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CHXII04:CHEMICAL KINETICS

320577 Average rate of reaction for the following reaction.
$2 {SO}_{2} (g) + O_{2} (g) ⟶ 2 {SO}_{3} (g)$ is written as

1

\frac{Δ [S O_{2}]}{Δ t}

2

- \frac{Δ [O_{2}]}{Δ t}

3

\frac{1}{2} \frac{Δ [{SO}_{2}]}{Δ t}

4

\frac{Δ [{SO}_{3}]}{Δ t}

Explanation:

Average rate of reaction is defined as the speed with which the reactants are converted into products.
For reaction, $2 {SO}_{2} (g) + O_{2} (g) ⟶ 2 {SO}_{3} (g)$
$- \frac{1}{2} \frac{Δ [{SO}_{2}]}{Δ t} = \frac{- Δ [O_{2}]}{Δ t} = + \frac{1}{2} \frac{Δ [{SO}_{3}]}{Δ t}$
So, average rate of reaction is written as
$\frac{- Δ [O_{2}]}{Δ t}$

MHTCET - 2016

CHXII04:CHEMICAL KINETICS

320578 The graph plotted between concentration versus time
supporting img

1 It gives rate of disappearance of reactant

2 Rate

=  - \frac{d [C_{2} - C_{1}]}{t_{2} - t_{1}}

3 Both (1) and (2)

4 It predicts the order of reaction

CHXII04:CHEMICAL KINETICS

320579 In an experiment to study the reaction $A + 2B \to C + 2D$ , the initial rate $\frac{- d[A]}{dt}$ at $t =$ 0 was found to be $2 .6 \times 1 0^{- 2} M s^{- 1}$ . What is the value of $\frac{- d[B]}{dt} at t = 0 in M s^{- 1}$ ?

1

2.6 \times 10^{- 2}

2

5.2 \times 10^{- 2}

3

1.3 \times 10^{- 2}

4

1.0 \times 10^{- 1}

Explanation:

$\frac{- d [B]}{d t} = 2 [\frac{- d [A]}{d t}]$
$= 2 \times 2 .6 \times 1 0^{- 2}$
$= 5 .2 \times 1 0^{- 2} M s^{- 1}$

CHXII04:CHEMICAL KINETICS

320580 For the reaction $N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$ under certain conditions of temperature and partial pressure of the reactants, the rate of formation of $N H_{3} is 0 .001 mole h r^{- 1}$ . The rate of conversion of $H_{2}$ under the same conditions is

1

1 .82 \times 1 0^{- 4} m o l e h r

2

0 .0015 m o l e h r

3

1 .52 \times 1 0^{4} m o l e h r

4

1 .82 \times 1 0^{- 14} m o l e h r

Explanation:

$\frac{- d [N_{2}]}{d t} = \frac{- d [H_{2}]}{3 d t} = \frac{1}{2} \frac{d [N H_{3}]}{d t}$
$\frac{d [H_{2}]}{d t} = \frac{3}{2} \times 0 .001 = 0 .0015 m o l h r^{- 1}$

CHXII04:CHEMICAL KINETICS

320577 Average rate of reaction for the following reaction.
$2 {SO}_{2} (g) + O_{2} (g) ⟶ 2 {SO}_{3} (g)$ is written as

1

\frac{Δ [S O_{2}]}{Δ t}

2

- \frac{Δ [O_{2}]}{Δ t}

3

\frac{1}{2} \frac{Δ [{SO}_{2}]}{Δ t}

4

\frac{Δ [{SO}_{3}]}{Δ t}

Explanation:

Average rate of reaction is defined as the speed with which the reactants are converted into products.
For reaction, $2 {SO}_{2} (g) + O_{2} (g) ⟶ 2 {SO}_{3} (g)$
$- \frac{1}{2} \frac{Δ [{SO}_{2}]}{Δ t} = \frac{- Δ [O_{2}]}{Δ t} = + \frac{1}{2} \frac{Δ [{SO}_{3}]}{Δ t}$
So, average rate of reaction is written as
$\frac{- Δ [O_{2}]}{Δ t}$

