R2.2 How fast? The rate of chemical change - IB Chemistry Question Bank

Question 1

SL • Paper 1A

Easy

Calculator Permitted

A clock reaction is repeated using different reactant concentrations. In each trial, the time is measured for the same fixed amount of product to form. What quantity is most directly proportional to the initial rate?

A.

$t$

B.

$t^2$

C.

$\ln t$

D.

$1/t$

Question 2

SL • Paper 1A

Easy

Calculator Permitted

The temperature of a reacting gas mixture is increased from $300\ \text{K}$ to $330\ \text{K}$ . What is the main reason for the increase in reaction rate according to collision theory?

A.

A larger fraction of particles has energy at least equal to $E_a$ .

B.

The activation energy of the uncatalysed reaction decreases.

C.

The enthalpy change of the reaction becomes more negative.

D.

All collisions occur with the correct collision geometry.

Question 3

SL • Paper 1A

Easy

Calculator Permitted

For the reaction $2\text{NO(g)} + \text{O}_2\text{(g)} \to 2\text{NO}_2\text{(g)}$ , the concentration of $\text{NO}$ decreases from $0.240\ \text{mol dm}^{-3}$ to $0.160\ \text{mol dm}^{-3}$ in $50.0\ \text{s}$ . What is the average rate of reaction over this time interval?

A.

$8.00\times 10^{-4}\ \text{mol dm}^{-3}\ \text{s}^{-1}$

B.

$4.00\times 10^{-4}\ \text{mol dm}^{-3}\ \text{s}^{-1}$

C.

$3.20\times 10^{-3}\ \text{mol dm}^{-3}\ \text{s}^{-1}$

D.

$1.60\times 10^{-3}\ \text{mol dm}^{-3}\ \text{s}^{-1}$

Question 4

SL • Paper 1A

Easy

Calculator Permitted

Hydrogen gas is produced when magnesium reacts with excess dilute hydrochloric acid. The gas is to be collected and its volume measured continuously. What apparatus is most suitable?

A.

Gas syringe connected to the reaction flask

B.

Thermometer placed above the reaction flask

C.

pH probe placed in the reaction mixture

D.

Colorimeter and cuvette containing the reaction mixture

Question 5

SL • Paper 1A

Easy

Calculator Permitted

In repeated trials measuring the volume of gas produced in a reaction, all final gas volumes are lower than the expected stoichiometric volume by a similar amount. What is the most likely type of error?

A.

Random error from variation in reaction temperature

B.

Systematic error from gas leaking from the apparatus

C.

Random error from using a smaller measuring cylinder

D.

Systematic error from repeating the experiment several times

Question 6

HL • Paper 1A

Easy

Calculator Permitted

The elementary step $\text{NO}_2\text{(g)} + \text{CO(g)} \to \text{NO(g)} + \text{CO}_2\text{(g)}$ occurs in a proposed mechanism. What is the molecularity of this elementary step?

A.

Unimolecular

B.

Zeromolecular

C.

Termolecular

D.

Bimolecular

Question 7

SL • Paper 2

Easy

Calculator Permitted

A student investigates the rate of reaction between zinc granules and hydrochloric acid by measuring the hydrogen gas produced.

A simple laboratory apparatus diagram showing a conical flask containing zinc and hydrochloric acid connected by a delivery tube to a graduated gas syringe clamped horizontally; labels should identify the flask, bung, delivery tube and gas syringe without showing any numerical readings.

A

State one suitable piece of apparatus for measuring the volume of hydrogen continuously.

[1]

Write your answer here...

B

State two variables, other than acid concentration, that should be controlled when investigating the effect of acid concentration on the rate.

[2]

Write your answer here...

0

Question 8

SL • Paper 1A

Medium

Calculator Permitted

An exothermic reaction is carried out with and without a catalyst. The catalyst changes only the activation energy. The correct energy profile is shown by which diagram?

A.

B.

C.

D. Question 9

HL • Paper 1A

Medium

Calculator Permitted

Initial-rate data for a reaction are shown.

