15891064-rate-of-reaction

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RATE OF REACTION/F5/HST

RATE OF REACTION

1. Concept Map

2. Rate of reaction

(a) Rate of reaction is the at which reactants react to form products in a

chemical reaction.

(b) Not all chemical reactions have the same rate of reaction, some reactions occur

with rate of reaction that is .., and some reactions occur

with rate of reaction that is ...

(c) Examples of fast chemical reaction:

Type of reaction Example of chemical equation for the reaction

Neutralisation

Double decomposition

reaction

HST/RATE OF REACTION/SMKPB1

Rate of reaction

Observable changes in chemical reaction

Average rate of reaction Rate of reaction at a given

Factors affecting rate of reaction

Collision Theory to

explain factorsaffecting rate of

reaction


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Acid with active metals

Combustion of magnesium

(d) Examples of slow chemical reaction.

Corrosion of iron

Photosynthesis

Reaction of hydrochloric

acid with sodiumthiosulphate solution.

(e) Time taken for a fast chemical reaction is and the time taken forslow

chemical reaction of. Hence the rate of reaction is to

time taken for the reaction.

(f) The rate of reaction can be determined by measuring the time taken for an observablechemical change to occur.

Rate of reaction = Observable chemical changeTime taken

(g) The observable chemical changes in a chemical reaction are

(i) .

(ii)

(iii) .

(iv)

(v) ..


Rate of reaction

..


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(h) Rate of reaction can be defined as the rate of change of volume of gas producedper unit time.

Rate of reaction = Change in volume of gas producedTime taken

= cm3

s-1

(i) Example: If 50.0 cm3 of hydrogen gas is collected in 20 seconds during a chemical

reaction between magnesium and dilute hydrochloric acid . What is the rate of reaction?

Rate of reaction = = cm3 s-1

(ii) Example: If 5.0 gram of magnesium ribbon reacts completely with dilutehydrochloric acid in 25s, what is the rate of reaction?

Rate of reaction = = g s-1.

3. To determine the rate of reaction from graph.

(a) For a chemical reaction, if the concentration of reactants or mass of reactant is

plotted against the time, sketch the graph produced:

(b) For a chemical reaction, if the concentration of products or the volume of gasreleased is plotted against time, sketch the graph is produced.


Concentration of

reactant / mol

dm-3

Mass of

reactant/ g

Time/s Time/s

Time/s Time/s

Concentration ofproduct / mol dm-

3

Volume ofgas/cm3

Vmax


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(c) If the concentration of reactant is plotted against 1/time, sketch the graph produced.

(d) In a chemical reaction involving release of a gas, it is easier to determine the rate of

reaction by measuring the .. at a certain time interval.

(f) There are 2 methods to determine the rate of reaction, namely

(i) average rate or overall rate of reaction

Average rate of reaction = Total volume of gas released

Time taken

= V cm3 s-1 or cm3 min-1

t

(ii) rate of reaction at a given time.To determine the rate of reaction at a given time t1 s on the graph at point

M, the following steps are taken.

- Draw a tangent at the point M on the graph.- Draw a right angle triangle using the tangent as hypotenuse.

- Determine the gradient of the tangent.

- Rate of reaction at t1 s = y/x cm3 s-1

Example:


Concentration ofreactant / mol

dm-3

1/time , s-1

t1 t2 t3 Time/s

Volume of

gas/cm3

Rate of reaction at t1=



M


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Example: To determine the rate of reaction between zinc and dilute hydrochloricacid.

Aim of experiment: To investigate..

Apparatus:

Material:

Procedure:

(diagram)

(i)

(ii)

(iii)

(iv)

(v)

(vi)

(vii)



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Result:

Time/minute 0.0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0

Burette

reading/cm3

49.0

0

36.0

0

25.0

0

17.0

0

11.00 8.00 6.00 5.00 4.00 4.00 4.00

Volume of

gas

collected/cm3

0.00 13.0

0

24.0

0

32.0

0

38.0

0

41.0

0

43.0

0

44.0

0

45.0

0

45.0

0

45.00

Discussion:1. Plot a graph of volume of gas collected against time of reaction.

2. From the graph, calculate the(i) overall average rate of reaction.

(ii) rate of the reaction in the first 3 minutes.

(iii) rate of reaction in the second minute

(iv) rate of reaction at(a) 1 minute

(b) 2 minute

(c) 3 minute

3. Compare the rate of reaction obtained in 2(iv). Explain your answer.



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4. Write a balance chemical equation of the reaction between zinc and hydrochloric acid.

