Derive the relation between `K_(p)` and `K_(c)` for the equilibrium reaction.
`N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)`

K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2N_(3)(g) is 0.5 at 400K find K_(p)

Decribe the effect of : addition of CH_(3)OH on the equilibrium of the reaction 2H_(2)(g)+CO(g) hArr CH_(3)OH(g)

A mixture of 1.57 mol of N_(2) , 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20L reaction vessel at 500K . At this temperature, the equilibrium constant, K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium ? If not, what is the direction of the net reaction ?

A mixture of H_(2), N_(2) and NH_(3) with molar concentration 5.0xx10^(-3) "mol" L^(-1), 4.0xx10^(-3) "mol" L^(-1) and 2.0xx10^(-3) "mol" L^(-1) respectively was prepared and heated to 500K . The value of K_(c) for the reaction: 3H_(2)(g)+N_(2)(g)hArr2NH_(3)(g) at this temperature is 60. Predict whether ammonia tends to form or decompose at this stage of concenration.