hydrogen gas and oxygen gas.

Diagram 6What is the activation energy for this reaction?A 510 kJB 320 kJC 190 kJ D 830 kJ

27 Diagram 7 shows the energy level for the reaction P Q R.

Diagram 7 Which of the following represents the activation energy?A SB TC U D W

28 Which of the following does not explain the increase of rate of reaction between sodium thiosulphate and hydrochloric acid when the experiment is carried out at a higher temperature?A The frequency of effective

collision decreases.B The effective collisions frequency

increases.C The kinetic energy of the

reactants increases.D Number of particles with the

minimum activation energy increases.

29 Which of the following matches regarding the effect of catalyst is not true?

Reaction without catalyst

Reaction with

catalyst

A Rate of Slower Faster



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reaction

B Force of collision

Similar Similar

C Activation energy

Less More

D Frequency of effective collision

Less More

30 The chemical equation below shows the decomposition of hydrogen peroxide that involved the black copper (II) oxide as the catalyst.

What can you observed from the boiling tube at the end of the reaction?I A white solid.

II A black solid.III A colourless solution.IV Black solid dissolved.A I and III onlyB I and IV onlyC II and III onlyD III and IV only

31 Diagram 8 shows the energy level of a reaction.

Diagram 8 Which of the following is true about the diagram?

A The activation energy is W kJ.B The activation energy is (X + W) kJ.C W kJ energy is absorbed by the

reaction.D The reaction is exothermic.

32 Why does the food that is kept in refrigerator last longer?A The carbon dioxide in the

refrigerator kills the microorganism in food.

B Bacteria is inactive under lower temperature.

C The high pressure slows down the decaying rate of the food.

D There is no sufficient oxygen in the refrigerator.

1 An experiment that involves the decomposition of sodium

chlorate(I) solution in the presence of manganese(IV) oxide as a catalyst will produce oxygen gas.The results obtained are as follow:

Time / s Total volume of gas / cm3

0 0.0

20 90

40 155

60 195

80 225

100 245

120 250

140 250

(a) Plot a graph of total volume of oxygen against time on graph paper.

[2 marks](b) From the graph,

(i) determine the average rate of reaction in the first 50 seconds.

___________________________________________________

[2 marks](ii) determine the average rate of reaction from 50

seconds to 90 seconds.

___________________________________________________

[2 marks](iii) determine the rate of reaction at 40 seconds.

___________________________________________________

[2 marks ]

(c) Write a chemical equation for the reaction.

________________________________________________________

[1 mark](d) At what time will the sodium chlorate(I) solution

completely decompose?

________________________________________________________

[1 mark](e) What is the function of manganese(IV) oxide as a

catalyst?

________________________________________________________

[1 marks]

2 Four experiments are carried out to investigate one of the factors that affect the rate of reaction. In each of the experiments, 40 cm3 of 0.2 mol dm–3 sodium thiosulphate, Na2S2O3 solution was allowed to react with 4 cm3 of 1.0 mol dm–3 sulphuric acid. The results are recorded in Table 1.

Experiment Temperature/°C

Time taken for the ‘X’

mark to disappear from view,

t/s

,

/s–1

1 28 57

2 40 38

3 50 24

4 60 15Table 1


PAPER 2 SECTION A

1

Time taken

1

t


PAPER 1

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(a) What factor is being investigated in these experiments?

________________________________________________________

[1 mark](b) Draw a labelled diagram of the set-up of the apparatus.

[2 marks](c) Complete Table 1.

________________________________________________________

[1 mark](d) Plot a graph of temperature of Na2S2O3 against

.

[1 mark ](e) Based on the graph in (d), what is the conclusion that

can be made from this investigation?

________________________________________________________

[2 marks](f) Write the ionic equation for the reaction.

________________________________________________________

[1 mark]

3 Two sets of experiments are carried out to study the effect of concentration to the rate of reaction.

Experiment Mixture of reactants

1 Excess Zn powder + 50 cm3 of 0.1 mol dm–3

HCl

2 Excess Zn powder + 25 cm3 of 0.15 mol dm–3 HCl

(a) Draw a labelled diagram for the set-up apparatus to collect the hydrogen gas.

[2 marks](b) Calculate the number of moles of HCl in Experiment 1

and 2.

[2 marks](c) Match the experiments with the curves from the graph.

(i) Experiment 1:

___________________________________________________

(ii) Experiment 2:

___________________________________________________

[2 marks](d) Calculate the average rate of reaction of Experiment 1 in

(i) cm3 s–1

(ii) mol s–1

[2 marks](e) What can you do to increase the rate of reaction for

Experiment 1?

________________________________________________________

[2 marks]

4 Three experiments are carried out to investigate the factors affecting the rate of reaction of magnesium under different condition. Table 2 shows the different reacting condition and time taken to collect 60 cm3 of gas liberated.

Experiment Reactants Time / s

A Excess magnesium ribbon + 30 cm3 of 1.5 mol dm–3 hydrochloric acid

50

B Excess magnesium powder + 30 cm3

of 1.5 mol dm–3 hydrochloric acid35

C Excess magnesium powder + 30 cm3

of 1.5 mol dm–3 sulphuric acid25

Table 2

(a) (i) Write the chemical equation for the reaction that has the highest rate of reaction.

___________________________________________________

[1 mark](ii) Calculate the average rate of reaction for

Experiment B and C.

[2 marks ](iii) Why is the rate of reaction of Experiment C is

higher than B?

___________________________________________________

[1 mark](b) Explain why the time taken for Experiment B is shorter

than Experiment A by using the collision theory. .


