The rate constant, k of the reaction,
`N_2O_(2(g))rarr2NO_(2(g))+1/2O_(2(g))` is `2.3xx10^(-2)s^(-1)`
Which equation given below describes the change of `[N_2O_5]` with time? `[N_2O_5]_0` and `[N_2O_5]`, correspond to concentration of `N_2O_5` initially and at time t.

Options

A. `[N_2O_5]_t=[N_2O_5]_0+kt`
B. `log[N_2O_5]_t=log[N_2O_5]_0-kt`
C. `[N_2O_5]_0=[N_2O_5]_te^(kt)`
D. In `([N_2O_5]_0)/(N_2O_5]_t)=kt`

Answer

D

Explanation

`k=1/t""In([N_2O_5]_0)/([N_2O_5]_t)implies" kt "In ([N_2O_5]_0)/([N_2O_5]_t)`