The rate of the reaction 2N2O3-4NO2 - O2 can be written in three ways-

2 N _ 2 O _ 3 → 4 NO _ 2 + O _ 2 Rate= 1 / 2 d[ N _ 2 O _ 3 ] #160; / dt Rate= 1 / 4 d[ NO _ 2 ] #160; / dt Rate= 1 / 1 d( O _ ...

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Standard XII

Chemistry

Ionic Bond

The rate of t...

Question

The rate of the reaction $2 N_{2} O_{3} \to 4N O_{2} + O_{2}$ can be written in three ways.

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Solution

$2 N_{2} O_{3} \to 4 {N O}_{2} + O_{2}$

Rate= $- \frac{1}{2} d \frac{[N_{2} O_{3}]}{d t}$

Rate= $\frac{1}{4} d \frac{[{N O}_{2}]}{d t}$

Rate= $\frac{1}{1} d \frac{(O_{2})}{d t}$
These are the three ways of writing the rate of reaction for this reaction.

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Q. The rate of the reaction

2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}

can be written in three ways:

\frac{- d [N_{2} O_{5}]}{d t} = k [N_{2} O_{5}]

\frac{d [N O_{2}]}{d t} = k^{'} [N_{2} O_{5}]

\frac{d [O_{2}]}{d t} = k^{''} [N_{2} O_{5}]

The relationship between

k

and

k^{'}

and between

k

and

k^{''}

are :

Q. The rate of the reaction

2 N_{2} O_{5} \to 4 N O_{2} + O_{2}

can be written in three ways:

\frac{- d [N_{2} O_{5}]}{d t} = k [N_{2} O_{5}]

\frac{d [N O_{2}]}{d t} = k^{'} [N_{2} O_{5}]

\frac{d [O_{2}]}{d t} = k^{''} [N_{2} O_{5}]

The relationship between

k

and

k^{'}

are:

The chemical reaction $2 O_{3} \to 3 O_{2}$ involves two elementary steps :
$O_{3} f a s t - - \to O_{2} + O; O + O_{3} S l o w - -- \to 2 O_{2}$
The differential rate law expression will be :

The reaction ; $2 O_{3}$ → $3 O_{2}$ , is assigned the following mechanism.

(I) $O_{3} ⇋ O_{2} + O (i i) O_{3} + O s l o w ⇌ 2 O_{2}$

The rate law of the reaction will therefore be

Q. The chemical reaction,

2 O_{3} \to 3 O_{2}

proceeds as follows:

O_{3} ⇌ O_{2} + O

....(fast)

O + O_{3} \to 2 O_{2}

....(slow)

The rate law expression should be:

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The rate of the reaction 2N2O3→4NO2 + O2 can be written in three ways.

2N2O3→4NO2+O2Rate= −12d[N2O3]dtRate= 14d[NO2]dtRate= 11d(O2)dtThese are the three ways of writing the rate of reaction for this reaction.

The rate of the reaction $2 N_{2} O_{3} \to 4N O_{2} + O_{2}$ can be written in three ways.

$2 N_{2} O_{3} \to 4 {N O}_{2} + O_{2}$

Rate= $- \frac{1}{2} d \frac{[N_{2} O_{3}]}{d t}$

Rate= $\frac{1}{4} d \frac{[{N O}_{2}]}{d t}$

Rate= $\frac{1}{1} d \frac{(O_{2})}{d t}$
These are the three ways of writing the rate of reaction for this reaction.