5.What is the name of the gas released and suggest a test for the gas.

Conclusion:

4. Factors affecting rate of reactionName the factors that affect the rate of reaction..

(A)

(B)

(C)

(D)

(E)

(A) Effect of total surface area of reactant on the rate of reaction.

(a) The smaller the size of particle of solid reactant the larger the surface area of reactantexposed, hence the higher is the rate of reaction.

Give 3 examples for the above statement.

(i) Cube sugar dissolves slower than that of fine sugar of the same mass in same amount

of water.

(ii) Minced meat cooks faster that solid piece of meat of the same mass.

(iii) Powdered zinc reacts faster than granulated zinc of the same mass with hydrochloricacid of the same volume and concentration.



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(b) Experiment to investigate the effect of total surface area of calcium carbonate on

the rate of reaction

Problem statement:

Hypothesis:

Variables:

(i) manipulate variable:

(ii) responding variable:

(iii) fixed variable:

Materials:

Apparatus:

Procedure:

(i)

(ii)

(iii)

(iv)

(v)



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(vi)

(vii)

(viii)

Results:

(i) Experiment I using large marble chips:

Time/ minute 0.0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 5.5

Burettereading/cm3

49.50

45.20

42.0

39.00

36.50

34.00

31.80

29.50

27.80

26.20

24.50

23.50

Volume of

gascollected/cm3

(ii) Experiment II using crushed marble chips:

Time/ minute 0.0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 5.5

Burette

reading/cm349.0

0

39.0

0

33.0

0

28.5

0

25.0

0

21.5

0

19.0

0

16.7

0

14.7

0

13.0

0

11.50 10.00

Volume of

gascollected/cm3

1. Plot the graph of total volume of gas collected against time taken for the reaction forexperiment I and II on the same axes.

2. Based on the graph , calculate

(a) the overall rate of rate of reaction for the first 5 minutes of the reaction between

hydrochloric acid and

(i) large marble chips:

(ii) crushed marble chips



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(b) The rate of reaction at 2.5 minute for

(i) large marble chips:

(ii) crushed marble chips:

3. Based on your answers in 2(a) and 2(b) , how does the rate of reaction differ?

4. What is the factor that causes the difference in rate of reaction?

5. Write a balanced chemical equation for the reaction between calcium carbonate andhydrochloric acid.

6. Explain why does the rate of reaction decreases with increase of time.

7. If both reactions are allowed to react until completion, is the total volume of gas

collected the same? Explain your answer.

8. If the marble chips used in the experiment is in excess, what is the maximum total

volume of gas collected?

[ 1 mole of gas at room temperature occupies a volume of 24dm3]

Conclusion:



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5. The effect of concentration of reactant on the rate of reaction.

(a)When concentration of reactant increases, the rate of reaction increases.

Give one example for the above statement.

(b) Experiment to investigate the effect of concentration of sodium thiosulphate with

hydrochloric acid on the rate of reaction

Problem statement:

Hypothesis:

Variables:(i) manipulated variable:



Procedure:

(diagram)

(i)

(ii)

(iii)

(iv)

(v)



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(vi)

(vii)

Results:

Experiment 1 2 3 4 5

Volume of 0.2moldm-3 sodium

thiosulphate solution, V1 cm3

45 40 35 30 25

Volume of distilled water added/cm3 0.0 5.0 10.0 15.0 20.0

Volume of 1.0mol hydrochloric acid

added/cm35.0 5.0 5.0 5.0 5.0

Total volume of reactant /cm3 50.0 50.0 50.0 50.0 50.0

Concentration of sodiumthiosulphate solution used/moldm-3

Time taken/s 16 20 27 41 83

1/time , s-1

1. Plot the graph of concentration of sodium thiosulphate solution used against time takenfor the reaction.

2. Plot the graph of concentration of thiosuphate solution used against 1/time.

3. What does the value of 1/time represents?

4. Based on your graph, state the relationship between

(i) the concentration of sodium thiosulphate and the time taken for the reaction.

(ii) the rate of reaction and the concentration of sodium thiosulphate solution.

5. What is colour of the precipitate formed and name the precipitate.

6. What is the time taken for the mark X to disappear if the concentration of sodium

thiosulphate solution used is 0.10 mol dm-3?

7. Write a balanced chemical equation for the reaction in this experiment.



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8. Write an ionic equation for the reaction in this experiment.

