For the reaction : `N_(2(g))+3H_(2(g))hArr2NH_(3(g))`, `DeltaH=-ve`, the correct statement is :

Options

A. addition of catalyst does not change `K_(p)` but changes `DeltaH`
B. at equilibrium, `2G_(NH_(3))=G_(N_(2))+3H_(H_(2))` (`G` is Gibbs' energy)
C. at higher temperature, the rate of forward and backward reaction increases by a factor `2`.
D. at `400 K`, addition of catalyst increases rate of forward reaction by `2 times` and backward by `1.7 times`.

Explanation

`DeltaG=2G_(NH_(3))-G_(N_(2))-3xxG_(H_(2))`
and `Delta G=0` at equilibrium