`N_(2) + 3H_(2) hArr 2NH_(3)" "K=4xx 10^(6)"at"298`
`" "K=41 "at" 400 k`
Which statements is correct?

Options

A. If `N_(2)` is added at equlibrium condition, the equilibrium will shift to the forward direction because according to `II^(nd)` law of thermodynamics the entropy must increases in the direction of spontaneous reaction .
B. The condition for equlibrium is `2DeltaG_(NH_(3)) = 3DeltaG_(N_(2)) + DeltaG_(N_(2))` where G is Gibbs free energy per mole of the gaseous species measured at that partial pressure.
C. Addition of catalyst does not change `K_(p)` but changes `DeltaH`.
D. At 400 K addition of catalyst will increase forward reaction by `2` times while reverse reaction rate will be changed by 1.7 times.

Answer

B

Explanation

When nitrogen is added at equilibrium condition, the equilibrium will shift according to Le- chatelier principle at equilibrium `DeltaG^(@)=0` and catalyst changes the rate of forward and backward reactions by equal extent. `K_(P)` of reaction is a function of temperture only.