9. If dilute sulphuric acid of the same concentration is used to replace hydrochloric acid

in this experiment, predict the rate of reaction and explain your answer.

Conclusion:

6. The effect of temperature on rate of reaction.

(a) Increase in temperature of reaction, increases the rate of reaction.

Give two examples for the above statement.(i)

(ii)

(b) Experiment to investigate the effect of temperate on the rate of reaction between

thiosulphate solution and dilute hydrochloric acid.

Problem statement:

Hypothesis:

Variables:(i) manipulate variable:



Procedure:



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(diagram)

(i)

(ii)

(iii)

(iv)

(v)

(vi)

(vii)

(viii)

Results:

Experiment 1 2 3 4 5

Temperature/oC 30 35 40 45 50

Time taken/s 55 48 42 37 33

1/time, s-1



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1. Plot the graph of

(i) temperature against time and

(ii) temperature against 1/time.

2. Based on your graph, what is the relationship between rate of reaction with

temperature.

3. Write a balance chemical equation for the reaction of this experiment.

4. why is the volume of sodium thiosulphate solution and hydrochloric acid fixed for

each experiment?

5. What is the time taken for the mark X to disappear when the temperature is 60oC?

Conclusion:

7. Effect of catalyst on the rate of reaction.

(a) A catalyst is a substance which added to a chemical reaction can . the rate of

reaction and itself remains . at the end of the reaction.

(b) A catalyst does not .. in a chemical reaction. It only

.. the rate of reaction if it is a positive catalyst, and

the rate of reaction if it is a negative catalyst.

(c) Example: When copper(II) sulphate solution is added into a reaction between zinc

and hydrochloric acid, the rate of reaction increases but the final quantity of hydrogen

produced is the same the reaction of zinc with hydrochloric acid without copper(II)sulphate solution.

Sketch the graphs of volume of hydrogen gas against time for comparison of reaction ofzinc and hydrochloric acid with catalyst and without catalyst .



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(d) Experiment to investigate the effect of catalyst on the rate of reaction fordecomposition of hydrogen peroxide solution.

Problem statement:

Hypothesis:

Variables:

(i) manipulated variable:



Apparatus:

Materials:

Procedure:

(i)

(ii)


Time/s

Volume of

hydrogen

released/cm3


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(iii)

(iv)

(v)

Observation:

Test tube Observation

A

B

Discussion:

1. What is the effect of manganese(IV) oxide on the decomposition of hydrogen peroxide

solution?

2. What is the function of manganese(IV) oxide in this experiment?

3. Write a balanced chemical equation for the reaction in this experiment.

4. Will the mass of manganese(IV) oxide change at the end of the reaction in test tube B?

Conclusion:

(e) Experiment to investigate the effect of the amount of catalyst on the rate of

reaction for decomposition of hydrogen peroxide solution.

Problem statement:

Hypothesis:

Variables:(i) manipulated variable:



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Apparatus:

Materials:

Procedure:

(i)

(ii)

(iii)

(iv)

(v)

(vi)

(vii)

(viii)

Results:



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(a) Experiment 1, using 0.2g of manganese(IV) oxide

Time/s 0.0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 5.5 6.0

Burette

reading/cm3

49.70 48.70 47.10 45.70 44.20 43.20 42.00 41.10 40.20 39.50 39.00 38.40 38.00

Volume of

gas cm3

(b) Experiment II, using 0.6g of manganese(IV) oxide

Time/s 0.0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 5.5 6.0

Burette

reading/cm349.00 43.60 40.50 38.00 36.00 34.50 33.00 31.70 30.50 29.70 29.00 28.20 28.00

Volume ofgas cm3

1. Plot the graph of total volume of gas against time for experiment I and experiment II

on the same axes.

2. Based on your graph, calculate the rate of reaction at 120 seconds for each of the

reaction .(i) Experiment I:

(ii) Experiment II:

3. How did the rates of reaction in experiment I and II differ?

4. Which experiment shows the higher rate of decomposition of hydrogen peroxide?

5. If both experiments are allowed to proceed until completion, is the total volume of gascollected in both experiments the same? Explain your answer.

Conclusion:

(f) Application of catalyst in industry.



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Most catalysts are transition elements or compounds of transition elements. Catalyst is

specific in its action and only a small amount is required in a chemical reaction.

