In a catalyst experiment involving the Haber process `N_(2) + 3H_(2) rarr 2NH_(3)`, the rate of reaction was measured as
Rate `= (Delta[NH_(3)])/(Delta t) = 2.0 xx 10^(-4) mol L^(-1) s^(-1)`
What is the rate of reaction expressed in terms of (a) `N_(2)` (b) `H_(2)` ?

Options

A. `2.50 xx 10^(-4) mol L^(-1) s^(-1)`
B. `1.25 xx 10^(-4) mol L^(-1) s^(-1)`
C. `3.75 xx 10^(-4) mol L^(-1) s^(-1)`
D. `5.00 xx 10^(-4) mol L^(-1) s^(-1)`

Answer

C

Explanation

`N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g)`
Rate `= (-d[N_(2)])/(dt) = (-d[H_(2)])/(3 dt) = (+d[NH_(3)])/(2dt)`
`:. (-d[H_(2)])/(dt) = (3)/(2)(d[NH_(3)])/(dt)`
`= (3)/(2) xx 2.5 xx 10^(-4) mol L^(-1) s^(-1)`
`= 3.75 xx 10^(-4) mol L^(-1) s^(-1)`