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, A + B → P = - d [ A ] d t = - d [ B ] d t = k [ A ] [ B ] and k t = 1 [ A ] 0 - [ B ] 0 ln [ A ] [ B ] 0 [ B ] [ A ] 0 when, [ A ] 0 ≠ [ B ] 0 If, [ A ] 0 = [ B ] 0 then the integrated rate law will he

1 [ A ] = 1 [ A ] 0 + k t or 1 [ B ] = 1 [ B ] 0 + k t

EASY

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Identify a concentration verses time graph for a second order reaction with single reactant.

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Important Questions on Chemical Kinetics (AHL)

EASY

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

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

HARD

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

Which of the following plots is(are) correct for the given reaction?

( $[P]_{0}$ is the initial concentration of $P$ )

Question Image

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

For the reaction,

2 A + B \to 3 C + D

, which of the following does not express the reaction rate?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

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

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

EASY

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

The unit of the rate constant of a zero-order reaction is _____. (

mole - litre per second / mole per litre per second

)

HARD

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

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

HARD

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

For the following reaction

2 X + Y \overset{k}{\to} P

the rate of reaction is

\frac{d [P]}{dt} = k [X]

. Two moles of

X

are mixed with one mole of

Y

to make

1.0 L

of solution. At

50 s, 0.5

mole of

Y

is left in the reaction mixture. The correct statement(s) about the reaction is(are)

(

Use:

\ln 2 = 0.693)

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

Slope of the straight line obtained by plotting

{log}_{10} k

against

\frac{1}{T}

represents which term?

HARD

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

According to the Arrhenius equation,

HARD

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

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)

HARD

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

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

EASY

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

For the reaction,

$A + B \to P = - \frac{d [A]}{d t} = - \frac{d [B]}{d t} = k [A] [B]$ and

$k t = \frac{1}{[A]_{0} - [B]_{0}} \ln \frac{[A] [B]_{0}}{[B] [A]_{0}}$ when, $[A]_{0} \neq [B]_{0}$
If, $[A]_{0} = [B]_{0}$ then the integrated rate law will he

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

The half-life period of a first-order chemical reaction is

6.93

minutes. The time required for the completion of

99 %

of the chemical reaction will be

(\log 2 = 0 .301)

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

What is the correct difference between first and second order reactions?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

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:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

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

HARD

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

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:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

In a bimolecular reaction, the steric factor

P

was experimentally determined to be

4.5

. The correct option(s) among the following is(are)

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

For a second order reaction, (

2 A \to

Product)

\frac{1}{[A]}

t

is represented as

EASY

Chemistry>Physical Chemistry>Chemical Kinetics (AHL)>Rate Equation

The ratio of the half-life time

(t_{1 / 2}),

to the three quarter life-time,

(t_{3 / 4}),

for a reaction that is sècond order

Identify a concentration verses time graph for a second order reaction with single reactant.

Important Questions on Chemical Kinetics (AHL)

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