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

HARD

Earn 100

Two reactions (I) $A \to$ Products (II) $B \to$ Products follow first order kinetics. The rate of the reaction (I) is doubled when temperature is raised from $300 K$ to $310 K$ . The half-life for this reaction at $310 K$ is $30$ minute. At the same temperature $B$ decomposes twice as fast as $A$ . If the energy of activation for the reaction (II) is half that of reaction (I) calculate the rate constant of reaction (II) at $300 K$

Important Questions on Chemical Kinetics

EASY

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

For a chemical reaction rate law is, rate

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

If [A] is doubled at constant

II : 2.303 \log_{10} \frac{K_{II} at 310}{K_{II} at 300} = \frac{E_{a_{II}}}{R} [\frac{310 - 300}{310 \times 300}] . . . . . . . . . . (6)

the rate of reaction.

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Order of a 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>Order of a 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:

HARD

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

The results given in the below table were obtained during kinetic studies of the following reaction: $(10)$

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>Order of a 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

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Order of a 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:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Order of a 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:

MEDIUM

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

The rate constant for a second order reaction,

A \to

Product, is

1.62 M^{- 1} s^{- 1}

. What will be the rate of reaction when concentration of reactant is

2 \times 10^{- 3} M

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Order of a 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:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Order of a 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>Order of a 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: