N O 2 required for a reaction is produced by the decomposition of N 2 O 5 in C C l 4 as per the equation, 2 N 2 O 5 g → 4 N O 2 g + O 2 g . The initial concentration of N 2 O 5 is 3.00 m o l L - 1 and it is 2.75 m o l L - 1 after 30 minutes. The rate of formation of N O 2 is:

1.667 × 10 - 2 m o l L - 1 m i n - 1

8.333 × 10 - 3 m o l L - 1 m i n - 1

4.167 × 10 - 3 m o l L - 1 m i n - 1

2.083 × 10 - 3 m o l L - 1 m i n - 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

EASY

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The plot of 1/[A] versus time is a straight line with k = slope of the line. Other graphs are curved for a second order reaction.

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Important Questions on Chemical Kinetics (AHL)

MEDIUM

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

The rate constant for the first order reaction is

60 s^{- 1} .

How much time will it take to reduce the concentration of the reactant to

\frac{1}{16} t h

value?

MEDIUM

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

Mechanism of a hypothetical reaction

X_{2} + Y_{2} \to 2 XY

is given below:

(i)

X_{2} \to X + X (fast)

(ii)

X + Y_{2} ⇌ XY + Y (slow)

(iii)

X + Y \to XY (fast)

The overall order of the reaction will be

HARD

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

518^{o} C,

the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of

363 Torr

was

1 .00 Torr s^{- 1}

when

5 %

had reacted and

0 .50 Torr s^{- 1}

when 33% had reacted. The order of the reaction is:

MEDIUM

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

For the reaction

2 A + B \to C

, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reactions is:

$[A] (m o l L^{- 1})$	$[B] (m o l L^{- 1})$	$I n i t i a l R a t e$ $(m o l L^{- 1} s^{- 1})$
0.05	0.05	0.045
0.10	0.05	0.090
0.20	0.10	0.72

EASY

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

The rate constant of the reaction

A ⟶ B

0.6 \times 10^{- 3}

mole per liter per second. If the initial concentration of A is 5 M, then the concentration of B after 20 minutes is:

MEDIUM

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

If the rate constant for a first order reaction is

k

, the time

(t)

required for the completion of

99 %

of the reaction is given by

HARD

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

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

15 minutes

. The amount of substance left after one hour will be

MEDIUM

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

The catalyst used in the Contact Process is

EASY

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

A + 2 B \to C

, the rate equation for the reaction is given as

Rate

= k [A] [B]

If the concentration of A is kept the same but that of B is doubled what will happen to the rate itself?

EASY

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

In preparation of sulphuric acid from Sulphur dioxide in lead chamber process. What substance is used as a catalyst?

EASY

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

N O_{2}

required for a reaction is produced by the decomposition of

N_{2} O_{5}

C C l_{4}

as per the equation,

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g) .

The initial concentration of

N_{2} O_{5}

3.00 m o l L^{- 1}

and it is

2.75 m o l L^{- 1}

after 30 minutes. The rate of formation of

N O_{2}

is:

MEDIUM

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

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?

MEDIUM

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

In the following reaction; $x A \to y B$

$\log_{10} [- \frac{d [A]}{d t}] = \log_{10} [- \frac{d [B]}{d t}] + 0.3010$

‘A’ and ‘B’ respectively can be:

EASY

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

For the elementary reaction

M \to N

, the rate of disappearance of

M

increases by a factor of

8

upon doubling the concentration of

M

. The order of the reaction with respect to

M

EASY

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

For a chemical reaction rate law is, rate

= K {[A]}^{2} [B] .

If [A] is doubled at constant

[B],

the rate of reaction.

EASY

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

Consider the following reactions
$A \to P 1; B \to P 2; C \to P 3; D \to P 4$
The order of the above reactions are $a, b, c and d,$ respectively. The following graph is obtained when log[rate] vs.log[conc.] are plotted:

Question Image
Among the following, the correct sequence for the order of the reactions is :

HARD

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

The results given in the below table were obtained during kinetic studies of the following reaction: $2 A + B \to C + D$

Experiment	$[A] / {molL}^{- 1}$	$[B] / {molL}^{- 1}$	Initial rate/ ${molL}^{- 1} \min^{- 1}$
I	$0.1$	$0.1$	$6.00 \times 10^{- 3}$
II	$0.1$	$0.2$	$2.40 \times 10^{- 2}$
III	$0.2$	$0.1$	$1.20 \times 10^{- 2}$
IV	X	$0.2$	$7.20 \times 10^{- 2}$
V	$0.3$	Y	$2.88 \times 10^{- 1}$

X and Y in the given table are respectively :

HARD

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

In the reaction,

P + Q \to R + S

the time taken for

75 %

reaction of

P

is twice the time taken for

50 %

reaction of

P

. The concentration of

Q

varies with reaction time as shown in the figure.The overall order of the reaction is:

Question Image

HARD

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

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

EASY

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

Higher order (>3) reactions are rare due to:

The plot of 1/[A] versus time is a straight line with k = slope of the line. Other graphs are curved for a second order reaction.

Important Questions on Chemical Kinetics (AHL)

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