Consider the chemical reaction :
`N_(2)(g) +3H_(2)(g) rarr 2NH_(3)(g)`
The rate of this reaction can be expressed in terms of time derivative of concentration of `N_(2)(g), H_(2)(g) "or" NH_(3)(g)` . Identify the correct relationship amongst the rate expressions :

Options

A. Rate `= -(d[N_(2)])/(dt)=-1//3d[H_(2)]//dt=(1)/(2)d[NH_(3)]/dt`
B. Rate `= -d[N_(2)]//dt=-3d[H_(2)]//dt=(2d[NH_(3)])/(1)`
C. Rate `=d[N_(2)]//dt=1//3d[H_(2)]//dt=(1)/(2d[NH_(3)]dt)`
D. Rate `=-d[N_(2)]//dt=-d[H_(2)]//dt=d[NH_(3)]//dt`

Answer

C

Explanation

(A) Correct relationship is
Rate =` -(d[N_(2)])/(dt) = -(1)/(3) (d[H_(2)])/(dt) = (1)/(2) (d[NH_(3)])/(dt)`