Experiment	$[A]/\text{mol dm}^{-3}$	$[B]/\text{mol dm}^{-3}$	Initial rate/ $\text{mol dm}^{-3}\ \text{s}^{-1}$
1	$0.100$	$0.100$	$2.00\times 10^{-4}$
2	$0.200$	$0.100$	$8.00\times 10^{-4}$
3	$0.100$	$0.300$	$6.00\times 10^{-4}$

What is the rate equation?

A.

$r=k[A]^2[B]^2$

B.

$r=k[A]^2[B]$

C.

$r=k[A][B]^2$

D.

$r=k[A][B]$

Question 10

HL • Paper 1A

Medium

Calculator Permitted

A proposed mechanism is shown.

Step 1: $A + B \to I$ slow

Step 2: $I + C \to D$ fast

What are the intermediate and the rate equation predicted by the rate-determining step?

A.

Intermediate $D$ ; $r=k[D]$

B.

Intermediate $I$ ; $r=k[A][B]$

C.

Intermediate $C$ ; $r=k[I][C]$

D.

Intermediate $B$ ; $r=k[A][B][C]$

Question 11

HL • Paper 1A

Medium

Calculator Permitted

For a reaction with rate equation $r=k[A][B]^2$ , rate is measured in $\text{mol dm}^{-3}\ \text{s}^{-1}$ and concentration in $\text{mol dm}^{-3}$ . What are the units of $k$ ?

A.

$\text{s}^{-1}$

B.

$\text{dm}^3\ \text{mol}^{-1}\ \text{s}^{-1}$

C.

$\text{mol dm}^{-3}\ \text{s}^{-1}$

D.

$\text{dm}^6\ \text{mol}^{-2}\ \text{s}^{-1}$

Question 12

HL • Paper 1A

Medium

Calculator Permitted

For an Arrhenius plot of $\ln k$ against $1/T$ , what are the gradient and vertical intercept?

A.

Gradient $E_a/R$ ; intercept $A$

B.

Gradient $\ln A$ ; intercept $-E_a/R$

C.

Gradient $-E_a/R$ ; intercept $\ln A$

D.

Gradient $-R/E_a$ ; intercept $\ln A$

Question 13

SL • Paper 2

Medium

Calculator Permitted

The concentration of bromine was monitored during its reaction with methanoic acid at constant temperature.

Time / s	$[\text{Br}_2]$ / $\text{mol dm}^{-3}$
0	$0.0100$
20	$0.00640$
40	$0.00440$

A

Determine the average rate of disappearance of bromine between $20$ s and $40$ s.

[2]

Write your answer here...

B

State how the instantaneous rate at $20$ s would be obtained from a concentration-time graph.

[1]

Write your answer here...

0

Question 14

SL • Paper 2

Medium

Calculator Permitted

The rate of reaction between iodide ions and peroxodisulfate ions increases when the temperature is raised from $298\ \text{K}$ to $318\ \text{K}$ .

A

Define activation energy.

[1]

Write your answer here...

B

Explain why increasing the temperature increases the rate of reaction, using collision theory.

[2]

Write your answer here...

0

Question 15

SL • Paper 2

Medium

Calculator Permitted

Magnesium reacts with excess dilute hydrochloric acid. In one experiment a single strip of magnesium is used. In a second experiment the same mass of magnesium is cut into many small pieces.

A

Predict the effect on the initial rate in the second experiment.

[1]

Write your answer here...

B

Explain your prediction in terms of collisions.

[2]

Write your answer here...

C

State why changing the pressure would have little direct effect on this reaction mixture.

[1]

Write your answer here...

0

Question 16

HL • Paper 2

Medium

Calculator Permitted

The energy profile for a multistep reaction is shown.

A

State the number of elementary steps and the number of intermediates shown.

[2]

Write your answer here...

B

Identify the rate-determining step and justify your answer.

[2]

Write your answer here...

0

Question 17

SL • Paper 1B

Medium

Calculator Permitted

Magnesium ribbon was reacted with excess dilute hydrochloric acid. The volume of hydrogen gas was collected in a gas syringe and recorded over time.

