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For the decomposition of N(2)O(5) it is...

For the decomposition of `N_(2)O_(5)` it is given that:
`2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g)`, activation energy `E_(a)`
`N_(2)O_(5) (g) to 2NO_(2)(g) + 1/2 O_(2)(g)` activation energy `E_(a)^(')`
then,

A

`E_(a)=E_(a)^(')`

B

`E_(a)gtE_(a)^(')`

C

`E_(a)ltE_(a)^(')`

D

`E_(a)=2E_(a)^(')`

Text Solution

Verified by Experts

The correct Answer is:
A
Activation energy does not depend on the way a reaction is formulated in the chemical equation
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For the first-order decomposition reaction of N_(2)O_(5) written as: 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) , rate =k[N_(2)O_(5)] N_(2)O_(5)(g) to 2NO_(2)(g) + 1/2O_(2)(g) , rate =k'[N_(2)O_(5)] which of the following facts is true?

The molecularity of a complex reaction given below is: 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g)

In the process 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) at t = 10, rate of reaction w.r.t. N_(2)O_(5), NO_(2) & O_(2) respectively are:

The decomposition of N_(2)O_(5) according to the equation, 2N_(2)O_(5) (g) rarr 4NO_(2) (g) + O_(2) (g) is a first order reaction, After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 mm Hg and on completion, the total pressure is 584.5 mm Hg. Calculate the rate constant of the reaction.

For the reaction 2NO_(2)(g) iff 2NO(g)+O_(2)(g), K_(c)=4 times 10^(-6) at 500 K. Hence, the K_(c) of the reaction NO(g)+1/2O_(2)(g) iff NO_(2)(g) at 500 K is

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