For the reaction `N_(2) + 3 H_(2) hArr 2 NH_(3)` equilibrium constant is `K_(1)` and that of for the reaction `NH_(3) hArr (1)/(2) N_(2) + (3)/(2) H_(2) is K_(2)` . (ii) Then calculate the relation between `K_(1)` and `K_(2)` .

(i) State law of mass action. (ii) For the reaction N_(2)+3H_(2)hArr 2NH_(3) equilibrium constant is K_(1) and that of for the reaction NH_(3)hArr (1)/(2)N_(2)+(3)/(2)H_(2) is K_(2) . Then calculate the relation between K_(1) and K_(2) . (iii) Calculate the pH of 0.01 (M) CH_(3)COOH at 25^(@)C . (K_(a)" of "CH_(3)COOH=1.75xx10^(-5)) .

For the reaction N_2 + 3H_2 harr 1/2 N_2 + 3/2 H_2 is K_2 . Then calculate teh relation between K_1 and K_2

For the reaction, N_2(g)+3H_2(g)hArr2NH_3(g) +heat the equilibrium shifts in forward direction-

The equilibrium constant for the reaction N_(2) + 3H_(2) hArr 2NH_(3) is 'K' . Then the equilibrium constant for the reaction 2N_(2) + 6H_(2) hArr 4NH_(3) will be

In the reaction, H_(2)(g)+I_(2)(g)hArr 2HI(g) , the value of equilibrium constant (K_(P)) changes with change in _____.

For reaction N_2(g)+3H_2(g)hArr 2NH_3(g) which of the following is valid

Write the expressions of K_(c) and K_(p) for the reaction: 3O_(2)(g)hArr2O_(3)(g) .

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.

For the reaction, 2NH_3(g) iff N_2(g) + 3H_2(g) the units of K_p will be

For the reaction, N_2(g)+O_2(g)hArr2No(g) equilibrium constant is K_1 . The equilibrium constant is K_2 for the reaction. 2NO(g)+O_2(g)hArr2NO_2(g) . What is K for the reaction, NO_2(g)hArr1/2N_2(g)+O_2(g) -