The equilibrium constant expression for a gas reaction is.`K_C = frac([NH_3]^4[O_2]^5) ([NO]^4[H_2O]^6)`Write the balanced chenmicl equatin corresponding to this expression.

Write expressions of k_c for following chemical reactions. N_2 O_4(g) harr 2NO_2(g) .

Write the expression for: 2 N_2O(g)rarr 4 NO_2(g) + O_2(g) ?

Write reaction of alc. NH_3 with C_6H_5I .

Equilibrium constant, K_c for the reaction, N_2(g) +3H_2(g) hArr 2NH_3(g) _(at 500 k is 0.061) At a particular time, the analysis shows that composition of the reaction mixtue is 3.0 mol L^(-1) N_2,2.0 mol L^(-1) H_2 .5 mol L^(-1) NH_3 Is the eaction at equilibrium ?If not in which direction does the reaction tend to proceed to reach equilibrium?

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 20 L reaction vessel at 500 kAt this temperature,the equilibrium constant. K_C for the reaction N_2(g) + 3H_2(g) hArr 2NH_3(g) is 1.7 xx 10 ^2 .Is the reaction mixture at equilibrium?If not,what is the direction of the net reaction?

Write expressions of k_c for following chemical reactions. 2SO_2(g) + O_2(g) harr 2SO_3(g) .

The equilibrium constant (K_c) for the reaction N_2(g) + O_2 (g) rarr 2NO (g) at temperature T is 4xx10^(-4) .The value of K_c for the reaction, NO(g) rarr1//2 N_2 (g) +1//2O_2 (g) at the same temperature is:

One mole of H_2O and one mole of CO are taken in 10L vessel and heated to 725 K.At equilibrium 40% of water (by mass) reacts with CO according to the equatin H_2O(g0 + CO(g) hArr H_2(g) +CO_2(g) Calculate the equilibrium constant for the reaction.