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CHXII04:CHEMICAL KINETICS

320141 Assertion :
The overall order of the reaction is the sum of the exponents of all the reactants in the rate expression.
Reason :
There are many higher order reactions.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII04:CHEMICAL KINETICS

320142 What is the order of a reaction which has a rate expression: rate $= k [A]^{3 / 2} [B]^{- 1}$

1

\frac{3}{2}

2

\frac{1}{2}

3 Zero

4 None

Explanation:

order $= \frac{3}{2} - 1 = \frac{1}{2}$ (order is sum of the powers of conc. terms in rate law).

CHXII04:CHEMICAL KINETICS

320143 The rate of the reaction ${CCl}_{3} CHO + NO \to {CHCl}_{3} + NO + CO$ is given by Rate $= K [{CCl}_{3} CHO] [NO]$ . If concentration is expressed in moles/litre, the units of k are

1

l i t r e^{2} m o l e^{- 2} s e c^{- 1}

2

m o l e l i t r e^{- 1} s e c^{- 1}

3

l i t r e m o l e^{- 1} s e c^{- 1}

4

s e c^{- 1}

Explanation:

It is a second-order reaction and the unit of rate constant, $k$ for second order reaction is litre ${mole}^{- 1} \sec^{- 1}$

CHXII04:CHEMICAL KINETICS

320144 The rate constants for forward reaction and backward reaction of hydrolysis of ester are $1.1 \times 10^{- 2} \min^{- 1}$ and $1.5 \times 10^{- 3} \min^{- 1}$ respectively. Equilibrium constant for the reaction is $C H_{3} COOC 2_{2} H_{5} + H_{2} O ⇌ C H_{3} COOH + C_{2} H_{5} OH$

1 33.7

2 7.33

3 5.33

4 33.3

Explanation:

$k_{f} = 1.1 \times 10^{- 2}, k_{b} = 1.5 \times 10^{- 3}$
$K_{c} = \frac{k_{f}}{k_{b}} = \frac{1.1 \times 10^{- 2}}{1.5 \times 10^{- 3}} = 7.33$

CHXII04:CHEMICAL KINETICS

320145 The unit of rate constant, $k$ for a third order reaction is ${mol}^{- X} L^{X} s^{- 1}$ . The value of ' X ' is ____.

1

\frac{1}{2}

2 2

3

\frac{3}{2}

4

- 1

Explanation:

Unit of rate constant of $n^{th}$ order reaction:
${(m o l L^{- 1})}^{1 - n} s^{- 1} = {(m o l L^{- 1})}^{1 - 3} s^{- 1}$
$= m o l^{- 2} L^{2} s^{- 1}$ .
Hence, the value of ' X ' is 2 .

CHXII04:CHEMICAL KINETICS

320141 Assertion :
The overall order of the reaction is the sum of the exponents of all the reactants in the rate expression.
Reason :
There are many higher order reactions.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII04:CHEMICAL KINETICS

320142 What is the order of a reaction which has a rate expression: rate $= k [A]^{3 / 2} [B]^{- 1}$

1

\frac{3}{2}

2

\frac{1}{2}

3 Zero

4 None

Explanation:

order $= \frac{3}{2} - 1 = \frac{1}{2}$ (order is sum of the powers of conc. terms in rate law).

CHXII04:CHEMICAL KINETICS

320143 The rate of the reaction ${CCl}_{3} CHO + NO \to {CHCl}_{3} + NO + CO$ is given by Rate $= K [{CCl}_{3} CHO] [NO]$ . If concentration is expressed in moles/litre, the units of k are

1

l i t r e^{2} m o l e^{- 2} s e c^{- 1}

2

m o l e l i t r e^{- 1} s e c^{- 1}

3

l i t r e m o l e^{- 1} s e c^{- 1}

4

s e c^{- 1}

Explanation:

It is a second-order reaction and the unit of rate constant, $k$ for second order reaction is litre ${mole}^{- 1} \sec^{- 1}$

CHXII04:CHEMICAL KINETICS

320144 The rate constants for forward reaction and backward reaction of hydrolysis of ester are $1.1 \times 10^{- 2} \min^{- 1}$ and $1.5 \times 10^{- 3} \min^{- 1}$ respectively. Equilibrium constant for the reaction is $C H_{3} COOC 2_{2} H_{5} + H_{2} O ⇌ C H_{3} COOH + C_{2} H_{5} OH$

1 33.7

2 7.33

3 5.33

4 33.3

Explanation:

$k_{f} = 1.1 \times 10^{- 2}, k_{b} = 1.5 \times 10^{- 3}$
$K_{c} = \frac{k_{f}}{k_{b}} = \frac{1.1 \times 10^{- 2}}{1.5 \times 10^{- 3}} = 7.33$

CHXII04:CHEMICAL KINETICS

320145 The unit of rate constant, $k$ for a third order reaction is ${mol}^{- X} L^{X} s^{- 1}$ . The value of ' X ' is ____.

