Free Printable Reaction Kinetics

1.

If a reaction is described as zero order with respect to reactant A, this means that

a)

A is a catalyst in the reaction

b)

A is not involved in the rate determining step

c)

the value of the rate constant is independent of A

d)

the rate of reaction in inversely propotional to the concentration of A

2.

The initial concentration of an active substance in an aqueous solution is 5.0 x $10^{-3}$ mol $dm^{-3}$ . After 20 monts,an analysis shows that its concentration becomes 4.2x $10^{-3}$ mol $dm^{-3}$ . Determine the decay duration of this medicine by assuming the decomposition of the active substance is a first order reaction.

[Decay duration of this medicine is the time required as it decomposes 10% of the initial concentration]

a)

9 months

b)

12 months

c)

18 months

d)

23 months

3.

The reaction A + 2B --> products was foundto have the rate law , rate =k[A] $\left[B\right]^2$ .Predict by what factor the rate of reaction will increase when the concentration of B is doubled and the concentration of a remained unchanged .

a)

2

b)

4

c)

6

d)

8

4.

Half-life of a reaction increases with initial concentration if the reaction is

a)

zero order

b)

first order

c)

second order

d)

none of above

5.

The half-life of a radioactive elements is 50 minutes. How long will it take for the element to decay by 87.5%?

a)

1.67 hours

b)

2.00 hours

c)

2.25 hours

d)

2.50 hours

6.

The rate equation for a reaction is

Rate = k $\left[A\right]^2$ $\left[B\right]^0$

Choose the correct statement(s):

a)

The reaction is a second order

b)

The unit of the rate constant , k is $mol^{-1}$ $dm^3$ $S^{-1}$

c)

If the concentration of A is doubled, the rate of the reaction will increase four fold

7.

Consider the first order reaction:

X-->Y

Which of the following is/are true?

a)

The rate of reaction is directly propotional to X

b)

A plot of ln[X] against time give a straight line

c)

The rate constant changes propotionally according to the concentration of X

8.

In the haber process for the manufacture of ammonia from nitrogen and hidrogen,the rate of formation of ammonia is 2.50 mol $dm^{-3}$ $\min^{-1}$ . what is the rate of disappearance of hydrogen?

a)

2.50 mol $dm^{-3}$ $\min^{-1}$

b)

3.75 mol $dm^{-3}$ $\min^{-1}$

c)

4.50 mol $dm^{-3}$ $\min^{-1}$

d)

5.00 mol $dm^{-3}$ $\min^{-1}$

9.

The rate equation for a reaction involving an organic compound W and hydrochloric acid is

rate=k[W] $\left[H^+\right]$

which of the following statements regarding the reaction is not correct

a)

The overall order of the reaction is second order

b)

The unit of the rate constant, k is $mol^{-1}$ $dm^3$ $s^{-1}$

c)

Replacing hydrochloric acid with ethanoic acid has no effect on the reaction rate

d)

The rate of reaction doubles when sulphuric acid of the same concentration is used

10.

The half-life for the decomposition of an organic compound W is 80 min. if the decomposition is the first order reaction, what is the percentage of W that remains after 6 hours ?

a)

4.42%

b)

7.25%

c)

8.86%

d)

10.33%

11.

The reaction between compound X and Y is an acid-catalysed reaction.What is the ratio of the reaction rates at pH1 and pH 3 if the reaction is the first order with respect to $H^+$ ions

a)

2

b)

3

c)

20

d)

100

12.

The time taken for the concentration of the compound X to decrease from 1.00 mol $dm^{-3}$ to 0.50 mol $dm^{-3}$ is 3.2 hours . if the decomposition of X is a second order reaction, how long would it take for the concentration of X decrease from 0.50 mol $dm^{-3}$ to 0.25 mol $dm^{-3}$ ?

a)

3.2 hours

b)

4.8 hours

c)

6.4 hours

d)

7.2 hours

13.

The rate of reaction between two gaseous reactants is much slower than the rate of reaction between two reactants in aqueous form because

a)

the gas molecules move too fast

b)

the gaseous reactants cannot form a stable intermediate

c)

the repulsive forces between gaseous reactants are much stronger

d)

the probability of an effective collasion happening is very low

14.

which of the following statements regarding collision theory and transition state theory is not correct?

a)

activation energy always positive

b)

reactant collision must be oriented properly to form products

c)

all reactants collision form products

d)

reactant molecules must be absorb energy to form transition state

15.

Which of the following does not increase the rate of a reacton between a solid and an aqueous solutio?

a)

use the reactants in finely divided state

b)

increases the tempreture of the solution

c)

increase the mixture of the reacting mixtures

d)

use the suitable substance that can lower the activation energy

Reaction Kinetics_MyOmar

Total questions: 15

Worksheet time: 13mins

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