The initial concentration of `N_(2)O_(5)` in the following first order reaction:
`N_(2)O_(5)(g) rarr 2NO_(2)(g)+(1)/(2)O_(2)(g)`
was `1.24 xx 10^(-2) mol L^(-1)` at `318 K`. The concentration of `N_(2)O_(5)` after `60 min` was `0.20 xx 10^(-2) mol L^(-1)`. Calculate the rate constant of the reaction at `318 K`.

Options

A. `0.0304" ""min"^(-1)`
B. `0.0204" ""min"^(-1)`
C. `0.0034" ""min"^(-1)`
D. `1.0304" ""min"^(-1)`

Explanation

For a first order reaction ,
`"log" ([A])/([A])=(kt)/2.303`
`k=(2.303)/(t)"log"([A]_(0))/([A])`
`=(2.303)/(60min)"log"((1.24xx10^-2))/((0.20xx10^(-2)))`
`=(2.303)/(60min)"log"6.2"min"^(_1)`
`k=0.0304"min"^(-1)`