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CHXII04:CHEMICAL KINETICS

320573 Ammonia and oxygen react at high temperature as $4 {NH}_{3 (g)} + 5 O_{2 (g)} \to 4 {NO}_{(g)} + 6 H_{2} O_{(g)}$ .
If rate of formation of ${NO}_{(g)}$ is $3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}$ , then rate of disappearance of ammonia is

1

7.2 \times 10^{- 3} mol L^{- 1} s^{- 1}

2

1.2 \times 10^{- 3} mol L^{- 1} s^{- 1}

3

2.4 \times 10^{- 3} mol L^{- 1} s^{- 1}

4

3.6 \times 10^{- 3} mol L^{-  1} s^{-  1}

Explanation:

Rate of reaction $= - \frac{1}{4} \frac{d [{NH}_{3}]}{dt}$
$= - \frac{1}{5} \frac{d [O_{2}]}{dt} = \frac{1}{4} \frac{d [NO]}{dt} = \frac{1}{6} \frac{d [H_{2} O]}{dt}$
$∴$ Rate of disappearance of ${NH}_{3} =$ Rate of formation of $NO$
$= 3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}$

MHTCET - 2021

CHXII04:CHEMICAL KINETICS

320574 For an elementary reaction,
$2 A + 3 B \to 4 C + D$ the rate of appearance of
$C$ at time ' $t$ ' is $2.8 \times 10^{- 3} mol L^{- 1} s^{- 1}$ . Rate of disappearance of $B$ at time ' $t$ ' will be

1

\frac{3}{4} (2.8 \times 10^{- 3}) mol L^{- 1} s^{- 1}

2

2 (2.8 \times 10^{- 3}) mol L^{- 1} s^{- 1}

3

\frac{1}{4} (2 .8 \times 1 0^{- 3}) m o l L^{- 1} s^{- 1}

4

\frac{4}{3} (2.8 \times 10^{- 3}) {molL}^{- 1} s^{- 1}

Explanation:

$2 A + 3 B \to 4 C + D$
$\begin{aligned} - \frac{1}{3} \frac{d (B)}{dt} = + \frac{1}{4} \frac{d (C)}{dt} \\ - \frac{d (B)}{dt} = \frac{3}{4} \frac{d (C)}{dt} \\ = \frac{3}{4} (2.8 \times 10^{- 3}) {molL}^{- 1} s^{- 1} \end{aligned}$
Rate of Law and order of reactions

KCET - 2020

CHXII04:CHEMICAL KINETICS

320575 Assertion :
For the reaction, ${PCl}_{5} \to {PCl}_{3} + {Cl}_{2}$ , the concentration of ${PCl}_{5}$ decreases with the increases in concentration of ${PCl}_{3}$ and ${Cl}_{2}$ .
Reason :
During the course of a reaction, the concentration of the reactants decreases while that of products increases.

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.

Explanation:

The reaction demonstrates the fundamental principle of chemical reactions, wherein the consumption of ${PCl}_{5}$ leads to a decrease in its concentration, while the production of ${PCl}_{3}$ and ${Cl}_{2}$ results in an increase in their concentrations. So option (1) is correct .

CHXII04:CHEMICAL KINETICS

320576 For a reaction $\frac{1}{2} A \to 2 B$ , rate of disappearance of 'A' is related to the rate of appearance of 'B' by the expression:

1

- \frac{d [A]}{d t} = \frac{1}{2} \frac{d [B]}{d t}

2

- \frac{d [A]}{d t} = \frac{1}{4} \frac{d [B]}{d t}

3

- \frac{d [A]}{d t} = \frac{d [B]}{d t}

4

- \frac{d [A]}{d t} = 4 \frac{d [B]}{d t}

Explanation:

$\frac{1}{2} A \to 2 B$
$- \frac{2 d [A]}{d t} = + \frac{d [B]}{2 d t} - \frac{d [A]}{d t} = \frac{1}{4} \frac{d [B]}{d t}$