MHTCET - 2016

CHXII04:CHEMICAL KINETICS

320578 The graph plotted between concentration versus time
supporting img

1 It gives rate of disappearance of reactant

2 Rate

=  - \frac{d [C_{2} - C_{1}]}{t_{2} - t_{1}}

3 Both (1) and (2)

4 It predicts the order of reaction

CHXII04:CHEMICAL KINETICS

320579 In an experiment to study the reaction $A + 2B \to C + 2D$ , the initial rate $\frac{- d[A]}{dt}$ at $t =$ 0 was found to be $2 .6 \times 1 0^{- 2} M s^{- 1}$ . What is the value of $\frac{- d[B]}{dt} at t = 0 in M s^{- 1}$ ?

1

2.6 \times 10^{- 2}

2

5.2 \times 10^{- 2}

3

1.3 \times 10^{- 2}

4

1.0 \times 10^{- 1}

Explanation:

$\frac{- d [B]}{d t} = 2 [\frac{- d [A]}{d t}]$
$= 2 \times 2 .6 \times 1 0^{- 2}$
$= 5 .2 \times 1 0^{- 2} M s^{- 1}$

CHXII04:CHEMICAL KINETICS

320580 For the reaction $N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$ under certain conditions of temperature and partial pressure of the reactants, the rate of formation of $N H_{3} is 0 .001 mole h r^{- 1}$ . The rate of conversion of $H_{2}$ under the same conditions is

1

1 .82 \times 1 0^{- 4} m o l e h r

2

0 .0015 m o l e h r

3

1 .52 \times 1 0^{4} m o l e h r

4

1 .82 \times 1 0^{- 14} m o l e h r

Explanation:

$\frac{- d [N_{2}]}{d t} = \frac{- d [H_{2}]}{3 d t} = \frac{1}{2} \frac{d [N H_{3}]}{d t}$
$\frac{d [H_{2}]}{d t} = \frac{3}{2} \times 0 .001 = 0 .0015 m o l h r^{- 1}$

CHXII04:CHEMICAL KINETICS

320577 Average rate of reaction for the following reaction.
$2 {SO}_{2} (g) + O_{2} (g) ⟶ 2 {SO}_{3} (g)$ is written as

1

\frac{Δ [S O_{2}]}{Δ t}

2

- \frac{Δ [O_{2}]}{Δ t}

3

\frac{1}{2} \frac{Δ [{SO}_{2}]}{Δ t}

4

\frac{Δ [{SO}_{3}]}{Δ t}

Explanation:

Average rate of reaction is defined as the speed with which the reactants are converted into products.
For reaction, $2 {SO}_{2} (g) + O_{2} (g) ⟶ 2 {SO}_{3} (g)$
$- \frac{1}{2} \frac{Δ [{SO}_{2}]}{Δ t} = \frac{- Δ [O_{2}]}{Δ t} = + \frac{1}{2} \frac{Δ [{SO}_{3}]}{Δ t}$
So, average rate of reaction is written as
$\frac{- Δ [O_{2}]}{Δ t}$

MHTCET - 2016

CHXII04:CHEMICAL KINETICS

320578 The graph plotted between concentration versus time
supporting img

1 It gives rate of disappearance of reactant

2 Rate

=  - \frac{d [C_{2} - C_{1}]}{t_{2} - t_{1}}

3 Both (1) and (2)

4 It predicts the order of reaction

CHXII04:CHEMICAL KINETICS

320579 In an experiment to study the reaction $A + 2B \to C + 2D$ , the initial rate $\frac{- d[A]}{dt}$ at $t =$ 0 was found to be $2 .6 \times 1 0^{- 2} M s^{- 1}$ . What is the value of $\frac{- d[B]}{dt} at t = 0 in M s^{- 1}$ ?