Hydrogen gas volume collected over time.

A

Determine the total volume of hydrogen gas produced.

[1]

Write your answer here...

B

Calculate the average rate of production of hydrogen gas between $20\ \text{s}$ and $60\ \text{s}$ .

[2]

Write your answer here...

C

Explain why the rate decreases during the reaction.

[2]

Write your answer here...

0

Question 18

SL • Paper 1B

Medium

Calculator Permitted

A clock reaction was carried out between sodium thiosulfate solution and hydrochloric acid. The time taken for a fixed amount of sulfur precipitate to obscure a mark was recorded at different sodium thiosulfate concentrations. Temperature and total volume were kept constant.

Na2S2O3 concentration / mol dm^-3	Time / s
0.0250	160
0.0500	80
0.100	40

A

State why $1/t$ can be used as a measure of rate in this experiment.

[1]

Write your answer here...

B

Use the data to compare the rate when the sodium thiosulfate concentration is doubled from $0.0500\ \text{mol dm}^{-3}$ to $0.100\ \text{mol dm}^{-3}$ .

[2]

Write your answer here...

C

Explain the effect of increasing the sodium thiosulfate concentration using collision theory.

[2]

Write your answer here...

0

Question 19

SL • Paper 1B

Medium

Calculator Permitted

Equal masses of calcium carbonate were reacted separately with excess hydrochloric acid. In experiment 1, large chips were used. In experiment 2, powdered calcium carbonate was used. The volume of carbon dioxide was recorded over time.

Volume of carbon dioxide produced over time for calcium carbonate chips and powder.

A

Compare the initial rates and final volumes of carbon dioxide for the two experiments.

[2]

Write your answer here...

B

Explain the difference in rate between the two experiments.

[2]

Write your answer here...

0

Question 20

HL • Paper 1A

Medium

Calculator Permitted

A two-step reaction is exothermic. The second step is rate-determining and there is one intermediate. The correct energy profile is shown by which diagram?

A.

B.

C.

D. Question 21

SL • Paper 2

Medium

Calculator Permitted

A Maxwell-Boltzmann distribution can be used to show the effect of temperature on the proportion of particles able to react.

A

Sketch Maxwell-Boltzmann energy distribution curves for the same sample at two temperatures, $T_1$ and $T_2$ , where $T_2 > T_1$ . Label the activation energy, $E_a$ , and show the relative number of particles with energy greater than $E_a$ at each temperature.

[3]

Write your answer here...

0

Question 22

SL • Paper 2

Medium

Calculator Permitted

Hydrogen peroxide decomposes exothermically. Manganese(IV) oxide acts as a catalyst for the decomposition.

A

Sketch an energy profile for the reaction with and without the catalyst.

[3]

Write your answer here...

B

State the effect of the catalyst on the enthalpy change of the reaction.

[1]

Write your answer here...

0

Question 23

HL • Paper 2

Medium

Calculator Permitted

The following mechanism is proposed for the reaction $2\text{NO}(g) + \text{Cl}_2(g) \to 2\text{NOCl}(g)$ .

Step 1: $\text{NO}(g) + \text{Cl}_2(g) \to \text{NOCl}_2(g)$ slow

Step 2: $\text{NOCl}_2(g) + \text{NO}(g) \to 2\text{NOCl}(g)$ fast

A

Identify the intermediate in the mechanism.

[1]

Write your answer here...

B

State the molecularity of the slow step.

[1]

Write your answer here...

C

The experimentally determined rate equation is $r = k[\text{NO}][\text{Cl}_2]$ . Evaluate whether the mechanism is consistent with the kinetic and stoichiometric data.

[2]

Write your answer here...

0

Question 24

HL • Paper 2

Medium

Calculator Permitted

Initial-rate data were obtained for the reaction $\text{A} + \text{B} \to \text{products}$ at constant temperature.