Industrial

process

Product produced Equation Catalyst

Haber Process

Contact Process

Ostwald Process

Hydrogenation of

vegetable oil

Cracking of

petroleum

(g) Other examples: Table shows the reacting conditions for the following experiments.

For the following experiments , sketch graph of(i) volume of gas against time

Experiment 1 5cm3 5 volume of H2O2 + 45cm3 water + MnO2

Experiment 2 3cm3 5 volume of H2O2 + 47cm3 water + MnO2

(ii) volume of gas against time

Experiment 1 5cm3 5 volume of H2O2 + 45cm3 water at 40oC

Experiment 2 5cm3 5 volume of H2O2 + 45cm3 water at room temperature

(iii) Volume of hydrogen against time


Volume of

oxygen/cm3

Time/s

Volume of

oxygen/cm3

Time/s


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Experiment 1 4 g of excess zinc powder + 100 cm3 of sulphuric acid 0.5 mol dm-3 +5cm3 copper(II) sulphate solution at room temperature

Experiment 2 4 g of excess zinc powder + 100 cm3 of sulphuric acid 0.5 mol dm-3

room temperature

Experiment 3 4 g of excess zinc powder + 50 cm3

of sulphuric acid 0.5 mol dm-3

atroom temperature

8. Collision Theory

(a) For a chemical reaction to occur, the particles of the reactants must collide with eachother. However, not all collisions result in a chemical reaction to form products.

(b) According to collision theory, only those collisions which(i) with .. orientation and

(ii) posses amount of energy called activation energy , Eawill result in chemical reaction.

(c) Collisions of particles of reactants that result in chemical reaction is known as

.

(d) Activation energy , Ea, is defined as the minimum amount of energy of collision thatis required for particles of reactant to react or to produce effective collision.

(i) Exothermic reaction (ii) Endothermic reaction

(e) Using Collision Theory to explain the factors affecting the rate of reaction.


Energy Energy

Volume of

hydrogen/cm3

Time/s


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1. The effect of increase in total surface area of reactant.

Using solid reactant that is smaller in size.

When size of solid reactant is smaller, the total surface area increases

The frequency of collision of particles of reactant increases The frequency of effective collision increases

The rate of reaction increases.

2. The effect of increase in concentration of reactant.

Increasing the concentration of reactant will increase the number ofparticles of reactant per unit volume.

The frequency of collision of particles of reactant increases.

The frequency of effective collision increases.


3. The effect of increase in temperature of reaction

o By increasing the temperature of the reactant

o Increased in temperature, increases the kinetic energy of the reactant

particles.

o The frequency of colliding particles possesses energy higher than the

activation energy increases.

o The frequency of effective collision increases

o The rate of reaction increases.

4. The effect of catalyst on the rate of reaction.

Addition of a positive catalyst to a chemical reaction provides an

alternative path of reaction that requires a lower activation energy.

The frequency of effective collision increases


Energy profile diagrams to show the effect of catalyst on rate of reaction.


Energy Energy


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9. The effect of pressure on rate of reaction.

(i) The effect of pressure only affects the rate of chemical reaction when the reactants arein the gaseous state.

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

(ii) Increased in pressure by increasing the concentration of gas or by reducing the

volume of the vessel,

o the number of particles per unit volume increases.

o The frequency of collision among the reactant particles increases

o The frequency of effective collision increases

o Hence the rate of reaction increases.

Reinforce exercise;

1. Which of the following can be used to determine the rate of the reaction?I Release of gas per unit time.

II Change of colour intensity per unit time.

III Formation of precipitate per unit time.IV Increase in the mass of reactant per unit time.

A. I and II

B. III and IVC. I, II and III

D. II, III and IV

2. An equation of a reaction is as follows

In the reaction represented by the equation above, it was found that the change of

colour from green to brown was faster when the reactant mixture was heated.This was due to the

I. decrease in the activation energy.

II. increase in the frequency of effective collision .III. increase in the kinetic energy of ferrum(II) ions and chlorine molecules.

IV. increase in the frequency of collision between ferrum(II) ions and chlorinemolecules.

A. I and II onlyB. II and III only

C. I, III and IV only

D. II, III and IV only


2Fe2+ + Cl2 2Fe3+ + 2Cl

Green Brown


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3. Table 4 shows the total volume of gas collected at regular intervals in a reaction.

Time / s 0 30 60 90 120 150 180 210

Volume of gas/ cm3 0 2.0 3.7 5.2 6.4 7.3 8.6 8.6 What is the average rate of reaction in the second minute ?

