Conisder 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 derivatives of the concentration of `N_(2)(g), H_(2)(g)`, or `NH_(3)(g)`. Identify the correct relationship among the rate expresisons.

Options

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

Answer

A

Explanation

`2N_(2)(g) + 3H_(2)(g) rarr 2NH_(3) (g)`
Rate `= (-d[N_(2)])/(dt) = -(1)/(3)(d[H_(2)])/(dt) = +(1)/(2)(d[NH_(3)])/(dt)`
The concentration of the reactants decrease and the concentration of the Products increase with the progress of the reaction. To equalize the rates with respect to various components, suitable coefficients are used.