R.C. Mukherjee Test: Chemical Kinetics

Question 1

The rate of a reaction is expressed in different ways as follows :

=

The reaction is :

Accepted Answer

B + 3D → 4A + 2C

Answer

4A + B → 2C + 3D

Answer

A + B → C + D

Answer

B + D → A + C

Question 2

The rate constant for the forward reaction A(g) 2B(g) is 1.5 × 10^-3 s^-1 at 100 K. If 10^-5moles of A and 100 moles of B are present in a 10 litre vessel at equilibrium then rate constant for the backward reaction at this temperature is

Accepted Answer

1.5 × 10^-11

Answer

1.50 × 10⁴ L mol^-1 s^-1

Answer

1.5 × 10¹¹ L mol^-1 s^-1

Answer

1.5 × 10¹⁰ L mol^-1 s^-1

Question 3

Reaction A + B → C + D follow's following rate law : rate = k[A]^+1/2[B]^1/2. Starting with initial conc. of 1 M of A and B each, what is the time taken for concentration of A of become 0.25 M.

Given : k = 2.303 × 10^-3 sec^-1.

Accepted Answer

600 sec

Answer

300 sec

Answer

900 sec

Answer

none of these

Question 4

Consider the following first order competing reactions :

X A+ B and y C+D

if 50% of the reaction of X was completed when 96% of the reaction of Y was completed, the ratio of their rate constants is

Accepted Answer

4.65

Answer

4.06

Answer

0.215

Answer

1.1

Question 5

Units of rate constant for first and zero order reactions in terms of molarity (M) are respectively.

Accepted Answer

sec^-1, M sec^-1

Answer

sec-1, M

Answer

M sec^-1, sec^-1

Answer

M, sec-1

Question 6

The rate of a chemical reaction doubles for every 10°C rise of temperature. If the temperature is raised by 50°C, the rate of the reaction increases by about

Accepted Answer

32 times

Answer

64 times

Answer

10 times

Answer

24 times

Question 7

For a reaction pA + qB → products, the rate law expression is r = k[A]^l[B]^m, then :

Accepted Answer

(p + q) may or may not be equal to (I + m)

Answer

(p + q) < (1 + m)

Answer

(p + q) > (1 + m)

Answer

(p + q) = (1 + m)

Question 8

In the reaction : A + 2B → 3C + D, which of the following expression does not describe changes in the conc. of various species as a function of time :

Accepted Answer

{2d[B]/dt} = {d[A]/dt}

Answer

{-d[C]/dt} = {3/2d[B]/dt}

Answer

{3d[D]/dt} = {d[C]/dt}

Answer

{3d[B]/dt} = {-2d[C]/dt}

Question 9

A first order reaction is 87.5% complete in an hour. The rate constant of the reaction is

Accepted Answer

0.0346 min^–1

Answer

0.0693 h^–1

Answer

0.0693 min^–1

Answer

0.0346 h^–1

Question 10

Half-life period of a second order reaction is

Accepted Answer

inversely proportional to the initial conc

Answer

independent of the concentration

Answer

inversely proportional to conc.

Answer

directly proportional to the conc.

Question 11

A first order reaction is 50% completed in 20 minutes at 27°C and in 5 min at 47°C. The energy of activation of the reaction is

Accepted Answer

55.3 kJ/mol

Answer

43.85 kJ/mol

Answer

11.97 kJ/mol

Answer

6.65 kJ/mol

Question 12

For the first order reaction A → B + C, carried out at 27°C if 3.8 × 10^-16% of the reactant molecules exists in the activated state, the E_a (activation energy) of the reaction is

Accepted Answer

100 KJ/mole

Answer

12 kJ/mole

Answer

831.4 kJ/mole

Answer

88.57 kJ/mole

Question 13

The rate constant, the activation energy and the Arrhenius parameter (A) of a chemical reaction at 25°C are 3.0 × 10^-4 s^-1, 104.4 kJ mol^-1 and 6.0 × 10^-4s^-1respectively. The value of the rate constant at T → ∞ is

Accepted Answer

6 × 10^-4 s^-1

Answer

2.0 × 10¹⁸ s^-1

Answer

6.0 × 10¹⁴ s^-1

Answer

infinity

Question 14

The following mechanism has been proposed for the exothermic catalyzed complex reaction.

If k₁ is much smaller than k₂. The most suitable qualitative plot of potential energy (P.E.) versus reaction coordinate for the above reaction.

