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CHXII04:CHEMICAL KINETICS

320590 For the reaction, $3 A + 2 B \to C + D$ , the differential rate law can be written as

1

- \frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

2

+ \frac{1}{3} \frac{d [A]}{dt} = - \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

3

\frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

4

- \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

Explanation:

Rate $= - \frac{1}{3} \frac{d [A]}{dt} = - \frac{1}{2} \frac{d [B]}{dt} = \frac{d [C]}{dt} = \frac{d [D]}{dt}$
$\begin{aligned} Rate = k [A]^{n} [B]^{m} \\ \begin{aligned} - \frac{1}{3} \frac{d [A]}{dt} & = - \frac{1}{2} \frac{d [B]}{dt} = \frac{d [C]}{dt} = \frac{d [D]}{dt} \\ = k [A]^{n} [B]^{m} \end{aligned} \end{aligned}$
$So, - \frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}$

JEE - 2014

CHXII04:CHEMICAL KINETICS

320591 Identify the incorrect statement

1 Rusting of iron in the presence of air and moisture, is a slow reaction.

2 Inversion of a cane sugar occurs at a moderate rate.

3 Hydrolysis of starch is a fast reaction.

4 Ionic reactions are the examples of fast reactions.

CHXII04:CHEMICAL KINETICS

320592 The rate of a chemical reaction

1 Increases as the reaction proceeds

2 May increase or decrease during the reaction

3 Decreases as the reaction proceeds

4 Remains constant as the reaction proceeds

CHXII04:CHEMICAL KINETICS

320593 What is the rate of appearance of $Z$ in following reaction? $3 x \to 2 y + z$ , if rate of disappearance of $x$ is $0 .072 mol s^{- 1}$ .

1

0 .072 mol s^{-  1}

2

0 .048 mol s^{-  1}

3

0 .024 mol s^{-  1}

4

0 .096 mol s^{-  1}

Explanation:

$3x \to 2y + z$
Rate of formation $= - \frac{1}{3} \frac{d [x]}{dt} = \frac{1}{2} \frac{d [y]}{dt} = \frac{d [z]}{dt}$
$\frac{d [z]}{dt} = \frac{1}{3} (0.072) = 0.024 mol s^{- 1}$

MHTCET - 2021

CHXII04:CHEMICAL KINETICS

320590 For the reaction, $3 A + 2 B \to C + D$ , the differential rate law can be written as

1

- \frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

2

+ \frac{1}{3} \frac{d [A]}{dt} = - \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

3

\frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

4

- \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

Explanation:

Rate $= - \frac{1}{3} \frac{d [A]}{dt} = - \frac{1}{2} \frac{d [B]}{dt} = \frac{d [C]}{dt} = \frac{d [D]}{dt}$
$\begin{aligned} Rate = k [A]^{n} [B]^{m} \\ \begin{aligned} - \frac{1}{3} \frac{d [A]}{dt} & = - \frac{1}{2} \frac{d [B]}{dt} = \frac{d [C]}{dt} = \frac{d [D]}{dt} \\ = k [A]^{n} [B]^{m} \end{aligned} \end{aligned}$
$So, - \frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}$

JEE - 2014

CHXII04:CHEMICAL KINETICS

320591 Identify the incorrect statement

1 Rusting of iron in the presence of air and moisture, is a slow reaction.

2 Inversion of a cane sugar occurs at a moderate rate.

3 Hydrolysis of starch is a fast reaction.

4 Ionic reactions are the examples of fast reactions.

CHXII04:CHEMICAL KINETICS

320592 The rate of a chemical reaction

1 Increases as the reaction proceeds

2 May increase or decrease during the reaction

3 Decreases as the reaction proceeds

4 Remains constant as the reaction proceeds

CHXII04:CHEMICAL KINETICS

320593 What is the rate of appearance of $Z$ in following reaction? $3 x \to 2 y + z$ , if rate of disappearance of $x$ is $0 .072 mol s^{- 1}$ .

