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

Answer

B

Explanation

`-(d[N_(2)O_(5)])/(d t) = (1)/(2)(d[NO_(2)])/(d t) = (2d[O_(2)])/(d t) = R`