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

N_(2) + 3H_(2) hArr 2NH_(3)""K=4xx 10^(6)"at"298 ""K=41 "at" 400 k W

1.	N_(2) + 3H_(2) hArr 2NH_(3)""K=4xx 10^(6)"at"298 ""K=41 "at" 400 k Which statements is correct?
Answer» 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 . 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 speciesmeasured at that partial pressure. ADDITION of catalyst does not change `K_(p)` but changes`DELTAH`. At 400 K 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 isa function of temperture only.