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The rate constant k, for the reaction N(...

The rate constant `k`, for the reaction `N_(2)O_(5)(g) rarr 2NO_(2) (g) + (1)/(2) O_(2)(g)` is `2.3 xx 10^(-2) s^(-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)` correspond to concentration of `N_(2)O_(5)` initially and at time, `t` ?

A

`[N_(2)O_(5)]_(t) =[N_(2)O_(5)]_(o) + kt`

B

`[N_(2)O_(5)]_(o) =[N_(2)O_(5)]_(t) e^(-kt)`

C

`log [N_(2)O_(5)]_(t) =log [N_(2)O_(5)]_(o) +kt`

D

`In ([N_(2)O_(5)]_(o))/([N_(2)O_(5)]_(t))=kt`

Text Solution

Verified by Experts

The correct Answer is:
D
The rate constant is `2.3xx10^(-2) s^(-1)` which implies first order kinetics since `r=(-d[N_(2)O_(5)])/(dt)` Integrating it will provide In `([N_(2)O_(5)]_(0))/([N_(2)O_(5)]_(0)=kt`
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