Experiment	$[\text{A}]$ / $\text{mol dm}^{-3}$	$[\text{B}]$ / $\text{mol dm}^{-3}$	Initial rate / $\text{mol dm}^{-3}\ \text{s}^{-1}$
1	$0.100$	$0.100$	$2.00 \times 10^{-5}$
2	$0.200$	$0.100$	$8.00 \times 10^{-5}$
3	$0.100$	$0.200$	$2.00 \times 10^{-5}$

A

Deduce the order of reaction with respect to A and with respect to B.

[2]

Write your answer here...

B

Write the rate equation and state the overall order.

[2]

Write your answer here...

0

Question 25

HL • Paper 2

Medium

Calculator Permitted

For a reaction at $298\ \text{K}$ , the rate equation is $r = k[\text{P}][\text{Q}]^2$ . When $[\text{P}] = 0.120\ \text{mol dm}^{-3}$ and $[\text{Q}] = 0.200\ \text{mol dm}^{-3}$ , the initial rate is $5.76 \times 10^{-5}\ \text{mol dm}^{-3}\ \text{s}^{-1}$ .

A

Calculate the value of the rate constant, $k$ , including its units.

[3]

Write your answer here...

0

Question 26

HL • Paper 2

Medium

Calculator Permitted

The decomposition of X was followed at constant temperature. Three plots were tested using the same concentration-time data. Only the plot of $\ln[\text{X}]$ against time was linear, with gradient $-1.80 \times 10^{-2}\ \text{s}^{-1}$ .

Time / s	[X] / mol dm^-3
0	0.100
20	0.0698
40	0.0487
60	0.0340
80	0.0237
100	0.0165
120	0.0115

A

Determine the order of reaction with respect to X.

[1]

Write your answer here...

B

Determine the value and units of the rate constant, $k$ .

[2]

Write your answer here...

0

Question 27

SL • Paper 1B

Medium

Calculator Permitted

The diagram shows Maxwell-Boltzmann energy distributions for the same reacting gas mixture at two different temperatures. The activation energy, $E_a$ , for the reaction is also shown.

Maxwell-Boltzmann distributions for the same gas at two temperatures and an activation energy line.

A

State what the area under each distribution curve represents.

[1]

Write your answer here...

B

Describe two differences between the distribution at higher temperature and the distribution at lower temperature.

[2]

Write your answer here...

C

Explain why the rate is greater at the higher temperature.

[2]

Write your answer here...

0

Question 28

SL • Paper 1B

Medium

Calculator Permitted

An energy profile is shown for an exothermic reaction, with and without a catalyst.

A

Identify which pathway has the lower activation energy.

[1]

Write your answer here...

B

State the effect of the catalyst on the overall enthalpy change of the reaction.

[1]

Write your answer here...

C

Explain how the catalyst increases the rate of reaction.

[2]

Write your answer here...

0

Question 29

HL • Paper 1B

Medium

Calculator Permitted

A proposed mechanism for a reaction is shown. The experimentally determined rate equation is also given.

Item	Details
Step 1 (slow)	$\text{NO}_2 + \text{Cl}_2 \to \text{NO}_2\text{Cl} + \text{Cl}$
Step 2 (fast)	$\text{Cl} + \text{NO}_2 \to \text{NO}_2\text{Cl}$
Experimental rate law	r = k[NO2][Cl2]

A

Identify the intermediate in the mechanism.

[1]

Write your answer here...

B

Deduce the overall equation by adding the elementary steps.

[1]

Write your answer here...

C

Evaluate whether the mechanism is consistent with the experimental rate equation.

[2]

Write your answer here...

0

Question 30

HL • Paper 1B

Medium

Calculator Permitted

The concentration of reactant A was monitored during a reaction at constant temperature. Three possible linearized plots were produced from the same concentration-time data.

Time / s	[A] / mol dm^-3	ln([A])	1/[A] / dm^3 mol^-1
0	1.000	0.000	1.000
25	0.3679	-1.000	2.719
50	0.1353	-2.000	7.390
75	0.04979	-3.000	20.09
100	0.01832	-4.000	54.60
125	0.006738	-5.000	148.4

A

Identify the order of reaction with respect to A.

[1]

Write your answer here...