CHXII04:CHEMICAL KINETICS

320573 Ammonia and oxygen react at high temperature as $4 {NH}_{3 (g)} + 5 O_{2 (g)} \to 4 {NO}_{(g)} + 6 H_{2} O_{(g)}$ .
If rate of formation of ${NO}_{(g)}$ is $3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}$ , then rate of disappearance of ammonia is

1

7.2 \times 10^{- 3} mol L^{- 1} s^{- 1}

2

1.2 \times 10^{- 3} mol L^{- 1} s^{- 1}

3

2.4 \times 10^{- 3} mol L^{- 1} s^{- 1}

4

3.6 \times 10^{- 3} mol L^{-  1} s^{-  1}

Explanation:

Rate of reaction $= - \frac{1}{4} \frac{d [{NH}_{3}]}{dt}$
$= - \frac{1}{5} \frac{d [O_{2}]}{dt} = \frac{1}{4} \frac{d [NO]}{dt} = \frac{1}{6} \frac{d [H_{2} O]}{dt}$
$∴$ Rate of disappearance of ${NH}_{3} =$ Rate of formation of $NO$
$= 3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}$

MHTCET - 2021

CHXII04:CHEMICAL KINETICS

320574 For an elementary reaction,
$2 A + 3 B \to 4 C + D$ the rate of appearance of
$C$ at time ' $t$ ' is $2.8 \times 10^{- 3} mol L^{- 1} s^{- 1}$ . Rate of disappearance of $B$ at time ' $t$ ' will be

1

\frac{3}{4} (2.8 \times 10^{- 3}) mol L^{- 1} s^{- 1}

2

2 (2.8 \times 10^{- 3}) mol L^{- 1} s^{- 1}

3

\frac{1}{4} (2 .8 \times 1 0^{- 3}) m o l L^{- 1} s^{- 1}

4

\frac{4}{3} (2.8 \times 10^{- 3}) {molL}^{- 1} s^{- 1}

Explanation:

$2 A + 3 B \to 4 C + D$
$\begin{aligned} - \frac{1}{3} \frac{d (B)}{dt} = + \frac{1}{4} \frac{d (C)}{dt} \\ - \frac{d (B)}{dt} = \frac{3}{4} \frac{d (C)}{dt} \\ = \frac{3}{4} (2.8 \times 10^{- 3}) {molL}^{- 1} s^{- 1} \end{aligned}$
Rate of Law and order of reactions

KCET - 2020

CHXII04:CHEMICAL KINETICS

320575 Assertion :
For the reaction, ${PCl}_{5} \to {PCl}_{3} + {Cl}_{2}$ , the concentration of ${PCl}_{5}$ decreases with the increases in concentration of ${PCl}_{3}$ and ${Cl}_{2}$ .
Reason :
During the course of a reaction, the concentration of the reactants decreases while that of products increases.

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.

Explanation:

The reaction demonstrates the fundamental principle of chemical reactions, wherein the consumption of ${PCl}_{5}$ leads to a decrease in its concentration, while the production of ${PCl}_{3}$ and ${Cl}_{2}$ results in an increase in their concentrations. So option (1) is correct .

CHXII04:CHEMICAL KINETICS

320576 For a reaction $\frac{1}{2} A \to 2 B$ , rate of disappearance of 'A' is related to the rate of appearance of 'B' by the expression:

1

- \frac{d [A]}{d t} = \frac{1}{2} \frac{d [B]}{d t}

2

- \frac{d [A]}{d t} = \frac{1}{4} \frac{d [B]}{d t}

3

- \frac{d [A]}{d t} = \frac{d [B]}{d t}

4

- \frac{d [A]}{d t} = 4 \frac{d [B]}{d t}

Explanation:

$\frac{1}{2} A \to 2 B$
$- \frac{2 d [A]}{d t} = + \frac{d [B]}{2 d t} - \frac{d [A]}{d t} = \frac{1}{4} \frac{d [B]}{d t}$