1

\frac{1}{2}

2 2

3

\frac{3}{2}

4

- 1

Explanation:

Unit of rate constant of $n^{th}$ order reaction:
${(m o l L^{- 1})}^{1 - n} s^{- 1} = {(m o l L^{- 1})}^{1 - 3} s^{- 1}$
$= m o l^{- 2} L^{2} s^{- 1}$ .
Hence, the value of ' X ' is 2 .

CHXII04:CHEMICAL KINETICS

320141 Assertion :
The overall order of the reaction is the sum of the exponents of all the reactants in the rate expression.
Reason :
There are many higher order reactions.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII04:CHEMICAL KINETICS

320142 What is the order of a reaction which has a rate expression: rate $= k [A]^{3 / 2} [B]^{- 1}$

1

\frac{3}{2}

2

\frac{1}{2}

3 Zero

4 None

Explanation:

order $= \frac{3}{2} - 1 = \frac{1}{2}$ (order is sum of the powers of conc. terms in rate law).

CHXII04:CHEMICAL KINETICS

320143 The rate of the reaction ${CCl}_{3} CHO + NO \to {CHCl}_{3} + NO + CO$ is given by Rate $= K [{CCl}_{3} CHO] [NO]$ . If concentration is expressed in moles/litre, the units of k are

1

l i t r e^{2} m o l e^{- 2} s e c^{- 1}

2

m o l e l i t r e^{- 1} s e c^{- 1}

3

l i t r e m o l e^{- 1} s e c^{- 1}

4

s e c^{- 1}

Explanation:

It is a second-order reaction and the unit of rate constant, $k$ for second order reaction is litre ${mole}^{- 1} \sec^{- 1}$

CHXII04:CHEMICAL KINETICS

320144 The rate constants for forward reaction and backward reaction of hydrolysis of ester are $1.1 \times 10^{- 2} \min^{- 1}$ and $1.5 \times 10^{- 3} \min^{- 1}$ respectively. Equilibrium constant for the reaction is $C H_{3} COOC 2_{2} H_{5} + H_{2} O ⇌ C H_{3} COOH + C_{2} H_{5} OH$

1 33.7

2 7.33

3 5.33

4 33.3

Explanation:

$k_{f} = 1.1 \times 10^{- 2}, k_{b} = 1.5 \times 10^{- 3}$
$K_{c} = \frac{k_{f}}{k_{b}} = \frac{1.1 \times 10^{- 2}}{1.5 \times 10^{- 3}} = 7.33$

CHXII04:CHEMICAL KINETICS

320145 The unit of rate constant, $k$ for a third order reaction is ${mol}^{- X} L^{X} s^{- 1}$ . The value of ' X ' is ____.

1

\frac{1}{2}

2 2

3

\frac{3}{2}

4

- 1

Explanation:

Unit of rate constant of $n^{th}$ order reaction:
${(m o l L^{- 1})}^{1 - n} s^{- 1} = {(m o l L^{- 1})}^{1 - 3} s^{- 1}$
$= m o l^{- 2} L^{2} s^{- 1}$ .
Hence, the value of ' X ' is 2 .

CHXII04:CHEMICAL KINETICS

320141 Assertion :
The overall order of the reaction is the sum of the exponents of all the reactants in the rate expression.
Reason :
There are many higher order reactions.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII04:CHEMICAL KINETICS

320142 What is the order of a reaction which has a rate expression: rate $= k [A]^{3 / 2} [B]^{- 1}$

1

\frac{3}{2}

2

\frac{1}{2}

3 Zero

4 None

Explanation:

order $= \frac{3}{2} - 1 = \frac{1}{2}$ (order is sum of the powers of conc. terms in rate law).

