The equilibrium pressure of `CO_2`, CO and `O_2` for the reaction `2CO_2(g)iff2CO(g)+O_2(g)` at 3000K are 0.6, 0.4 and 0.2 atm respectively calculate (i) `K_p` and (ii) `K_c` for this reaction at that temperature.

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

Establish the relation between K_p and K_c for the reaction 2SO_2(g)+O_2(g)iff2SO_3(g)

For the reaction 2SO_2(g) + O_2 (g) iff 2SO_3 (g) at 300K, the value of DeltaG^@ is - 690.9R. The equilibrium constant value for the reaction at that temperature is (R is gas constant)

The value of K_p for the reaction 2H_2O(g) +2Cl_2(g) iff 4HCl(g) +O_2(g), is 0.035 atm at 400^@C , when the partial pressure are expressed in atmosphere. Calculate the value of K_c for the same reaction.

Find out K_(p)//K_(c) for the reactio CO(g)+(1)/(2)O_(2)(g)hArr CO_(2)(g) .

At a particular temperature, CO(g) reacts with Cl_(2)(g) in a closed container to produce COCl_(2)(g) . In the equilibrium mixture, partial pressures of CO(g), Cl_(2)(g) and COCl_(2)(g) are found to be 0.12, 1.2 and 0.58 atm respectively. Find the value of K_(p) of the reaction, CO(g)+Cl_(2)(g)hArr COCl_(2)(g) .

The equilibrium constants of the reactions : SO_2 +1/2 O_2 iff SO_3 and 2SO_2 + O_2(g) iff 2SO_3(g) and K_1 and K_2 respectively. The relationship between K_1 and K_2 is

The equilibrium constant (K_c) for the reaction N_2(g) + O_2(g) rarr 2NO (g) at temperature T is 4 xx 10^-4 . The value of K_c for the reaction NO(g) rarr 1/2 N_2(g) + 1/2 O_2(g) at the same temperature is