B

Determine the rate constant, including its units.

[2]

Write your answer here...

C

State how the value of $k$ would be affected by increasing the temperature, assuming no other change is made.

[1]

Write your answer here...

0

Question 31

HL • Paper 2

Medium

Calculator Permitted

For a first-order decomposition, an Arrhenius plot of $\ln k$ against $1/T$ is linear. The gradient of the best-fit line is $-9.20 \times 10^3\ \text{K}$ and the intercept is $27.5$ . Use $R = 8.31\ \text{J mol}^{-1}\ \text{K}^{-1}$ .

Arrhenius plot of ln k against 1/T with a straight-line trend.

A

Calculate the activation energy, $E_a$ , in $\text{kJ mol}^{-1}$ .

[2]

Write your answer here...

B

Determine the Arrhenius factor, $A$ , including units.

[2]

Write your answer here...

0

Question 32

SL • Paper 1B

Hard

Calculator Permitted

A student investigated the effect of hydrochloric acid concentration on the initial rate of reaction with magnesium ribbon. The initial rate was determined from the gradient of a tangent to the volume-time curve for each trial. Several repeats were carried out at each acid concentration.

Scatter graph of initial rate against hydrochloric acid concentration with repeated measurements and a fitted trend line.

A

Use the graph to determine whether the initial rate is directly proportional to the hydrochloric acid concentration over the range investigated.

[2]

Write your answer here...

B

Comment on the reliability of the data, referring to random error and the anomalous point.

[2]

Write your answer here...

C

State one variable, other than acid concentration, that should be controlled in this investigation.

[1]

Write your answer here...

0

Question 33

HL • Paper 1B

Hard

Calculator Permitted

Initial-rate data were obtained for the reaction between reactants A and B at constant temperature.

Experiment	[A] / mol dm^-3	[B] / mol dm^-3	Initial rate / mol dm^-3 s^-1
1	0.100	0.100	2.00 × 10^-4
2	0.200	0.100	4.00 × 10^-4
3	0.100	0.200	8.00 × 10^-4
4	0.200	0.200	1.60 × 10^-3

A

Deduce the order of reaction with respect to A and with respect to B.

[2]

Write your answer here...

B

Write the rate equation for the reaction.

[1]

Write your answer here...

C

Calculate the rate constant, including its units, using the first experiment.

[2]

Write your answer here...

0

Question 34

HL • Paper 1B

Hard

Calculator Permitted

An energy profile is shown for a reaction that occurs in three elementary steps.

A

State the number of transition states and intermediates shown.

[2]

Write your answer here...

B

Identify the rate-determining step and justify your answer.

[1]

Write your answer here...

C

Calculate the overall enthalpy change for the reaction.

[1]

Write your answer here...

D

Suggest why changing the concentration of a reactant involved only in step 1 may have little effect on the overall rate under these conditions.

[1]

Write your answer here...

0

Question 35

SL • Paper 2

Hard

Calculator Permitted

A student investigates the reaction between marble chips, $CaCO_3(s)$ , and excess hydrochloric acid.

$CaCO_3(s) + 2HCl(aq) \to CaCl_2(aq) + H_2O(l) + CO_2(g)$

The volume of carbon dioxide is recorded using a gas syringe.

Carbon dioxide volume recorded during the reaction.

A

The tangent at $30\ \text{s}$ passes through $(10\ \text{s}, 14.0\ \text{cm}^3)$ and $(50\ \text{s}, 42.0\ \text{cm}^3)$ .

I.

Calculate the instantaneous rate of formation of carbon dioxide at $30\ \text{s}$ in $\text{cm}^3\ \text{s}^{-1}$ .

[2]

Write your answer here...

II.

State why the rate calculated from a tangent is an instantaneous rate rather than an average rate.

[1]

Write your answer here...

B

The experiment is repeated using the same mass of powdered calcium carbonate instead of marble chips. Explain the expected change in the initial rate and the final volume of carbon dioxide.

[2]

Write your answer here...

C

Suggest one improvement to the apparatus if the graph showed a lower final gas volume than expected. Explain how this improvement would affect the data.