Accepted Answer

Answer

Answer

Answer

Question 15

The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol^–1. The ratio of rate constant to the Arrhenius factor is

Accepted Answer

0.1

Answer

0.01

Answer

0.001

Answer

0.02

Question 16

Consider + heat, If activation energy for forward reaction is 100 kJ/mole then activation energy for backward reaction and heat of reaction is :

Accepted Answer

140,40

Answer

100, 200

Answer

80,20

Answer

120,220

Question 17

In a reaction, the thershold energy is equal to :

Accepted Answer

Activation energy + normal energy of reactants

Answer

Activation energy - normal energy of reactants

Answer

Activation energy

Answer

Normal energy of reactants.

Question 18

The first order rate constant k is related to temperature as log k = 15.0 - (10⁶/T). Which of the following pair of value is correct ?

Accepted Answer

A = 10¹⁵ and E = 1.9 × 10⁴ KJ

Answer

A = 10^-15 and E = 40 KJ

Answer

A = 10¹⁵ and E = 40 KJ

Answer

A = 10^-15 and E = 1.9 × 10⁴ KJ

Question 19

When a graph between log K and 1/T is drawn a straight line is obtained. The temperature at which line cuts y-axis and x-axis.

Accepted Answer

∞, E_a/(R ln A)

Answer

0, E_a/2.303 R log A

Answer

0, log A

Answer

None of these

Question 20

The rate constant, the activation energy and the frequency factor of a chemical reaction at 25°C are 3.0 × 10^-2 s^-1, 104.4 KJ mol^-1 and 6.0 × 10¹⁴ s^-1 respectively. The value of the rate constant as T → ∞ is :

Accepted Answer

6.0 × 10¹⁴ s^-1

Answer

2.0 × 10¹⁸ s^-1

Answer

Infinity

Answer

3.6 × 10³⁰ s^-1

Question 21

The rate data for the net reaction at 25°C for the reaction X + 2Y → 3Z are given below :

[X₀] [Y₀] Time required for [Z] to increase by 0.005 mol per litre.

0.01 0.01 72 sec

0.02 0.005 36 sec

0.02 0.01 18 sec

The intial rate (as given by Z) is :

Accepted Answer

Second order in X and first order in Y

Answer

First order in both X and Y

Answer

First order in X and second order in Y

Answer

None of the above

Question 22

The rate of production of NH₃ in N₂ + 3H₂ → 2NH₃ is 3.4 kg min^-1. The rate of consumption of H₂ is :

Accepted Answer

5.1 kg min^-1

Answer

0.01 kg sec^-1

Answer

0.6 kg hr^-1

Answer

None of these

Question 23

For a given reaction of first order it takes 20 min. for the conc. to drop from 1.0 M to 0.60 M. The time required for the conc. to drop from 0.60 M to 0.36 M will be :

Accepted Answer

20 min

Answer

More than 20 min

Answer

Less than 30 min

Answer

Cannot tell.

Question 24

For a first order reaction, the concentration of reactant :

Accepted Answer

Varies exponentially with time

Answer

Is independent of time

Answer

Varies linearly with time

Answer

None

Question 25

Radioactivity of a sample (z = 22) decreases 90% after 10 years. What will be the half-life of the sample?

Accepted Answer

3 years

Answer

5 years

Answer

2 years

Answer

10 years

Question 26

Mathematical representation for t_1/4 life for first order reaction is over is given by :

Accepted Answer

t_1/4 = [(2.303)/(K)] log(4/3)

Answer

t_1/4 = [(2.303)/(K)] log 4

Answer

t_1/4 = [(2.303/(K)] log 3

Answer

t_1/4 = [(2.303)/(K)]log(3/4)

Question 27

For a reaction A → Products, the conc. of reactant C₀, aC₀, a²C₀, a³C₀............ after time interval 0, t, 2t ............ where 'a' is constant. Then :

Accepted Answer

Reaction is of 1st order and K = (1/t) ln (1/a)

Answer

Reaction is of 1 st order and K = (1/t) ln a

Answer

Reaction is of 2nd order and K = (1/tC₀)(1 – a)/a

Answer

Reaction is of zero order and K = {(1 – a)}C₀/t

Question 28

Half-life is independent of conc. of A. After 10 minutes volume N₂ gas is 10 L and after complete reaction 50 L. Hence rate constant in min^-1 :

Accepted Answer

(2.303/10) log 1.25

Answer

(2.303/10) log 5

Answer

(2.303/10) log 2

Answer

(2.303/10) log 4

Question 29

In a zero-order reaction for every 10° rise of temperature, the rate is doubled. If the temperature is increased from 10°C to 100°C, the rate of the reaction will become

Accepted Answer

512 times

Answer

64 times

Answer

128 times

Answer

256 times

Question 30

In acidic medium the rate of reaction between (BrO₃)^- & Br^- ions is given by the expression, –[d(BrO₃^-) /dt] = K[BrO₃^-][Br^-][H⁺]²It means :

Accepted Answer

Doubling the conc. of H⁺ ions will increase the reaction rate by 4 times.

