For the reaction `N_(2)O_(5) rarr 2NO_(2) + (1)/(2) O_(2)`, the rate of disappearance of `N_(2)O_(5)` is `6.25 xx 10^(-3) "mol L"^(-1) s^(-1)`. The rate of formation of `NO_(2)` and `O_(2)` will be respectively.

Options

A. `6.25 xx 10^(-3) mol L^(-1)s^(-1) & 6.25 xx 10^(-3) mol L^(-1)s^(-1)`
B. `1.25 xx 10^(-2) mol L^(-1)s^(-1) & 3.125 xx 10^(-3) mol L^(-1)s^(-1)`
C. `6.25 xx 10^(-3) mol L^(-1)s^(-1) & 3.125 xx 10^(-3) mol L^(-1) s^(-1)`
D. `1.25 xx 10^(-2) mol L^(-1) s^(-1) & 3.125 xx 10^(-3) mol L^(-1) s^(-1)`

Explanation

`-(d[N_2O_5])/(dt)= 1/2(d[NO_2])/(dt)= (2d[O_2])/(dt)`