[2]

Write your answer here...

0

Question 36

SL • Paper 2

Hard

Calculator Permitted

The reaction between iodide ions and peroxodisulfate ions is followed using a clock method. A fixed amount of thiosulfate ion and starch indicator is added. The time taken for a blue-black colour to appear is measured for different initial concentrations.

$S_2O_8^{2-}(aq) + 2I^-(aq) \to 2SO_4^{2-}(aq) + I_2(aq)$

Clock reaction results showing how the time to the blue-black endpoint changes with initial iodide concentration.

A

The clock endpoint corresponds to the formation of the same small amount of iodine in every trial.

I.

Explain why $\frac{1}{t}$ can be used as a measure proportional to the initial rate in this experiment.

[2]

Write your answer here...

II.

Explain, using collision theory, why increasing the concentration of iodide ions is expected to decrease the time to the endpoint.

[2]

Write your answer here...

B

Evaluate two variables, other than the concentration being investigated, that must be controlled to make the comparison of rates valid.

[2]

Write your answer here...

0

Question 37

SL • Paper 2

Hard

Calculator Permitted

A student investigates the reaction between sodium thiosulfate solution and hydrochloric acid by timing how long it takes for a cross under the flask to disappear.

$S_2O_3^{2-}(aq) + 2H^+(aq) \to SO_2(aq) + S(s) + H_2O(l)$

Scatter plot of relative rate against sodium thiosulfate concentration with a straight-line best fit showing slight scatter and a non-zero intercept.

A

The time for the cross to disappear in one trial is $48.0\ \text{s}$ .

I.

Calculate the relative rate, using $\frac{1}{t}$ , in $\text{s}^{-1}$ .

[1]

Write your answer here...

II.

Explain why the disappearance of the cross is a fixed endpoint for comparing rates.

[1]

Write your answer here...

B

Design a fair comparison to investigate the effect of thiosulfate concentration on the rate.

[3]

Write your answer here...

C

Use the graph to distinguish between random error and systematic error in this investigation.

[2]

Write your answer here...

0

Question 38

HL • Paper 1B

Hard

Calculator Permitted

Rate constants were measured for a first-order reaction at several temperatures. The data were used to construct an Arrhenius plot of $\ln k$ against $1/T$ .

Measured points and best-fit line for an Arrhenius plot.

A

Determine the activation energy, $E_a$ , from the gradient of the Arrhenius plot.

[2]

Write your answer here...

B

Determine the Arrhenius factor, $A$ , including units.

[2]

Write your answer here...

C

Explain why temperature must be expressed in kelvin in the Arrhenius equation.

[1]

Write your answer here...

0

Question 39

HL • Paper 1B

Hard

Calculator Permitted

Two mechanisms have been proposed for the reaction $2\text{NO}+\text{Br}_2\to 2\text{NOBr}$ . The experimentally determined rate equation is $r=k[\text{NO}]^2[\text{Br}_2]$ .

Mechanism	Step 1	Step 2
A	NO + Br2 -> NOBr2 slow	NOBr2 + NO -> 2NOBr fast
B	NO + Br2 ⇌ NOBr2 fast	NOBr2 + NO -> 2NOBr slow

A

State the molecularity of the slow step in mechanism B.

[1]

Write your answer here...

B

Show that mechanism B gives the correct overall equation.

[1]

Write your answer here...

C

Evaluate which mechanism is more consistent with the experimental rate equation.

[2]

Write your answer here...

D

State why a mechanism that matches the rate equation is still described as a possible mechanism.

[1]

Write your answer here...

0

Question 40

SL • Paper 2

Hard

Calculator Permitted

The rate of a gas-phase reaction increases when the temperature is raised from $T_1$ to $T_2$ , where $T_2>T_1$ .

A blank Maxwell-Boltzmann distribution set of axes. The vertical axis is labelled frequency of particles and the horizontal axis is labelled kinetic energy. A vertical line labelled $E_a$ is shown to the right of the most probable energy, leaving space for students to sketch two curves at different temperatures.