Answer

Rate constant of overall reaction is 4 sec^-1

Answer

Rate of reaction is independent of the conc. of acid

Answer

The change in pH of the solution will not affect the rate

Chemical Kinetics - Free MCQ Practice Test with solutions, JEE Chemistry

MCQ Practice Test & Solutions: R.C. Mukherjee Test: Chemical Kinetics (30 Questions)

The rate of a reaction is expressed in different ways as follows : = The reaction is :

The rate constant for the forward reaction A(g) 2B(g) is 1.5 × 10-3 s-1 at 100 K. If 10-5 moles of A and 100 moles of B are present in a 10 litre vessel at equilibrium then rate constant for the backward reaction at this temperature is

Reaction A + B → C + D follow's following rate law : rate = k[A]+1/2[B]1/2. Starting with initial conc. of 1 M of A and B each, what is the time taken for concentration of A of become 0.25 M.Given : k = 2.303 × 10-3 sec-1.

Consider the following first order competing reactions :X A+ B and y C+Dif 50% of the reaction of X was completed when 96% of the reaction of Y was completed, the ratio of their rate constants is

Units of rate constant for first and zero order reactions in terms of molarity (M) are respectively.

The rate of a chemical reaction doubles for every 10°C rise of temperature. If the temperature is raised by 50°C, the rate of the reaction increases by about

For a reaction pA + qB → products, the rate law expression is r = k[A]l[B]m, then :

In the reaction : A + 2B → 3C + D, which of the following expression does not describe changes in the conc. of various species as a function of time :

A first order reaction is 87.5% complete in an hour. The rate constant of the reaction is

Half-life period of a second order reaction is

A first order reaction is 50% completed in 20 minutes at 27°C and in 5 min at 47°C. The energy of activation of the reaction is

For the first order reaction A → B + C, carried out at 27°C if 3.8 × 10-16% of the reactant molecules exists in the activated state, the Ea (activation energy) of the reaction is

The rate constant, the activation energy and the Arrhenius parameter (A) of a chemical reaction at 25°C are 3.0 × 10-4 s-1, 104.4 kJ mol-1 and 6.0 × 10-4s-1respectively. The value of the rate constant at T → ∞ is

The following mechanism has been proposed for the exothermic catalyzed complex reaction.If k1 is much smaller than k2. The most suitable qualitative plot of potential energy (P.E.) versus reaction coordinate for the above reaction.

The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol–1. The ratio of rate constant to the Arrhenius factor is

Consider + heat, If activation energy for forward reaction is 100 kJ/mole then activation energy for backward reaction and heat of reaction is :

In a reaction, the thershold energy is equal to :

The first order rate constant k is related to temperature as log k = 15.0 - (106/T). Which of the following pair of value is correct ?

When a graph between log K and 1/T is drawn a straight line is obtained. The temperature at which line cuts y-axis and x-axis.

The rate constant, the activation energy and the frequency factor of a chemical reaction at 25°C are 3.0 × 10-2 s-1, 104.4 KJ mol-1 and 6.0 × 1014 s-1 respectively. The value of the rate constant as T → ∞ is :

The rate data for the net reaction at 25°C for the reaction X + 2Y → 3Z are given below :[X0] [Y0] Time required for [Z] to increase by 0.005 mol per litre.0.01 0.01 72 sec0.02 0.005 36 sec0.02 0.01 18 secThe intial rate (as given by Z) is :

The rate of production of NH3 in N2 + 3H2 → 2NH3 is 3.4 kg min-1. The rate of consumption of H2 is :

For a given reaction of first order it takes 20 min. for the conc. to drop from 1.0 M to 0.60 M. The time required for the conc. to drop from 0.60 M to 0.36 M will be :

For a first order reaction, the concentration of reactant :

Radioactivity of a sample (z = 22) decreases 90% after 10 years. What will be the half-life of the sample?

Mathematical representation for t1/4 life for first order reaction is over is given by :

For a reaction A → Products, the conc. of reactant C0, aC0, a2C0, a3C0............ after time interval 0, t, 2t ............ where 'a' is constant. Then :

Half-life is independent of conc. of A. After 10 minutes volume N2 gas is 10 L and after complete reaction 50 L. Hence rate constant in min-1 :

In a zero-order reaction for every 10° rise of temperature, the rate is doubled. If the temperature is increased from 10°C to 100°C, the rate of the reaction will become

In acidic medium the rate of reaction between (BrO3)- & Br- ions is given by the expression, –[d(BrO3-) /dt] = K[BrO3-][Br-][H +]2 It means :

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The rate of a reaction is expressed in different ways as follows :
=
The reaction is :