The reaction, `2NO+2H_(2)rarr N_(2)+2H_(2)O` has been assigned to follow the following mechanism :
I. `NO+NO hArr N_(2)O_(2)" "` (fast)
II. `N_(2)O_(2)+H_(2) rarr N_(2)O+H_(2)O " "` (slow)
III. `N_(2)O +H_(2) rarr N_(2)+H_(2)O " "` (fast)
The rate constant of step II is `1.2 xx 10^(-4) "mole"^(-1)L"min"^(-1)` while equilibrium constant of step I is `1.4 xx 10^(-2)`. What is the rate of reaction when concentration of `NO` and `H_(2)` each is `0.5` mole `L^(-1)` ?

Options

A. `2.1 xx 10^(-7)` mol`L^(-1) "min"^(-1)`
B. `3.2 xx 10^(-6)` mol`L^(-1) "min"^(-1)`
C. `3.5 xx 10^(-4)` mol`L^(-1) "min"^(-1)`
D. None of above

Answer

A