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

HARD

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The decomposition of $N_{2} O_{5}$ in ${CCl}_{4}$ solution at $318 K$ has been studied by monitoring the concentration of $N_{2} O_{5}$ in the solution. Initially the concentration of $N_{2} O_{5}$ is $2.33 M$ and after $184$ minutes, it is reduced to $2.08 M$ . The reaction takes place according to the equation: $2 N_{2} O_{5} ⟶ 4 {NO}_{2} + O_{2}$ .

Calculate the average rate of this reaction in terms of hours, minutes and seconds. What is the rate of production of ${NO}_{2}$ during this period?

Important Questions on Chemical Kinetics

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a 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

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

For the reaction,

3A + 2B \to C + D

, the differential rate law can be written as :

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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 ________

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

For the reaction

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

, which statement is correct?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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>Rate of a Chemical Reaction

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

Important Questions on Chemical Kinetics

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