The mechanism of the reaction- 2NO g -2 H 2 g - N 2 g -2 H 2 O g - is-Step 1- 2NO g - H 2 g N 2 - H 2 O 2Step 2- H 2 O 2 - H 2 2 H 2 OWhich ofthe following statements is-are correct-

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Byju's Answer

Standard XII

Chemistry

Order of Reaction

The mechanism...

Question

The mechanism of the reaction, $2 N O (g) + 2 H_{2} (g) ⟶ N_{2} (g) + 2 H_{2} O (g)$ , is:
Step 1: $2 N O (g) + H_{2} (g) s l o w - ----- \to N_{2} + H_{2} O_{2}$
Step 2: $H_{2} O_{2} + H_{2} f a s t - ----- \to 2 H_{2} O$
Which ofthe following statement(s) is/are correct?

Rate

= k {[N O]}^{2} {[H_{2}]}^{2}

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Rate

= k [H_{2} O_{2}] [H_{2}]

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On doubling the concentration of

H_{2}

, keeping the concentration of

N O

constant, the rate will become double

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If the initial concentration of

H_{2}

and

N O

C_{0}

and after time '

t

' the concentration of

N_{2}

x

, then Rate

= k {(C_{0} - 2 x)}^{x}

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Solution

The correct option is C On doubling the concentration of $H_{2}$ , keeping the concentration of $N O$ constant, the rate will become double
Slowest step is rate determining,
$∴$ Rate $= k {[N O]}^{2} [H_{2}]$
$∴$ On doubling the concentration of $H_{2}$ without changing the concentration of $N O$ , the rate will become double.

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Similar questions

Q. Assertion :In the reaction,

N O_{2} (g) + C O (g) ⟶ C O_{2} (g) + N O (g)

, rate

= k {[N O_{2}]}^{2}

.
The rate of reaction does not depend on the concentration of

C O

. Reason: Carbon monoxide is involved in fast step.

Q. In the Haber's process of ammonia manufacture,

N_{2} (g) + 3 H_{2} (g) ⟶ 2 N H_{3} (g)

, the rate of appearance of

N H_{3}

is:

\frac{d [N H_{3}]}{d t} = 2 \times 10^{- 4}

m o l

L^{- 1} {s e c}^{- 1}

The rates of the reaction expressed in terms of

N_{2}

and

H_{2}

will be:

Rates in terms of

H_{2}

(m o l L^{- 1} {s e c}^{- 1})

Rates in terms of

N_{2}

(m o l L^{- 1} {s e c}^{- 1})

Q. The rate constant for the reaction,

N_{2} O_{5} (g) ⟶ 2 N O_{2} (g) + \frac{1}{2} O_{2} (g)

, is

2.3 \times 10^{- 2} {s e c}^{- 1}

. Which equation given below describes the change of

[N_{2} O_{5}]

with time,

{[N_{2} O_{5}]}_{0}

and

{[N_{2} O_{5}]}_{t}

corresponds to concentration of

N_{2} O_{5}

initially and time

t

respectively?

Q. Predict which of the following reaction will have appreciable concentration of reactants and products:
a)

{C l}_{2} (g) ⇌ 2 C l (g); K_{c} = 5 \times 10^{- 39}

{C l}_{2} (g) + 2 N O (g) ⇌ 2 N O C l (g); K_{c} = 3.7 \times 10^{8}

{C l}_{2} (g) + 2 {N O}_{2} (g) ⇌ 2 {N O}_{2} C l (g); K_{c} = 1.8

Q. Ozone depletion takes place as,

2 O_{3} (g) ⟶ 3 O_{2} (g)

:
Step 1:

O_{3} (g) k ⇌ O_{2} (g) + [O] (g)

(fast)
Step 2:

O_{3} (g) + [O] k^{'} - -------- \to 2 O_{2} (g)

(slow)
The order of the overall reaction is:

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The mechanism of the reaction, 2NO(g)+2H2(g)⟶N2(g)+2H2O(g), is:Step 1: 2NO(g)+H2(g)slow−−−−−−→N2+H2O2Step 2: H2O2+H2fast−−−−−−→2H2OWhich ofthe following statement(s) is/are correct?

The correct option is C On doubling the concentration of H2, keeping the concentration of NO constant, the rate will become doubleSlowest step is rate determining,∴ Rate =k[NO]2[H2]∴ On doubling the concentration of H2 without changing the concentration of NO, the rate will become double.

The mechanism of the reaction, $2 N O (g) + 2 H_{2} (g) ⟶ N_{2} (g) + 2 H_{2} O (g)$ , is:
Step 1: $2 N O (g) + H_{2} (g) s l o w - ----- \to N_{2} + H_{2} O_{2}$
Step 2: $H_{2} O_{2} + H_{2} f a s t - ----- \to 2 H_{2} O$
Which ofthe following statement(s) is/are correct?