CHXII04:CHEMICAL KINETICS

320573 Ammonia and oxygen react at high temperature as $4 {NH}_{3 (g)} + 5 O_{2 (g)} \to 4 {NO}_{(g)} + 6 H_{2} O_{(g)}$ .
If rate of formation of ${NO}_{(g)}$ is $3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}$ , then rate of disappearance of ammonia is

1

7.2 \times 10^{- 3} mol L^{- 1} s^{- 1}

2

1.2 \times 10^{- 3} mol L^{- 1} s^{- 1}

3

2.4 \times 10^{- 3} mol L^{- 1} s^{- 1}

4

3.6 \times 10^{- 3} mol L^{-  1} s^{-  1}

Explanation:

Rate of reaction $= - \frac{1}{4} \frac{d [{NH}_{3}]}{dt}$
$= - \frac{1}{5} \frac{d [O_{2}]}{dt} = \frac{1}{4} \frac{d [NO]}{dt} = \frac{1}{6} \frac{d [H_{2} O]}{dt}$
$∴$ Rate of disappearance of ${NH}_{3} =$ Rate of formation of $NO$
$= 3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}$

MHTCET - 2021

CHXII04:CHEMICAL KINETICS

320574 For an elementary reaction,
$2 A + 3 B \to 4 C + D$ the rate of appearance of
$C$ at time ' $t$ ' is $2.8 \times 10^{- 3} mol L^{- 1} s^{- 1}$ . Rate of disappearance of $B$ at time ' $t$ ' will be

1

\frac{3}{4} (2.8 \times 10^{- 3}) mol L^{- 1} s^{- 1}

2

2 (2.8 \times 10^{- 3}) mol L^{- 1} s^{- 1}

3

\frac{1}{4} (2 .8 \times 1 0^{- 3}) m o l L^{- 1} s^{- 1}

4

\frac{4}{3} (2.8 \times 10^{- 3}) {molL}^{- 1} s^{- 1}

Explanation:

$2 A + 3 B \to 4 C + D$
$\begin{aligned} - \frac{1}{3} \frac{d (B)}{dt} = + \frac{1}{4} \frac{d (C)}{dt} \\ - \frac{d (B)}{dt} = \frac{3}{4} \frac{d (C)}{dt} \\ = \frac{3}{4} (2.8 \times 10^{- 3}) {molL}^{- 1} s^{- 1} \end{aligned}$
Rate of Law and order of reactions

KCET - 2020

CHXII04:CHEMICAL KINETICS

320575 Assertion :
For the reaction, ${PCl}_{5} \to {PCl}_{3} + {Cl}_{2}$ , the concentration of ${PCl}_{5}$ decreases with the increases in concentration of ${PCl}_{3}$ and ${Cl}_{2}$ .
Reason :
During the course of a reaction, the concentration of the reactants decreases while that of products increases.

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.

Explanation:

The reaction demonstrates the fundamental principle of chemical reactions, wherein the consumption of ${PCl}_{5}$ leads to a decrease in its concentration, while the production of ${PCl}_{3}$ and ${Cl}_{2}$ results in an increase in their concentrations. So option (1) is correct .

CHXII04:CHEMICAL KINETICS

320576 For a reaction $\frac{1}{2} A \to 2 B$ , rate of disappearance of 'A' is related to the rate of appearance of 'B' by the expression:

1

- \frac{d [A]}{d t} = \frac{1}{2} \frac{d [B]}{d t}

2

- \frac{d [A]}{d t} = \frac{1}{4} \frac{d [B]}{d t}

3

- \frac{d [A]}{d t} = \frac{d [B]}{d t}

4

- \frac{d [A]}{d t} = 4 \frac{d [B]}{d t}

Explanation:

$\frac{1}{2} A \to 2 B$
$- \frac{2 d [A]}{d t} = + \frac{d [B]}{2 d t} - \frac{d [A]}{d t} = \frac{1}{4} \frac{d [B]}{d t}$