1

2.6 \times 10^{- 2}

2

5.2 \times 10^{- 2}

3

1.3 \times 10^{- 2}

4

1.0 \times 10^{- 1}

Explanation:

$\frac{- d [B]}{d t} = 2 [\frac{- d [A]}{d t}]$
$= 2 \times 2 .6 \times 1 0^{- 2}$
$= 5 .2 \times 1 0^{- 2} M s^{- 1}$

CHXII04:CHEMICAL KINETICS

320580 For the reaction $N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$ under certain conditions of temperature and partial pressure of the reactants, the rate of formation of $N H_{3} is 0 .001 mole h r^{- 1}$ . The rate of conversion of $H_{2}$ under the same conditions is

1

1 .82 \times 1 0^{- 4} m o l e h r

2

0 .0015 m o l e h r

3

1 .52 \times 1 0^{4} m o l e h r

4

1 .82 \times 1 0^{- 14} m o l e h r

Explanation:

$\frac{- d [N_{2}]}{d t} = \frac{- d [H_{2}]}{3 d t} = \frac{1}{2} \frac{d [N H_{3}]}{d t}$
$\frac{d [H_{2}]}{d t} = \frac{3}{2} \times 0 .001 = 0 .0015 m o l h r^{- 1}$

CHXII04:CHEMICAL KINETICS

320577 Average rate of reaction for the following reaction.
$2 {SO}_{2} (g) + O_{2} (g) ⟶ 2 {SO}_{3} (g)$ is written as

1

\frac{Δ [S O_{2}]}{Δ t}

2

- \frac{Δ [O_{2}]}{Δ t}

3

\frac{1}{2} \frac{Δ [{SO}_{2}]}{Δ t}

4

\frac{Δ [{SO}_{3}]}{Δ t}

Explanation:

Average rate of reaction is defined as the speed with which the reactants are converted into products.
For reaction, $2 {SO}_{2} (g) + O_{2} (g) ⟶ 2 {SO}_{3} (g)$
$- \frac{1}{2} \frac{Δ [{SO}_{2}]}{Δ t} = \frac{- Δ [O_{2}]}{Δ t} = + \frac{1}{2} \frac{Δ [{SO}_{3}]}{Δ t}$
So, average rate of reaction is written as
$\frac{- Δ [O_{2}]}{Δ t}$

MHTCET - 2016

CHXII04:CHEMICAL KINETICS

320578 The graph plotted between concentration versus time
supporting img

1 It gives rate of disappearance of reactant

2 Rate

=  - \frac{d [C_{2} - C_{1}]}{t_{2} - t_{1}}

3 Both (1) and (2)

4 It predicts the order of reaction

CHXII04:CHEMICAL KINETICS

320579 In an experiment to study the reaction $A + 2B \to C + 2D$ , the initial rate $\frac{- d[A]}{dt}$ at $t =$ 0 was found to be $2 .6 \times 1 0^{- 2} M s^{- 1}$ . What is the value of $\frac{- d[B]}{dt} at t = 0 in M s^{- 1}$ ?

1

2.6 \times 10^{- 2}

2

5.2 \times 10^{- 2}

3

1.3 \times 10^{- 2}

4

1.0 \times 10^{- 1}

Explanation:

$\frac{- d [B]}{d t} = 2 [\frac{- d [A]}{d t}]$
$= 2 \times 2 .6 \times 1 0^{- 2}$
$= 5 .2 \times 1 0^{- 2} M s^{- 1}$

CHXII04:CHEMICAL KINETICS

320580 For the reaction $N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$ under certain conditions of temperature and partial pressure of the reactants, the rate of formation of $N H_{3} is 0 .001 mole h r^{- 1}$ . The rate of conversion of $H_{2}$ under the same conditions is

1

1 .82 \times 1 0^{- 4} m o l e h r

2

0 .0015 m o l e h r

3

1 .52 \times 1 0^{4} m o l e h r

4

1 .82 \times 1 0^{- 14} m o l e h r

Explanation:

$\frac{- d [N_{2}]}{d t} = \frac{- d [H_{2}]}{3 d t} = \frac{1}{2} \frac{d [N H_{3}]}{d t}$
$\frac{d [H_{2}]}{d t} = \frac{3}{2} \times 0 .001 = 0 .0015 m o l h r^{- 1}$

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