The decomposition of H2O2 is represented as- H2O2- H2O-Oslow O-O- O2fast- The order of the reaction is-

The correct option is A 1 The slowest step of a #160;chemical reaction is the rate determining step of the reaction. #160;Thus, the 1st step involving ...

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Standard XII

Chemistry

Characteristics of Equilibrium Constant

The decomposi...

Question

The decomposition of $H_{2} O_{2}$ is represented as:

$H_{2} O_{2} \to H_{2} O + O (s l o w)$
$(O) + (O) \to O_{2} (f a s t)$ .

The order of the reaction is:

1

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Solution

The correct option is A $1$
The slowest step of a chemical reaction is the rate-determining step of the reaction.

Thus, the 1st step involving the decomposition of $H_{2} O_{2}$ is the rate-determining step.

$R a t e = k [H_{2} O_{2}]$

Thus, the order of the reaction is 1.

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Similar questions

Q. In the reaction,

A g_{2} O + H_{2} O_{2} \to 2 A g + H_{2} O + O_{2}

, the

H_{2} O_{2}

acts as:

Q. A decomposition reaction has following mechanism:

2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}

(overal)

N_{2} O_{5} ⇌ N O_{2} + N O_{3}

(fast decomposition)

N O_{2} + N O_{3} ⟶ N O + N O_{2} + O_{2}

(slow)

N O + N O_{3} ⟶ 2 N O_{2}

(fast)
Determine rate law and show the mechanism corresponds to first order reaction.

Consider the following equation of the chemical reaction of a metal M :

$4 M + 3 O_{2}$ $⟶$ $2 M_{2} O_{3}$

This equation represents :

(a) combination reaction as well as reduction reaction

(b) decomposition reaction as well as oxidation reaction

(d) combination reaction as well as oxidation reaction

A + H_{2} O_{2} \to B + O_{2} .

In this reaction, the role of

H_{2} O_{2}

is:

Q. At

380^{o} C

, the half life period for the first order decomposition of

H_{2} O_{2}

360

m i n

. The energy of activation of the reaction is

200

k J

{m o l}^{- 1}

. Calculate the time required for

75

% decomposition at

450^{o} C

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The decomposition of H2O2 is represented as: H2O2→H2O+O(slow) (O)+(O)→O2(fast). The order of the reaction is:

The correct option is A 1The slowest step of a chemical reaction is the rate-determining step of the reaction. Thus, the 1st step involving the decomposition of H2O2 is the rate-determining step.Rate=k[H2O2]Thus, the order of the reaction is 1.

The decomposition of $H_{2} O_{2}$ is represented as:

$H_{2} O_{2} \to H_{2} O + O (s l o w)$
$(O) + (O) \to O_{2} (f a s t)$ .

The order of the reaction is:

The correct option is A $1$
The slowest step of a chemical reaction is the rate-determining step of the reaction.

Thus, the 1st step involving the decomposition of $H_{2} O_{2}$ is the rate-determining step.

$R a t e = k [H_{2} O_{2}]$

Thus, the order of the reaction is 1.