`N_(2)+3H_(2) hArr 2NH_(3)`
Which of the following statements is correct if `N_(2)` added at equilibrium condition?

Options

A. The equilibrium will shift to forward direction because according to 2nd law of thermodynamics, the entropy must increase in the direction of the spontaneous reaction
B. The condition for equilibrium is `G(N_(2))+3G(H_(2))=2G(NH_(3))` , where G is Gibbs free energy per mole of the gaseous species measured at ehtir partial pressure. The condition of equilibrium is unaffected by the use of catalyst which increases the rate of both the forward and the backward directions to the same extent
C. The catalyst will increase the rate of forward reaction by `beta`.
D. The catalyst will not alter the rate either of the reaction.

Answer

B

Explanation

At equilibrium , `Delta G=0`
i.e., `Sigma` ( Reactant) `=Sigma G` ( Product) .
Further, the condition of equilibrium is unaffected by the use of catalyst which increases the rate of forward and backward reaction to the same extent.