1

Time


PAPER 1

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________________________________________________________

[3 marks](c) What will happen if the gas evolved is tested with

glowing wooden splint?

________________________________________________________

[1 mark](d) Name of catalyst that can be used to increase the rate of

reaction.

________________________________________________________

[1 mark](e) Substance X is used to replace magnesium in

Experiment C to produce carbon dioxide and water. What can substance X most likely be?

________________________________________________________[1 mark]

5 The following apparatus are set up to investigate the effect

of catalyst on rate of reaction.

I II

(a) (i)

Complete the table.[4 marks]

(ii) Will the mass of manganese(IV) oxide powder decrease after the reaction?

[1 mark](b) (i) Plan an experiment and make amendments to the

arrangements of apparatus in Set II to determine the effect of amount of catalyst on the rate of reaction.

[12 marks](ii) Sketch a graph to distinguish the effect of using

different amount of catalyst.

[3marks]

6 (a)

The graph above shows the production of ammonia at two different pressures.

(i) Which of the curve is obtained at higher pressure?

[1 mark](ii) What is the name of the production of ammonia

in industrial process? Name the catalyst used in this process.

[2 marks](iii) Explain how will the increase of pressure affect

the rate of reaction..

[4 marks](iv) Will the increase in pressure for the reaction that

involves aqueous reactant result in higher rate of reaction?

[1 mark](v) Give three other factors that can increase the

rate of reaction without changing the amount of product.

[3 marks](vi) How does the use of pressure cooker speed up

cooking?

[1 mark](b)


SECTION B

Set Observation

I

II


PAPER 1

SULIT

NAMA: _______________________________________________ TINGKATAN: ______________


Explain the statement above based on collision theory and give suitable examples. [8 marks]

7 (a) What are the main ideas about collision theory?

[2 marks](b) Explain the meaning of activation energy by sketching

the energy profile diagrams.

[6 marks]

(c) Give four factors that can increase the rate of reaction and explain how these factors take place in term of collision theory.

[12 marks]8 (a)

The graph shown above are the plots of volume of hydrogen gas produced against time for two sets of experiments.

Set P: 3 g of zinc powder + 30 cm3 of 0.1 mol of sulphuric acid

Set Q: 3 g of zinc powder + 30 cm3 of 0.1 mol of sulphuric acid + copper(II) sulphate solution.

(i) Does the graph represent the result of the two experiment correctly? If your answer is no, please sketch the correct graph. [4 marks]

(ii) Write the chemical equation for the experiment[1 mark]

(iii) What is the use of copper(II) sulphate solution in Set Q? [4 marks]

(b) (i) What is meant by catalyst?[2 marks]

(ii) Name the catalyst that are used in Ostwald process and Contact process.

[4 marks](iii) Describe the characteristics of catalyst.

[10 marks]

1 Diagram 1.1 shows the six sets, I, II, III, IV, V and VI of apparatus set-up for an experiment to investigate the effect of temperature on the rate of reaction between sodium thiosulphate solution and sulphuric acid. 50 cm3

of 0.2 mol dm–3 of sodium thiosulphate solution is poured into a conical flask and is heated up to 30 °C. The conical flask is then placed on a paper marked with ‘X’ as shown in Diagram 1.1. 5 cm3 of 1 mol dm–3 of sulphuric acid is added immediately to the sodium thiosulphate solution and the mixture is stirred. The time taken for the mark ‘X’ to disappear from sight is recorded.

Diagram 1.1The experiment is repeated using sodium thiosulphate at 35 °C, 40 °C, 45 °C, 50 °C and 60 °C. Diagram 1.2 shows the reading of the stop-watch in each experiment.

(a) (i) Record the stop-watch readings in the space provided in Table 1.

[3 marks]

Set I Set II


SECTION C

PAPER 3

1

time


PAPER 1

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At 30 °C________ s

At 35 °C________ s

Set III

At 40 °C________ s

Set IV

At 45 °C________ s

Set V

At 50 °C________ s

Set VI

At 60 °C________ s

Diagram 1.2

(ii) Calculate for each experiment. Construct a table to record and show all the data which include temperature, time and for the experiments.

[3 marks]

(iii) Plot a graph of against temperature.

[3 marks](b) State a hypothesis for this experiment.

[3 marks](c) State the operational definition of the rate of reaction

based on this experiment.

[3 marks](d) State the following variables in this experiment.

1. Manipulated variables2. Responding variables

3. Constant variables [3 marks]

(e) Based on the graph you have drawn, predict the time taken for the mark ‘X’ to disappear from sight if the temperature of sodium thiosulphate solution is 45 °C.

[3 marks](f) If 50 cm3 of 0.10 mol dm–3 of sodium thiosulphate is

used in Experiment 1, predict the time taken for the ‘X’ mark to disappear from sight. Explain your answer.

[3 marks](g)

Based on situation above, explain this observation.

[3 marks](h) In another experiment, the effect of concentration on the

rate of reaction is studied. 50 cm3 of 0.08 mol dm–3 sodium thiosulphate solution is prepared from 0.2 mol dm–3 sodium thiosulphate solution. Calculate the volume of 0.2 mol dm–3 sodium thiosulphate solution used.

[3 marks](i) Describe the steps to prepare the sodium thiosulphate

solution in (h) accurately.[3 marks]

2

Using the suitable apparatus and materials, you are required to design a laboratory experiment to investigate the effect of the size of reactant on the rate of reaction.Your planning must include the following items:(a) Statement of the problem.(b) All the variables.(c) Hypothesis. (d) Lists of materials and apparatus.(e) Procedure.(f) Tabulation of data.

[17 marks]


1

Time

1

m

it chem f5 topical test 1 (e)

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