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. `1 xx 10^(-4) M s^(-1)`
B. `4 xx 10^(-4) Ms^(-1)`
C. `5 xx 10^(-3) Ms^(-1)`
D. `1 xx 10^(-3) Ms^(-1)`

Answer

A

Explanation

Rate `= (1)/(2)(d[NH_(3)])/(dt)=-(1)/(3)(d[H_(2)])/(dt)=-(d[N_(2)])/(dt)`
`:. -(d[N_(2)])/(dt)=(1)/(2)(d[NH_(3)])/(dt)=(1)/(2)xx(2xx10^(-4)"Ms"^(-1))`
`=10^(-4)"M s"^(-1)`.