A

Use the axes provided.

I.

Sketch Maxwell-Boltzmann energy distribution curves for $T_1$ and $T_2$ .

[2]

Write your answer here...

II.

Explain why the increase in temperature causes a large increase in rate.

[2]

Write your answer here...

B

catalyst is added at constant temperature. Explain how the Maxwell-Boltzmann diagram can be used to show the effect of the catalyst on the rate.

[3]

Write your answer here...

0

Question 41

SL • Paper 2

Hard

Calculator Permitted

An uncatalysed exothermic reaction is represented by an energy profile. The same reaction can also occur by a catalysed pathway.

A

Refer to the energy profile shown.

I.

Identify the activation energy and the transition state on the diagram.

[2]

Write your answer here...

II.

State how the diagram shows that the reaction is exothermic.

[1]

Write your answer here...

B

Sketch the catalysed pathway on the same diagram and explain the effect of the catalyst on the rate.

[3]

Write your answer here...

C

Discuss the statement: "A catalyst increases the yield of product because it makes the products more stable."

[2]

Write your answer here...

0

Question 42

SL • Paper 2

Hard

Calculator Permitted

Hydrogen peroxide decomposes slowly at room temperature but much faster in the presence of catalase, an enzyme found in potato tissue.

$2H_2O_2(aq) \to 2H_2O(l) + O_2(g)$

A simple apparatus diagram showing a conical flask containing hydrogen peroxide solution and pieces of potato, connected through a bung and delivery tube to a gas syringe for collecting oxygen gas.

A

The volume of oxygen collected is used to determine the reaction rate.

I.

Explain why using a gas syringe is suitable for following the rate continuously.

[2]

Write your answer here...

II.

At one instant oxygen is forming at $1.20\times10^{-4}\ \text{mol dm}^{-3}\ \text{s}^{-1}$ . Determine the rate of disappearance of hydrogen peroxide at this instant.

[2]

Write your answer here...

B

Explain the roles of sufficient energy and proper orientation in the decomposition of hydrogen peroxide.

[2]

Write your answer here...

C

Compare the effect of catalase with the effect of finely divided manganese(IV) oxide, $MnO_2$ , on this reaction.

[2]

Write your answer here...

0

Question 43

HL • Paper 2

Hard

Calculator Permitted

The initial rate of a reaction involving aqueous reactants $A$ , $B$ and $C$ is measured at constant temperature. The balanced equation is not sufficient to determine the rate equation.

Experiment	[A] / mol dm^-3	[B] / mol dm^-3	[C] / mol dm^-3	Initial rate / mol dm^-3 s^-1
1	0.100	0.100	0.100	2.00×10^-4
2	0.200	0.100	0.100	8.00×10^-4
3	0.100	0.200	0.100	4.00×10^-4
4	0.100	0.100	0.300	2.00×10^-4

A

Use the initial-rate data.

I.

Deduce the order of reaction with respect to $A$ , $B$ and $C$ .

[3]

Write your answer here...

II.

Write the rate equation and state the overall order.

[2]

Write your answer here...

B

In one experiment, $[A]=0.100\ \text{mol dm}^{-3}$ , $[B]=0.100\ \text{mol dm}^{-3}$ and the initial rate is $2.00\times10^{-4}\ \text{mol dm}^{-3}\ \text{s}^{-1}$ . Calculate $k$ and give its units.

[2]

Write your answer here...

C

Explain why the orders in the rate equation cannot be deduced from the coefficients in the overall balanced equation.

[1]

Write your answer here...

0

Question 44

HL • Paper 2

Hard

Calculator Permitted

A possible mechanism for a reaction is shown.

$\begin{aligned} \text{Step 1: }& A \to I &&\text{fast}\\ \text{Step 2: }& I+B \to P &&\text{slow}\\ \text{Step 3: }& P+B \to C+D &&\text{fast} \end{aligned}$

A

Consider the proposed sequence of elementary steps.

I.

Show that the steps give the overall equation and identify the intermediates.

[3]

Write your answer here...

II.

