`N_(2) (g) + 3 H_(2) (g) hArr 2 NH_(3) (g)`
`NH_(3)` is x . Express `K_(p)` of the reaction with respect to x and P , where value of x is very small .

N_(2)+3H_(2)hArr 2NH_(3) . Total pressure of the system is P and mole-fraction of NH_(3) is x. express K_(p) of the reaction with respect to x and P, where value of x is very small.

For the reaction, N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g) express the rate of the reaction with respect to the reactants and the product formed.

For the following reaction : NH_(2) COO NH_(4) (s) hArr 2 NH_(3) (g) + CO_(2) (g) If the total pressure of the system at equilibrium is 3 atm , then the value of K_(p) will be -

N_2(g) + 3H_2(g) → 2 NH_3(g) . For the above reaction the correct statement is

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

Consider the equilibrium: N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)+ heat. Apply the i.e., chatelier's principle to explain the effect of pressure, temperature and addition of inert gas at constant volume on the equilibrium yield of NH_(3) .

Equilibrium constant, K_(c) for the reaction, N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g) at 500K is 0.061. at a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol*L^(-1)" "N_(2),2.0mol*L^(-1)" "H_(2) and 0.5mol*L^(-1)NH_(3) . is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium ?

N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g) , For this reaction ......... xx rate of disappearance of H_(2) = …………….. xx rate of production of NH_(3)

At a constant temperature, the equilibrium constant of the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is K and that of the reaction (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g)hArrNH_(3)(g) is sqrt(K) . Explain this difference of K values in spite of the fact that the reactants and products in both the reactions are same.