N_(2)3H_(2)hArr2NH_(3) K=4xx10^(6) "at" 298 K=41 "at" 400 K Which statements is correct?

N_(2)3H_(2)hArr2NH_(3) K=4xx10^(6) "at" 298 K=41 "at" 400 K Which st

1.	N_(2)3H_(2)hArr2NH_(3) K=4xx10^(6) "at" 298 K=41 "at" 400 K Which statements is correct?
Answer» If `N_(2)` is added at equilibrium 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. The condition for equilibrium is `2DeltaG_(NH_(3))=3DeltaG_(H_(2)+DeltaG_(N_(2))` where `G` gibbs free energy per mole of the gaseous species measured at that partial pressure. Addition of catalyst does not change `K_(P)` but CHANGES `DeltaH`. At `400K` addition of catalyst will increase forward reaction by `2` times while reverse reaction rate will be changed by `1.7` times. Solution :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 temperature only.