CHXII04:CHEMICAL KINETICS

320143 The rate of the reaction ${CCl}_{3} CHO + NO \to {CHCl}_{3} + NO + CO$ is given by Rate $= K [{CCl}_{3} CHO] [NO]$ . If concentration is expressed in moles/litre, the units of k are

1

l i t r e^{2} m o l e^{- 2} s e c^{- 1}

2

m o l e l i t r e^{- 1} s e c^{- 1}

3

l i t r e m o l e^{- 1} s e c^{- 1}

4

s e c^{- 1}

Explanation:

It is a second-order reaction and the unit of rate constant, $k$ for second order reaction is litre ${mole}^{- 1} \sec^{- 1}$

CHXII04:CHEMICAL KINETICS

320144 The rate constants for forward reaction and backward reaction of hydrolysis of ester are $1.1 \times 10^{- 2} \min^{- 1}$ and $1.5 \times 10^{- 3} \min^{- 1}$ respectively. Equilibrium constant for the reaction is $C H_{3} COOC 2_{2} H_{5} + H_{2} O ⇌ C H_{3} COOH + C_{2} H_{5} OH$

1 33.7

2 7.33

3 5.33

4 33.3

Explanation:

$k_{f} = 1.1 \times 10^{- 2}, k_{b} = 1.5 \times 10^{- 3}$
$K_{c} = \frac{k_{f}}{k_{b}} = \frac{1.1 \times 10^{- 2}}{1.5 \times 10^{- 3}} = 7.33$

CHXII04:CHEMICAL KINETICS

320145 The unit of rate constant, $k$ for a third order reaction is ${mol}^{- X} L^{X} s^{- 1}$ . The value of ' X ' is ____.

1

\frac{1}{2}

2 2

3

\frac{3}{2}

4

- 1

Explanation:

Unit of rate constant of $n^{th}$ order reaction:
${(m o l L^{- 1})}^{1 - n} s^{- 1} = {(m o l L^{- 1})}^{1 - 3} s^{- 1}$
$= m o l^{- 2} L^{2} s^{- 1}$ .
Hence, the value of ' X ' is 2 .

CHXII04:CHEMICAL KINETICS

320141 Assertion :
The overall order of the reaction is the sum of the exponents of all the reactants in the rate expression.
Reason :
There are many higher order reactions.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII04:CHEMICAL KINETICS

320142 What is the order of a reaction which has a rate expression: rate $= k [A]^{3 / 2} [B]^{- 1}$

1

\frac{3}{2}

2

\frac{1}{2}

3 Zero

4 None

Explanation:

order $= \frac{3}{2} - 1 = \frac{1}{2}$ (order is sum of the powers of conc. terms in rate law).

CHXII04:CHEMICAL KINETICS

320143 The rate of the reaction ${CCl}_{3} CHO + NO \to {CHCl}_{3} + NO + CO$ is given by Rate $= K [{CCl}_{3} CHO] [NO]$ . If concentration is expressed in moles/litre, the units of k are

1

l i t r e^{2} m o l e^{- 2} s e c^{- 1}

2

m o l e l i t r e^{- 1} s e c^{- 1}

3

l i t r e m o l e^{- 1} s e c^{- 1}

4

s e c^{- 1}

Explanation:

It is a second-order reaction and the unit of rate constant, $k$ for second order reaction is litre ${mole}^{- 1} \sec^{- 1}$

CHXII04:CHEMICAL KINETICS

320144 The rate constants for forward reaction and backward reaction of hydrolysis of ester are $1.1 \times 10^{- 2} \min^{- 1}$ and $1.5 \times 10^{- 3} \min^{- 1}$ respectively. Equilibrium constant for the reaction is $C H_{3} COOC 2_{2} H_{5} + H_{2} O ⇌ C H_{3} COOH + C_{2} H_{5} OH$

1 33.7

2 7.33

3 5.33

4 33.3

Explanation:

$k_{f} = 1.1 \times 10^{- 2}, k_{b} = 1.5 \times 10^{- 3}$
$K_{c} = \frac{k_{f}}{k_{b}} = \frac{1.1 \times 10^{- 2}}{1.5 \times 10^{- 3}} = 7.33$

CHXII04:CHEMICAL KINETICS

320145 The unit of rate constant, $k$ for a third order reaction is ${mol}^{- X} L^{X} s^{- 1}$ . The value of ' X ' is ____.

1

\frac{1}{2}

2 2

3

\frac{3}{2}

4

- 1

Explanation:

Unit of rate constant of $n^{th}$ order reaction:
${(m o l L^{- 1})}^{1 - n} s^{- 1} = {(m o l L^{- 1})}^{1 - 3} s^{- 1}$
$= m o l^{- 2} L^{2} s^{- 1}$ .
Hence, the value of ' X ' is 2 .