1 mol of CH_4, 1 mole of CS_2 and 2 mole of H_2S are 2 mol of H_2 are mixed in a 500 mL flask. The equilibrium constant for the reaction K_C = 4 xx 10^(-2) mol^2 lit^(-2). In which direaction will the reaction proceed to reach equilibrium ?

1 mol of CH_4, 1 mole of CS_2 and 2 mole of H_2S are 2 mol of H_2 are

1.	1 mol of CH_4, 1 mole of CS_2 and 2 mole of H_2S are 2 mol of H_2 are mixed in a 500 mL flask. The equilibrium constant for the reaction K_C = 4 xx 10^(-2) mol^2 lit^(-2). In which direaction will the reaction proceed to reach equilibrium ?
Answer» Solution :`CH_4 (g)+ 2H_2S (g) hArr CS_2(g) + 4H_2(g)` `K_C =4 xx 10^(-2) mol^2 L^(-2)` VOLUME`= 500 mL= 1/2 L` `[CH_4]= (1 mol)/(1/2L) = 2mol L^(-1)` `[CS_2] = (1 mol)/(1/2L) = 2mol L^(-1)` `[H_2S] = (2 mol)/(1/2L) = 4mol L^(-1)` `[H_2]= (2mol)/(1/2L) = 4 mol L^(-1)` `Q = ([CS_2][H_2]^4)/([CH_4][H_2S]^2)` `:. Q = (2 xx (4)^4)/(2 xx (4)^2) = 16` `Q gt K_C` `:.` The reaction will PROCEED in the reverse direction to REACH the equilibrium.