The decomposition of N2O5 occurs as - 2N2O5- 4NO2 -O2 - and follows first order kinetics hence

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Standard XII

Chemistry

Molecularity of Reaction

The decomposi...

Question

The decomposition of $N_{2} O_{5}$ occurs as ,
$2 N_{2} O_{5} \to 4 N O_{2} + O_{2},$ and follows first order kinetics hence

The reaction is biomolecular

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The reaction is unimolecular

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t_{1 / 2} α a^{0}

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None of these

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Solution

The correct option is B The reaction is biomolecular
$2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}$
The reaction follows first order kinetics and the reaction is bimolecular because it involves $2$ molecules of $N_{2} O_{3}$ in the reaction.

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Similar questions

Q. The decomposition of

N_{2} O_{5}

occurs as,

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

and follows first order KInetic ; hence:

Q. The thermal decomposition of

N_{2} O_{5}

occurs in the following steps:
Step I

N_{2} O_{5} s l o w - - \to N O_{2} + N O_{3}

Step II

N_{2} O_{5} + N O_{2} f a s t - - \to 3 N O_{2} + O_{2}

Overall reaction

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

Suggest the rate expression.

Q. The decomposition of

N_{2} O_{5}

takes place according to I order as

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

Calculate:
(a) The rate constant, if instantaneous rate is

1.4 \times 10^{- 6} m o l l i t r e^{- 1} {sec}^{- 1}

when concentration of

N_{2} O_{5}

0.04 M

.
(b) The rate of reaction when concentration of

N_{2} O_{5}

1.20 M

.
(c) The concentration of

N_{2} O_{5}

when the rate of reaction will be

2.45 \times 10^{- 5} m o l l i t r e^{- 1} {sec}^{- 1}

Q. The decomposition of

N_{2} O_{5}

C C l_{4}

solution at 320 K takes place as

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

; On the basis of given data order and the rate constant of the reaction is :

Time in minutes	10	15	20	25	$\infty$
The volume of $O_{2}$ evolved (in mL)	6.30	8.95	11.40	13.50	34.75

Q. For the reaction

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

, if the initial concentration of

N_{2} O_{5}

7.2 m o l L^{- 1}

and after

20

minutes,

[N O_{2}]

becomes

2.4 m o l L^{- 1}

, then what will be rate of decomposition of

N_{2} O_{5}

m o l L^{- 1} m i n^{- 1}

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The decomposition of N2O5 occurs as , 2N2O5→4NO2+O2, and follows first order kinetics hence

The correct option is B The reaction is biomolecular2N2O5⟶4NO2+O2The reaction follows first order kinetics and the reaction is bimolecular because it involves 2 molecules of N2O3 in the reaction.

The decomposition of $N_{2} O_{5}$ occurs as ,
$2 N_{2} O_{5} \to 4 N O_{2} + O_{2},$ and follows first order kinetics hence

The correct option is B The reaction is biomolecular
$2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}$
The reaction follows first order kinetics and the reaction is bimolecular because it involves $2$ molecules of $N_{2} O_{3}$ in the reaction.