State the molecularity of step 2 and explain why termolecular elementary steps are uncommon.

[2]

Write your answer here...

B

Use the energy profile.

I.

Identify the rate-determining step and the transition state for this step.

[2]

Write your answer here...

II.

Explain why the expression $r=k[I][B]$ is not normally written as the experimental rate equation for the overall reaction.

[1]

Write your answer here...

0

Question 45

HL • Paper 2

Hard

Calculator Permitted

The decomposition of a compound $X$ is monitored at constant temperature. The data are processed using three possible linear plots.

Linearised data for X during decomposition at constant temperature.

A

The gradient of the straight-line plot is $-4.62\times10^{-2}\ \text{s}^{-1}$ .

I.

Deduce the order of reaction with respect to $X$ .

[1]

Write your answer here...

II.

Determine the rate constant, including units.

[2]

Write your answer here...

III.

Calculate the half-life of $X$ .

[2]

Write your answer here...

B

Calculate the instantaneous rate when $[X]=0.0800\ \text{mol dm}^{-3}$ .

[1]

Write your answer here...

C

Explain why identifying a first-order graph does not prove a unique reaction mechanism.

[1]

Write your answer here...

0

Question 46

HL • Paper 2

Hard

Calculator Permitted

The hydrolysis of a tertiary halogenoalkane, $RBr$ , in aqueous alkali is investigated.

$RBr(aq)+OH^-(aq) \to ROH(aq)+Br^-(aq)$

Initial-rate data show that doubling $[RBr]$ doubles the rate, but doubling $[OH^-]$ has no effect on the rate.

A

Use the kinetic information.

I.

Deduce the rate equation.

[2]

Write your answer here...

II.

State the units of $k$ .

[1]

Write your answer here...

B

Two possible mechanisms are proposed.

Mechanism 1:

$\begin{aligned} \text{Step 1: }&RBr \to R^+ + Br^- &&\text{slow}\\ \text{Step 2: }&R^+ + OH^- \to ROH &&\text{fast} \end{aligned}$

Mechanism 2:

$RBr+OH^- \to ROH+Br^- \quad \text{slow}$

[3]

Write your answer here...

C

Evaluate whether the kinetic data prove mechanism 1.

[2]

Write your answer here...

0

Question 47

HL • Paper 2

Hard

Calculator Permitted

The rate constant for a first-order reaction is measured at different temperatures. An Arrhenius plot of $\ln k$ against $1/T$ is obtained.

A

The gradient of the line is $-7.20\times10^3\ \text{K}$ and the intercept is $18.4$ .

I.

Calculate the activation energy, $E_a$ , in $\text{kJ mol}^{-1}$ .

[2]

Write your answer here...

II.

Determine the Arrhenius factor, $A$ , including units.

[2]

Write your answer here...

B

Calculate $k$ at $310\ \text{K}$ using the line equation.

[2]

Write your answer here...

C

Explain the physical significance of the temperature scale and the Arrhenius factor in this analysis.

[2]

Write your answer here...

0

Question 48

HL • Paper 2

Hard

Calculator Permitted

A clock reaction is studied at two temperatures using identical initial concentrations and the same fixed visible endpoint. The reciprocal of the time to the endpoint is used as a value proportional to $k$ .

At $298\ \text{K}$ , $k=1.25\times10^{-2}\ \text{s}^{-1}$ . At $318\ \text{K}$ , $k=1.00\times10^{-1}\ \text{s}^{-1}$ .

A

Analyse the temperature-dependence data.

I.

Explain why $\frac{1}{t}$ can be used as a value proportional to $k$ only under the stated experimental conditions.

[2]

Write your answer here...

II.

Calculate the activation energy using the two values of $k$ .

[3]

Write your answer here...

B

Use the value $E_a=81.9\ \text{kJ mol}^{-1}$ to estimate the Arrhenius factor, $A$ , from the data at $298\ \text{K}$ .

[2]

Write your answer here...

C

Evaluate one major experimental limitation when using a clock reaction to determine Arrhenius parameters.

[1]

Write your answer here...

0