`N_(2)+3H_(2)hArr2NH_(3)`
Which is correct statement if `N_(2)` is added at equilibrium condition?

Options

A. The equilibrium will shift to forward direction because according to Iind law of the thermodynamcis the entropy must increase in the direction of spontaneous reaction.
B. The condition for equilibrium is `G_(N_(2)) + 3G_(NH_(3)) = 2G_(NH_(3))`, where G is Gibbs free energy per mole of the gaseous species measured at that partial pressure. The condition of equilibrium is unaffected by the ue of catalyst, which increases the rate of both the forward and backward reactions to the same extant.
C. The catalyst will increase the rate of forward reaction by `alpha` and that of backward reaction by `beta`.
D. Catalyst will not alter the rate of either of the reaction.

Answer

b

Explanation

Catalyst does not after the equilibrium established in lesser time in the presence of catalyst.