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CHEMICAL KINETICS

23419 For the reaction $N_{2} + 3 H_{2} \to 2 N H_{3}$ if $\frac{Δ [N H_{3}]}{Δ t} = 2 \times 10^{- 4} m o l l^{- 1} s^{- 1},$ the value of $\frac{- Δ [H_{2}]}{Δ t}$ would be

1

1 \times 10^{- 4} m o l l^{- 1} s^{- 1}

2

3 \times 10^{- 4} m o l l^{- 1} s^{- 1}

3

4 \times 10^{- 4} m o l l^{- 1} s^{- 1}

4

6 \times 10^{- 4} m o l l^{- 1} s^{- 1}

Explanation:

(b) $N_{2} + 3 H_{2}$ ? $2 N H_{3}$
$\frac{- Δ [N_{2}]}{Δ t} = - \frac{1}{3} \frac{Δ [H_{2}]}{Δ t} = \frac{1}{2} \frac{Δ [N H_{3}]}{Δ t}$
$∴ \frac{Δ [H_{2}]}{Δ t} = \frac{3}{2} \times \frac{Δ [N H_{3}]}{Δ t} = \frac{3}{2} \times 2 \times 10^{- 4}$
$= 3 \times 10^{- 4} m o l l i t r e^{- 1} s e c^{- 1}$

CHEMICAL KINETICS

23420 $A$ gaseous hypothetical chemical equation $2 A$ $⇌$ $4 B + C$ is carried out in a closed vessel. The concentration of $B$ is found to increase by $5 \times 10^{- 3} m o l l^{- 1}$ in $10$ second. The rate of appearance of $B$ is

1

5 \times 10^{- 4} m o l l^{- 1} s e c^{- 1}

2

5 \times 10^{- 5} m o l l^{- 1} s e c^{- 1}

3

6 \times 10^{- 5} m o l l^{- 1} \sec^{- 1}

4

4 \times 10^{- 4} m o l l^{- 1} \sec^{- 1}

Explanation:

(a) Increase in concentration of $B = 5 \times 10^{- 3} m o l l^{- 1}$ Time $= 10 \sec$
Rate of appearance of $B =$ $\frac{I n c r e a s e o f c o n c . B}{T i m e t a k e n}$
$= \frac{5 \times 10^{- 3} m o l l^{- 1}}{10 \sec} = 5 \times 10^{- 4} m o l l^{- 1} {Sec}^{- 1}$

CHEMICAL KINETICS

23421 The rate of a chemical reaction depends upon

1 Time

2 Pressure

3 Concentration

4 All of these

CHEMICAL KINETICS

23422 The rate of disappearance of $S O_{2}$ in the reaction $2 S O_{2} + O_{2} \to 2 S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ then the rate of formation of $S O_{3}$ is

1

0.64 \times 10^{- 3} g / s e c

2

0.80 \times 10^{- 3} g / s e c

3

1.28 \times 10^{- 3} g / s e c

4

1.60 \times 10^{- 3} g / s e c

Explanation:

(c)The rate of formation of $S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ .

CHEMICAL KINETICS

23423 When the concentration of A in the reaction $A + B$ $⇌$ $A B$ is doubled, the rate of reaction will be

1 Doubled

2 Decreased by half

3 Unchanged

4 Increased by four times

CHEMICAL KINETICS

23419 For the reaction $N_{2} + 3 H_{2} \to 2 N H_{3}$ if $\frac{Δ [N H_{3}]}{Δ t} = 2 \times 10^{- 4} m o l l^{- 1} s^{- 1},$ the value of $\frac{- Δ [H_{2}]}{Δ t}$ would be

1

1 \times 10^{- 4} m o l l^{- 1} s^{- 1}

2

3 \times 10^{- 4} m o l l^{- 1} s^{- 1}

3

4 \times 10^{- 4} m o l l^{- 1} s^{- 1}

4

6 \times 10^{- 4} m o l l^{- 1} s^{- 1}

Explanation:

