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, 3A + 2B → C + D , the differential rate law can be written as :

- 1 3 d A dt = d C dt = k A n B m

+ 1 3 d A dt = - d C dt = k A n B m

1 3 d A dt = d C dt = k A n B m

For the reaction 2 A + 3 B + 3 2 C → 3 P , which statement is correct?

dn A dt = 2 3 dn B dt = 4 3 dn C dt

d n A d t = 3 2 d n B d t = 3 4 d n C d t

dn A dt = 2 3 dn B dt = 3 4 dn C dt

MEDIUM

Earn 100

Show by using rate law, how much rate of the reaction, $2 NO + O_{2} ⟶ 2 {NO}_{2}$ , will change if the volume of the reaction vessel is reduced to one third of its initial value?

Important Questions on Chemical Kinetics

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

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

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below:

O_{3} (g) + {Cl}^{•} \to O_{2} (g) + {ClO}^{•} (g)

...(i)

k_{i} = 5.2 \times 10^{9} L m o l^{- 1} s^{- 1}

{ClO}^{•} (g) + O^{•} (g) \to O_{2} (g) + {Cl}^{•} (g)

...(ii)

k_{i i} = 2.6 \times 10^{10} L m o l^{- 1} s^{- 1}

The closest rate constant for the overall reaction

O_{3} (g) + O^{•} (g) \to 2 O_{2} (g)

is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For the chemical reaction

N_{2} (g) + 3 H_{2} (g) ⇋ 2 N H_{3} (g)

, the correct option is:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

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:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

Find the unit of the rate constant of a reaction represented with a rate equation, rate

= k {[A]}^{\frac{1}{2}} {[B]}^{\frac{3}{2}}

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

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:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For a reaction scheme

A \overset{k_{1}}{\to} B \overset{k_{2}}{\to} C,

if the net rate of formation of B is set to be zero then the concentration of B is given by:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

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 :

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

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

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For the reaction,

3A + 2B \to C + D

, the differential rate law can be written as :

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

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>The Rate Law and Rate Constant

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?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For the following reactions

Question Image

where,

k_{s}

and

k_{e}

, are respectively, the rate constants for substitution and elimination, and

μ = \frac{k_{s}}{k_{e}}

, the correct option is ________

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

Consider the kinetic data given in the following table for the reaction

A + B + C \to

Product.

Experiment No.	$[A]$ $(m o l {d m}^{- 3})$	$[B]$ $(m o l d m^{- 3})$	$[C]$ $(m o l d m^{- 3})$	Rate of reaction $(m o l d m^{- 3} s^{- 1})$
$1$	$0.2$	$0.1$	$0.1$	$6.0 \times 10^{- 5}$
$2$	$0.2$	$0.2$	$0.1$	$6.0 \times 10^{- 5}$
$3$	$0.2$	$0.1$	$0.2$	$1.2 \times 10^{- 4}$
$4$	$0.3$	$0.1$	$0.1$	$9.0 \times 10^{- 5}$

The rate of the reaction for

[A] = 0.15 m o l d m^{- 3}, [B] = 0.25 m o l d m^{- 3}

and

[C] = 0.15 m o l d m^{- 3}

is found to be

Y \times 10^{- 5} m o l d m^{- 3} s^{- 1} .

The value of

Y

is __________

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For the reaction

2 H_{2} (g) + 2 N O (g) \to N_{2} (g) + 2 H_{2} O (g)

the observed rate expression is, rate

= k_{f} {[NO]}^{2} [H_{2}]

. The rate expression for the reverse reaction is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

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 :

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For the reaction

2 A + 3 B + \frac{3}{2} C \to 3 P

, which statement is correct?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

The rate law for the reaction below is given by the expression

k [A] [B]

A + B \to P r o d u c t

If the concentration of

B

is increased from

0.1 to 0.3 mol

, keeping the value of

A

0.1 mol

, the rate constant will be:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For the non-stoichiometry reaction,

2 A + B \to C + D

, the following kinetic data were obtained in three separate experiments, all at

298 K

Initial Concentration (A)	Initial Concentration (B)	Initial rate of formation of C $({mol L}^{-} S^{-})$
$0.1 M$	$0.1 M$	$1.2 \times 1 0^{- 3}$
$0.1 M$	$0.2 M$	$1.2 \times 1 0^{- 3}$
$0.2 M$	$0.1 M$	$2.4 \times 1 0^{- 3}$

The rate law for the formation of

C

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

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

Show by using rate law, how much rate of the reaction, 2NO+O2⟶2NO2, will change if the volume of the reaction vessel is reduced to one third of its initial value?

Important Questions on Chemical Kinetics

Learn and Prepare for any exam you want !

Show by using rate law, how much rate of the reaction, $2 NO + O_{2} ⟶ 2 {NO}_{2}$ , will change if the volume of the reaction vessel is reduced to one third of its initial value?