A. 0.040 cm3s-1

B. 0.045 cm3s-1

C. 0.053 cm3s-1

D. 0.062 cm3s-1

4. The equation below represents the decomposition of hydrogen peroxide solution.

Which of the following are produced when 1 mole of hydrogen peroxide is

decomposed completely ?

[1 mole of gas occupies 24 dm3 at room condition;Avogadros constant : 6 X 1023 mol-1]

I 2 moles of water

II 12 dm3 of oxygen gas

III 3 X 1023 of oxygen moleculesIV 1.2 X 1024 of water molecules

A I and III only

B I and IV only

C II and III onlyD II and IV only

5 An experiment is carried out to study the rate of reaction between marble andhydrochloric acid to produce carbon dioxide gas.

Experiment Substances

I Excess marble and 50.0 cm3 of 2 mol dm-3 hydrochloric acid

II Excess marble and 100.0cm3 of 1 mol dm-3 hydrochloric acid

A C

B D

HST/RATE OF REACTION/SMKPB

2H2O

2(aq)2H

2O

(l)+ O

2(g)

24

Volume of

CO2/cm3Volume of

CO2/cm3

Volume of

CO2/cm3

Time/s Time/s

I

I

IIII


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6 The reaction between hydrochloric acid and zinc produces hydrogen gas. The

reaction is complete in 50 seconds and the maximum volume of gas produced is 25

cm3.

What is the average rate of the reaction?

A. 0.5 cm3 s-1 C. 2.0 cm3 s-1

B. 1.0 cm3 s-1 D. 4.0 cm3 s-1

7 The diagram shows the energy profile of a reaction.

Ea is the activation energy for this reaction.

What will change the activation energy from Ea to Ea?

A. Temperature C. Concentration

B. Catalyst D. Total surface area

8 Which of the following explains the meaning of effective collision?

A. The collision where its energy is less than the activation energy.B. The collision that has a low energy

C. The collision which takes place before a reaction

D. The collision that causes a reaction

9 The diagram shows the set up of the apparatus for an experiment to determine the

rate of reaction between sodium thiosulphate and sulphuric acid.


Volume ofCO2/cm

3

Time/s Time/s

I

III

II

Energy

Reactant

Products

Reaction path

Ea

Ea


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Which of the following combination of conditions take the shortest time for themark X to diappear from sight?

Sulphuric acid Sodium thiosulphate

Volume/cm3 Concentration/

mol dm-3Volume/cm3 Concentration/

mol dm-3

Temperature

/oC

A 10 1.0 50 0.5 30

B 10 1.0 50 0.5 40

C 10 0.5 50 0.5 30

D 20 0.5 40 0.5 40

10 In an experiment, the decomposition of 25cm3 of 0.1 mol dm-3 hydrogen peroxide

solution produces oxygen gas.

If the experiment is repeated using another solution, which solution will produce

curve Q?

A. 25 cm3

of 0.15 mol dm-3

hydrogen peroxideB. 20 cm3 of 0.15 mol dm-3 hydrogen peroxideC. 15 cm3 of 0.15 mol dm-3 hydrogen peroxide

D. 10 cm3 of 0.25 mol dm-3 hydrogen peroxide

11 The following statements are related to the collision theory of a reaction.

I. The total surface area of the reactant particles increases.

II. The kinetic energy of the reactant particles increases.III. The frequency of the collision between the reactant particles increases.

IV. The number of the reactant particles per unit volume increases.

Which of the following combinations is true about the effect of the rise in

temperature on the reactant particles?A I and II only C III and IV only

B II and III only D I and IV only

12 If you want to cook 100 potatoes within a short time, which is the most suitablemethod?


Volume of

oxygengas/cm3

Time/s

P

Q


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A Boil the potatoes in a pan

B Boil the potatoes in a pressure cooker

C Steam the potatoes in a steamerD Fry the potatoes in a wok

13 Which of the following reactants produces the highest rate of reaction with zincpowder?

A 25 cm3 of sulphuric acid 0.1 mol dm-3.

B 25 cm3 of ethanoic acid 0.1 mol dm-3.C 25 cm3 of nitric acid 0.1 mol dm-3.

D 25 cm3 of hydrochloric acid 0.1 mol dm-3.

Reinforce Exercise for Structural Questions and Essay Questions.

1. The rate of reaction is affected by several factors. One of the factors is the size of

particles.