CHXII04:CHEMICAL KINETICS

320573 Ammonia and oxygen react at high temperature as $4 {NH}_{3 (g)} + 5 O_{2 (g)} \to 4 {NO}_{(g)} + 6 H_{2} O_{(g)}$ .
If rate of formation of ${NO}_{(g)}$ is $3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}$ , then rate of disappearance of ammonia is

1

7.2 \times 10^{- 3} mol L^{- 1} s^{- 1}

2

1.2 \times 10^{- 3} mol L^{- 1} s^{- 1}

3

2.4 \times 10^{- 3} mol L^{- 1} s^{- 1}

4

3.6 \times 10^{- 3} mol L^{-  1} s^{-  1}

Explanation:

Rate of reaction $= - \frac{1}{4} \frac{d [{NH}_{3}]}{dt}$
$= - \frac{1}{5} \frac{d [O_{2}]}{dt} = \frac{1}{4} \frac{d [NO]}{dt} = \frac{1}{6} \frac{d [H_{2} O]}{dt}$
$∴$ Rate of disappearance of ${NH}_{3} =$ Rate of formation of $NO$
$= 3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}$

MHTCET - 2021

CHXII04:CHEMICAL KINETICS

320574 For an elementary reaction,
$2 A + 3 B \to 4 C + D$ the rate of appearance of
$C$ at time ' $t$ ' is $2.8 \times 10^{- 3} mol L^{- 1} s^{- 1}$ . Rate of disappearance of $B$ at time ' $t$ ' will be

1

\frac{3}{4} (2.8 \times 10^{- 3}) mol L^{- 1} s^{- 1}

2

2 (2.8 \times 10^{- 3}) mol L^{- 1} s^{- 1}

3

\frac{1}{4} (2 .8 \times 1 0^{- 3}) m o l L^{- 1} s^{- 1}

4

\frac{4}{3} (2.8 \times 10^{- 3}) {molL}^{- 1} s^{- 1}

Explanation:

$2 A + 3 B \to 4 C + D$
$\begin{aligned} - \frac{1}{3} \frac{d (B)}{dt} = + \frac{1}{4} \frac{d (C)}{dt} \\ - \frac{d (B)}{dt} = \frac{3}{4} \frac{d (C)}{dt} \\ = \frac{3}{4} (2.8 \times 10^{- 3}) {molL}^{- 1} s^{- 1} \end{aligned}$
Rate of Law and order of reactions

KCET - 2020

CHXII04:CHEMICAL KINETICS

320575 Assertion :
For the reaction, ${PCl}_{5} \to {PCl}_{3} + {Cl}_{2}$ , the concentration of ${PCl}_{5}$ decreases with the increases in concentration of ${PCl}_{3}$ and ${Cl}_{2}$ .
Reason :
During the course of a reaction, the concentration of the reactants decreases while that of products increases.

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.

Explanation:

The reaction demonstrates the fundamental principle of chemical reactions, wherein the consumption of ${PCl}_{5}$ leads to a decrease in its concentration, while the production of ${PCl}_{3}$ and ${Cl}_{2}$ results in an increase in their concentrations. So option (1) is correct .

CHXII04:CHEMICAL KINETICS

320576 For a reaction $\frac{1}{2} A \to 2 B$ , rate of disappearance of 'A' is related to the rate of appearance of 'B' by the expression:

1

- \frac{d [A]}{d t} = \frac{1}{2} \frac{d [B]}{d t}

2

- \frac{d [A]}{d t} = \frac{1}{4} \frac{d [B]}{d t}

3

- \frac{d [A]}{d t} = \frac{d [B]}{d t}

4

- \frac{d [A]}{d t} = 4 \frac{d [B]}{d t}

Explanation:

$\frac{1}{2} A \to 2 B$
$- \frac{2 d [A]}{d t} = + \frac{d [B]}{2 d t} - \frac{d [A]}{d t} = \frac{1}{4} \frac{d [B]}{d t}$