(b) $N_{2} + 3 H_{2}$ ? $2 N H_{3}$
$\frac{- Δ [N_{2}]}{Δ t} = - \frac{1}{3} \frac{Δ [H_{2}]}{Δ t} = \frac{1}{2} \frac{Δ [N H_{3}]}{Δ t}$
$∴ \frac{Δ [H_{2}]}{Δ t} = \frac{3}{2} \times \frac{Δ [N H_{3}]}{Δ t} = \frac{3}{2} \times 2 \times 10^{- 4}$
$= 3 \times 10^{- 4} m o l l i t r e^{- 1} s e c^{- 1}$

CHEMICAL KINETICS

23420 $A$ gaseous hypothetical chemical equation $2 A$ $⇌$ $4 B + C$ is carried out in a closed vessel. The concentration of $B$ is found to increase by $5 \times 10^{- 3} m o l l^{- 1}$ in $10$ second. The rate of appearance of $B$ is

1

5 \times 10^{- 4} m o l l^{- 1} s e c^{- 1}

2

5 \times 10^{- 5} m o l l^{- 1} s e c^{- 1}

3

6 \times 10^{- 5} m o l l^{- 1} \sec^{- 1}

4

4 \times 10^{- 4} m o l l^{- 1} \sec^{- 1}

Explanation:

(a) Increase in concentration of $B = 5 \times 10^{- 3} m o l l^{- 1}$ Time $= 10 \sec$
Rate of appearance of $B =$ $\frac{I n c r e a s e o f c o n c . B}{T i m e t a k e n}$
$= \frac{5 \times 10^{- 3} m o l l^{- 1}}{10 \sec} = 5 \times 10^{- 4} m o l l^{- 1} {Sec}^{- 1}$

CHEMICAL KINETICS

23421 The rate of a chemical reaction depends upon

1 Time

2 Pressure

3 Concentration

4 All of these

CHEMICAL KINETICS

23422 The rate of disappearance of $S O_{2}$ in the reaction $2 S O_{2} + O_{2} \to 2 S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ then the rate of formation of $S O_{3}$ is

1

0.64 \times 10^{- 3} g / s e c

2

0.80 \times 10^{- 3} g / s e c

3

1.28 \times 10^{- 3} g / s e c

4

1.60 \times 10^{- 3} g / s e c

Explanation:

(c)The rate of formation of $S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ .

CHEMICAL KINETICS

23423 When the concentration of A in the reaction $A + B$ $⇌$ $A B$ is doubled, the rate of reaction will be

1 Doubled

2 Decreased by half

3 Unchanged

4 Increased by four times

CHEMICAL KINETICS

23419 For the reaction $N_{2} + 3 H_{2} \to 2 N H_{3}$ if $\frac{Δ [N H_{3}]}{Δ t} = 2 \times 10^{- 4} m o l l^{- 1} s^{- 1},$ the value of $\frac{- Δ [H_{2}]}{Δ t}$ would be

1

1 \times 10^{- 4} m o l l^{- 1} s^{- 1}

2

3 \times 10^{- 4} m o l l^{- 1} s^{- 1}

3

4 \times 10^{- 4} m o l l^{- 1} s^{- 1}

4

6 \times 10^{- 4} m o l l^{- 1} s^{- 1}

Explanation:

(b) $N_{2} + 3 H_{2}$ ? $2 N H_{3}$
$\frac{- Δ [N_{2}]}{Δ t} = - \frac{1}{3} \frac{Δ [H_{2}]}{Δ t} = \frac{1}{2} \frac{Δ [N H_{3}]}{Δ t}$
$∴ \frac{Δ [H_{2}]}{Δ t} = \frac{3}{2} \times \frac{Δ [N H_{3}]}{Δ t} = \frac{3}{2} \times 2 \times 10^{- 4}$
$= 3 \times 10^{- 4} m o l l i t r e^{- 1} s e c^{- 1}$

CHEMICAL KINETICS

23420 $A$ gaseous hypothetical chemical equation $2 A$ $⇌$ $4 B + C$ is carried out in a closed vessel. The concentration of $B$ is found to increase by $5 \times 10^{- 3} m o l l^{- 1}$ in $10$ second. The rate of appearance of $B$ is