(a) Explain the above statement based on the size of the particles.

[2 marks]

(b) A student carried out three experiments to investigate the effects of the factors

influencing the rate of reaction. Table 1 shows the results of the experiments.


One kilogramme of meat, cut into big pieces, takes a longer time to

cook compared to one kilogram of meat cut into smaller pieces.


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(i) Write the chemical equation for the reaction between magnesium and hydrochloric

acid. Calculate the maximum volume of hydrogen gas produced.

[ Relative atomic mass: Mg,24; molar mass volume: 24 dm3 mol-1 at room condition][4 marks]

(ii) Sketch the graphs for the volume of hydrogen gas against time for Experiment I, II

and III on the same axes.[3 marks]

(iii) Calculate the average rate of reaction for Experiment I, II and III in cm3 s-1.

[3 marks]

(iv) Compare the rates of reaction between Experiment I and Experiment II, and betweenExperiment II and Experiment III.

With reference to collision theory, explain why there are differences in the rates of

reaction in the experiments.[8 marks]



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2. An experiment was conducted to find out the effects of temperature on the rate of

reaction. 50cm3 of sodium thiosulphate solution 0.05 mol dm-3 at 30oC was put into a

250cm3 conical flask. Then the conical flask was placed on an X sign on a piece ofwhite paper.

10cm3

of hydrochloric acid 1.0 mol dm-3

was added to the sodium thiosulphate solutionand shaken. At the same time, the stop watch was started. The stop watch was stopped as

soon as the X sign was no longer visible.

The same steps of the experiment were repeated for sodium thiosulphate solution whichwas heated to 35oC, 40oC, 45oC and 50oC.

Figure 1 shows the readings of the stop watch for each of the reaction at different

temperatures.

(a)

Record the time for each reaction in the spaces provided in Figure 1.

(b) Construct a table and record temperature, time and 1/time for this experiment.



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(c) (i) Draw a graph of temperature against 1/time on the graph paper.

(ii) Based on the graph in c(i) , state the relationship between the rate of reaction andtemperature.

(d) Predict the time taken as soon as the sign X to be not longer visible if thisexperiment is repeated at 55oC.

(e)(i) State the variables involved in this experiment.

Manipulated variable:

Responding variable:

Constant variable:

(ii) State how you would manipulate one variable while keeping the other variables

constant.

(f) State the hypothesis for this experiment.

(g) From the above experiment, the student found a relationship between temperature and

rate of reaction. The same situation can be applied in our daily lives, for example,

keeping food that is easily spoiled in the refrigerator.



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Using your knowledge of chemistry, state the relationship between temperature and the

rate at which food turns bad.

3(a) Food stored in a refrigerator last longer than food stored in a kitchen cabinet.

Explain why.[4 marks]

(b) A group of pupils carried out three experiments to investigate the factors affecting the

rate of a reaction.Table 7 shows information about the reactants and the temperature used in each

experiment.

Experiment Reactants Temperature /oC

I Excess calcium carbonate chips and 30 cm3 of 0.5

mod dm-3 hydrochloric acid

30

II Excess calcium carbonate chips and 30 cm3 of 0.5

mod dm-3 hydrochloric acid

40

III Excess calcium carbonate powder and 30 cm3 of

0.5 mod dm-3 hydrochloric acid

40

Table 7.

Graph 7 shows the results of these experiments.



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(i) Calculate the average rate of reaction for experiment I.

[2 marks]

(ii) Based on Table 7 and graph 7, compare the rate of reaction between:

Experiment I and Experiment II

Experiment II and Experiment III

In each case explain the difference in rate of reaction with reference to the

collision theory.

[ 10 marks]

(iii) The chemical equation below shows the reaction between calcium carbonate and

hydrochloric acid.

CaCO3 + 2HCl CaCl2 + CO2 + H2O

Given that the relative atomic mass of C=12, O=16, Ca=40 and the molar volume

of any gas is 24 cm3

mol-1

at room temperature and pressure.

Calculate the maximum volume of carbon dioxide gas produced in Experiment II.

[4 marks]



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4. Diagram 6 shows two experiments to investigate one factor that influences the rate of a

reaction.

(a) What is the factor that influences the rate of reaction in both experiments?

[1 mark]

(b) The reaction in the experiment is represented by the following equation:

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

(i) Among the products stated in the equation, which is the most suitable to be

chosen to determine the rate of reaction?

[1 mark]



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15891064-rate-of-reaction

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