1

0 .072 mol s^{-  1}

2

0 .048 mol s^{-  1}

3

0 .024 mol s^{-  1}

4

0 .096 mol s^{-  1}

Explanation:

$3x \to 2y + z$
Rate of formation $= - \frac{1}{3} \frac{d [x]}{dt} = \frac{1}{2} \frac{d [y]}{dt} = \frac{d [z]}{dt}$
$\frac{d [z]}{dt} = \frac{1}{3} (0.072) = 0.024 mol s^{- 1}$

MHTCET - 2021

CHXII04:CHEMICAL KINETICS

320590 For the reaction, $3 A + 2 B \to C + D$ , the differential rate law can be written as

1

- \frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

2

+ \frac{1}{3} \frac{d [A]}{dt} = - \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

3

\frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

4

- \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

Explanation:

Rate $= - \frac{1}{3} \frac{d [A]}{dt} = - \frac{1}{2} \frac{d [B]}{dt} = \frac{d [C]}{dt} = \frac{d [D]}{dt}$
$\begin{aligned} Rate = k [A]^{n} [B]^{m} \\ \begin{aligned} - \frac{1}{3} \frac{d [A]}{dt} & = - \frac{1}{2} \frac{d [B]}{dt} = \frac{d [C]}{dt} = \frac{d [D]}{dt} \\ = k [A]^{n} [B]^{m} \end{aligned} \end{aligned}$
$So, - \frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}$

JEE - 2014

CHXII04:CHEMICAL KINETICS

320591 Identify the incorrect statement

1 Rusting of iron in the presence of air and moisture, is a slow reaction.

2 Inversion of a cane sugar occurs at a moderate rate.

3 Hydrolysis of starch is a fast reaction.

4 Ionic reactions are the examples of fast reactions.

CHXII04:CHEMICAL KINETICS

320592 The rate of a chemical reaction

1 Increases as the reaction proceeds

2 May increase or decrease during the reaction

3 Decreases as the reaction proceeds

4 Remains constant as the reaction proceeds

CHXII04:CHEMICAL KINETICS

320593 What is the rate of appearance of $Z$ in following reaction? $3 x \to 2 y + z$ , if rate of disappearance of $x$ is $0 .072 mol s^{- 1}$ .

1

0 .072 mol s^{-  1}

2

0 .048 mol s^{-  1}

3

0 .024 mol s^{-  1}

4

0 .096 mol s^{-  1}

Explanation:

$3x \to 2y + z$
Rate of formation $= - \frac{1}{3} \frac{d [x]}{dt} = \frac{1}{2} \frac{d [y]}{dt} = \frac{d [z]}{dt}$
$\frac{d [z]}{dt} = \frac{1}{3} (0.072) = 0.024 mol s^{- 1}$

MHTCET - 2021

CHXII04:CHEMICAL KINETICS

320590 For the reaction, $3 A + 2 B \to C + D$ , the differential rate law can be written as

1

- \frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

2

+ \frac{1}{3} \frac{d [A]}{dt} = - \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

3

\frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

4

- \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}

Explanation:

Rate $= - \frac{1}{3} \frac{d [A]}{dt} = - \frac{1}{2} \frac{d [B]}{dt} = \frac{d [C]}{dt} = \frac{d [D]}{dt}$
$\begin{aligned} Rate = k [A]^{n} [B]^{m} \\ \begin{aligned} - \frac{1}{3} \frac{d [A]}{dt} & = - \frac{1}{2} \frac{d [B]}{dt} = \frac{d [C]}{dt} = \frac{d [D]}{dt} \\ = k [A]^{n} [B]^{m} \end{aligned} \end{aligned}$
$So, - \frac{1}{3} \frac{d [A]}{dt} = \frac{d [C]}{dt} = k [A]^{n} [B]^{m}$

JEE - 2014

CHXII04:CHEMICAL KINETICS

320591 Identify the incorrect statement

1 Rusting of iron in the presence of air and moisture, is a slow reaction.

2 Inversion of a cane sugar occurs at a moderate rate.

3 Hydrolysis of starch is a fast reaction.

4 Ionic reactions are the examples of fast reactions.

CHXII04:CHEMICAL KINETICS

320592 The rate of a chemical reaction

1 Increases as the reaction proceeds

2 May increase or decrease during the reaction

3 Decreases as the reaction proceeds

4 Remains constant as the reaction proceeds

CHXII04:CHEMICAL KINETICS

320593 What is the rate of appearance of $Z$ in following reaction? $3 x \to 2 y + z$ , if rate of disappearance of $x$ is $0 .072 mol s^{- 1}$ .

1

0 .072 mol s^{-  1}

2

0 .048 mol s^{-  1}

3

0 .024 mol s^{-  1}

4

0 .096 mol s^{-  1}

Explanation:

$3x \to 2y + z$
Rate of formation $= - \frac{1}{3} \frac{d [x]}{dt} = \frac{1}{2} \frac{d [y]}{dt} = \frac{d [z]}{dt}$
$\frac{d [z]}{dt} = \frac{1}{3} (0.072) = 0.024 mol s^{- 1}$

MHTCET - 2021

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