For a first order reaction A → P , the temperature T dependent rate constant k was found to follow the equation logk =- 2000 1 T + 6 .0 . The pre-exponential factor A and the activation energy E a , respectively, are

1.0 × 10 6 s - 1 and 38.3 kJ mol - 1

1.0 × 10 6 s - 1 and 9.2 kJ mol - 1

1.0 × 10 6 s - 1 and 16.6 kJ mol - 1

For the reaction, 2 A + B → products, when the concentration of A and B both were doubled, the rate of the reaction increased from 0.3 m o l L - 1 s - 1 to 2.4 m o l L - 1 s - 1 . When the concentration of A alone is doubled, the rate increased from 0.3 m o l L - 1 s - 1 to 0.6 m o l L - 1 s - 1 . Which one of the following statements is correct?

Order of the reaction with respect to B is 2

Total order of the reaction is 4

Order of the reaction with respect to A is 2

Order of the reaction with respect to B is 1

HARD

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A radioactive isotope, A undergoes simultaneous decay to different nuclei as :

Assuming that initially neither P nor Q was present, after how many hours, amount of Q will be just double to the amount of A remaining ?

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Important Questions on Chemical Kinetics

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The following results were obtained during kinetic studies of the reaction.

2 A + B \to

product

Experiment	$[A]$ $(in mol L^{- 1})$	$[B]$ $(i n m o l L^{- 1})$	Initial rate of reaction $(in mol L^{- 1} \min^{- 1})$
$I$	$0.10$	$0.20$	$6.93 \times 10^{- 3}$
$II$	$0.10$	$0.25$	$6.93 \times 10^{- 3}$
$III$	$0.20$	$0.30$	$1.386 \times 10^{- 2}$

The time (in minutes) required to consume half of

A

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The half-life of the first-order reaction,

{CH}_{3} CHO (g) \to {CH}_{4} (g) + CO (g)

, if the initial pressure of

{CH}_{3} CHO (g)

80 mm

Hg

and the total pressure at the end of

20

minutes is

120 mm

Hg

, is:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

N_{2} O_{5}

decomposes to

{NO}_{2}

and

O_{2}

follows the first order kinetics. After

50

minutes, the pressure inside the vessel increases from

50 mm Hg

87.5 mm Hg

. The pressure of the gaseous mixture after

100

minutes at constant temperature will be:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The rate of a first-order reaction is

0.04 m o l l^{- 1} s^{- 1}

10

second and

0.03 m o l l^{- 1} s^{- 1}

20

seconds after initiation of the reaction. The half-life period of the reaction is:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

For the reaction

2 N_{2} O_{5} \overset{}{\to} 4 {NO}_{2} + O_{2}

, rate and rate constant are

1.02 \times 10^{- 4} mol {lit}^{- 1} \sec^{- 1}

and

3.4 \times 10^{- 5} \sec^{- 1}

respectively then concentration of

N_{2} O_{5}

at that time will be

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The addition of a catalyst during a chemical reaction alters which of the following quantities?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

Slope of the straight line obtained by plotting

{log}_{10} k

against

\frac{1}{T}

represents which term?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

Decomposition of

X

exhibits a rate constant of

0 .05 μg / year

. How many years are required for the decomposition of

5 μg

X

into

2 .5 μg

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

What is the order with respect to [A], [B] and [C], respectively?

[A]	[B]	[C]	Rate $[M / \sec]$
$0.2$	$0.1$	$0.02$	$8.08 \times 10^{- 3}$
$0.1$	$0.2$	$0.02$	$2.01 \times 10^{- 3}$
$0.1$	$1.8$	$0.18$	$6.03 \times 10^{- 3}$
$0.2$	$0.1$	$0.08$	$6.464 \times 10^{- 2}$

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

For a first order reaction

A \to P,

the temperature

(T)

dependent rate constant

(k)

was found to follow the equation

logk =- (2000) \frac{1}{T} + 6 .0 .

The pre-exponential factor A and the activation energy

E_{a},

respectively, are

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

Consider the given plots for a reaction obeying Arrhenius equation $(0 ° C < T < 300 ° C) :$ ( $K$ and $E_{a}$ are rate constant and activation energy, respectively )

(I)

Question Image

(II)

Question Image

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

When initial concentration of the reactant is doubled, what happens to the half-life period of a zero order reaction?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

For the reaction,

2 A + B \to

products, when the concentration of

A

and

B

both were doubled, the rate of the reaction increased from

0.3 m o l L^{- 1} s^{- 1}

2.4 m o l L^{- 1} s^{- 1} .

When the concentration of

A

alone is doubled, the rate increased from

0.3 m o l L^{- 1} s^{- 1}

0.6 m o l L^{- 1} s^{- 1} .

Which one of the following statements is correct?

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

According to the Arrhenius equation,

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

For an elementary chemical reaction, $A_{2} ⇄_{k_{- 1}}^{k_{1}} 2 A$ , the expression for $\frac{d [A]}{dt}$ is:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

For a first order reaction

A (g) \to 2 B (g) + C (g)

at constant volume and 300 K, the total pressure at the beginning

(t = 0)

and at time are

p_{0} and p_{t}

, respectively. Initially, only A is present with concentration

{[A]}_{0}

, and

t_{\frac{1}{3}}

is the time required for the partial pressure of A to reach

1 / 3^{rd}

of its initial value. The correct option(s) is (are)
(Assume that all these gases behave as ideal gases)

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

For a reaction, consider the plot of $l n k$ versus $1 / T$ given in the figure. If the rate constant of this reaction at $400 K$ is $10^{- 5} s^{- 1}$ , then the rate constant at $500 K$ is:

Question Image