1

5 \times 10^{- 4} m o l l^{- 1} s e c^{- 1}

2

5 \times 10^{- 5} m o l l^{- 1} s e c^{- 1}

3

6 \times 10^{- 5} m o l l^{- 1} \sec^{- 1}

4

4 \times 10^{- 4} m o l l^{- 1} \sec^{- 1}

Explanation:

(a) Increase in concentration of $B = 5 \times 10^{- 3} m o l l^{- 1}$ Time $= 10 \sec$
Rate of appearance of $B =$ $\frac{I n c r e a s e o f c o n c . B}{T i m e t a k e n}$
$= \frac{5 \times 10^{- 3} m o l l^{- 1}}{10 \sec} = 5 \times 10^{- 4} m o l l^{- 1} {Sec}^{- 1}$

CHEMICAL KINETICS

23421 The rate of a chemical reaction depends upon

1 Time

2 Pressure

3 Concentration

4 All of these

CHEMICAL KINETICS

23422 The rate of disappearance of $S O_{2}$ in the reaction $2 S O_{2} + O_{2} \to 2 S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ then the rate of formation of $S O_{3}$ is

1

0.64 \times 10^{- 3} g / s e c

2

0.80 \times 10^{- 3} g / s e c

3

1.28 \times 10^{- 3} g / s e c

4

1.60 \times 10^{- 3} g / s e c

Explanation:

(c)The rate of formation of $S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ .

CHEMICAL KINETICS

23423 When the concentration of A in the reaction $A + B$ $⇌$ $A B$ is doubled, the rate of reaction will be

1 Doubled

2 Decreased by half

3 Unchanged

4 Increased by four times

CHEMICAL KINETICS

23419 For the reaction $N_{2} + 3 H_{2} \to 2 N H_{3}$ if $\frac{Δ [N H_{3}]}{Δ t} = 2 \times 10^{- 4} m o l l^{- 1} s^{- 1},$ the value of $\frac{- Δ [H_{2}]}{Δ t}$ would be

1

1 \times 10^{- 4} m o l l^{- 1} s^{- 1}

2

3 \times 10^{- 4} m o l l^{- 1} s^{- 1}

3

4 \times 10^{- 4} m o l l^{- 1} s^{- 1}

4

6 \times 10^{- 4} m o l l^{- 1} s^{- 1}

Explanation:

(b) $N_{2} + 3 H_{2}$ ? $2 N H_{3}$
$\frac{- Δ [N_{2}]}{Δ t} = - \frac{1}{3} \frac{Δ [H_{2}]}{Δ t} = \frac{1}{2} \frac{Δ [N H_{3}]}{Δ t}$
$∴ \frac{Δ [H_{2}]}{Δ t} = \frac{3}{2} \times \frac{Δ [N H_{3}]}{Δ t} = \frac{3}{2} \times 2 \times 10^{- 4}$
$= 3 \times 10^{- 4} m o l l i t r e^{- 1} s e c^{- 1}$

CHEMICAL KINETICS

23420 $A$ gaseous hypothetical chemical equation $2 A$ $⇌$ $4 B + C$ is carried out in a closed vessel. The concentration of $B$ is found to increase by $5 \times 10^{- 3} m o l l^{- 1}$ in $10$ second. The rate of appearance of $B$ is

1

5 \times 10^{- 4} m o l l^{- 1} s e c^{- 1}

2

5 \times 10^{- 5} m o l l^{- 1} s e c^{- 1}

3

6 \times 10^{- 5} m o l l^{- 1} \sec^{- 1}

4

4 \times 10^{- 4} m o l l^{- 1} \sec^{- 1}

Explanation:

(a) Increase in concentration of $B = 5 \times 10^{- 3} m o l l^{- 1}$ Time $= 10 \sec$
Rate of appearance of $B =$ $\frac{I n c r e a s e o f c o n c . B}{T i m e t a k e n}$
$= \frac{5 \times 10^{- 3} m o l l^{- 1}}{10 \sec} = 5 \times 10^{- 4} m o l l^{- 1} {Sec}^{- 1}$

CHEMICAL KINETICS

23421 The rate of a chemical reaction depends upon

1 Time

2 Pressure

3 Concentration

4 All of these

CHEMICAL KINETICS

23422 The rate of disappearance of $S O_{2}$ in the reaction $2 S O_{2} + O_{2} \to 2 S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ then the rate of formation of $S O_{3}$ is

1

0.64 \times 10^{- 3} g / s e c

2

0.80 \times 10^{- 3} g / s e c

3

1.28 \times 10^{- 3} g / s e c

4

1.60 \times 10^{- 3} g / s e c

Explanation:

(c)The rate of formation of $S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ .

CHEMICAL KINETICS

23423 When the concentration of A in the reaction $A + B$ $⇌$ $A B$ is doubled, the rate of reaction will be

1 Doubled

2 Decreased by half

3 Unchanged

4 Increased by four times

CHEMICAL KINETICS

23419 For the reaction $N_{2} + 3 H_{2} \to 2 N H_{3}$ if $\frac{Δ [N H_{3}]}{Δ t} = 2 \times 10^{- 4} m o l l^{- 1} s^{- 1},$ the value of $\frac{- Δ [H_{2}]}{Δ t}$ would be

1

1 \times 10^{- 4} m o l l^{- 1} s^{- 1}

2

3 \times 10^{- 4} m o l l^{- 1} s^{- 1}

3

4 \times 10^{- 4} m o l l^{- 1} s^{- 1}

4

6 \times 10^{- 4} m o l l^{- 1} s^{- 1}

Explanation:

(b) $N_{2} + 3 H_{2}$ ? $2 N H_{3}$
$\frac{- Δ [N_{2}]}{Δ t} = - \frac{1}{3} \frac{Δ [H_{2}]}{Δ t} = \frac{1}{2} \frac{Δ [N H_{3}]}{Δ t}$
$∴ \frac{Δ [H_{2}]}{Δ t} = \frac{3}{2} \times \frac{Δ [N H_{3}]}{Δ t} = \frac{3}{2} \times 2 \times 10^{- 4}$
$= 3 \times 10^{- 4} m o l l i t r e^{- 1} s e c^{- 1}$

CHEMICAL KINETICS

23420 $A$ gaseous hypothetical chemical equation $2 A$ $⇌$ $4 B + C$ is carried out in a closed vessel. The concentration of $B$ is found to increase by $5 \times 10^{- 3} m o l l^{- 1}$ in $10$ second. The rate of appearance of $B$ is

1

5 \times 10^{- 4} m o l l^{- 1} s e c^{- 1}

2

5 \times 10^{- 5} m o l l^{- 1} s e c^{- 1}

3

6 \times 10^{- 5} m o l l^{- 1} \sec^{- 1}

4

4 \times 10^{- 4} m o l l^{- 1} \sec^{- 1}

Explanation:

(a) Increase in concentration of $B = 5 \times 10^{- 3} m o l l^{- 1}$ Time $= 10 \sec$
Rate of appearance of $B =$ $\frac{I n c r e a s e o f c o n c . B}{T i m e t a k e n}$
$= \frac{5 \times 10^{- 3} m o l l^{- 1}}{10 \sec} = 5 \times 10^{- 4} m o l l^{- 1} {Sec}^{- 1}$

CHEMICAL KINETICS

23421 The rate of a chemical reaction depends upon

1 Time

2 Pressure

3 Concentration

4 All of these

CHEMICAL KINETICS

23422 The rate of disappearance of $S O_{2}$ in the reaction $2 S O_{2} + O_{2} \to 2 S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ then the rate of formation of $S O_{3}$ is

1

0.64 \times 10^{- 3} g / s e c

2

0.80 \times 10^{- 3} g / s e c

3

1.28 \times 10^{- 3} g / s e c

4

1.60 \times 10^{- 3} g / s e c

Explanation:

(c)The rate of formation of $S O_{3}$ is $1.28 \times 10^{- 3} g / s e c$ .

CHEMICAL KINETICS

23423 When the concentration of A in the reaction $A + B$ $⇌$ $A B$ is doubled, the rate of reaction will be

1 Doubled

2 Decreased by half

3 Unchanged

4 Increased by four times