For the reaction

A + B $$\rightleftharpoons$$ 2C

the value of equilibrium constant is 100 at 298 K. If the initial concentration of all the three species is 1 M each, then the equilibrium concentration of C is x $$\times$$ 10^$$-$$1 M. The value of x is ____________. (Nearest integer)

Value of K_P for the equilibrium reaction

N₂O_4(g) $$\rightleftharpoons$$ 2NO_2(g) at 288 K is 47.9. The K_C for this reaction at same temperature is ____________. (Nearest integer)

(R = 0.083 L bar K^$$-$$1 mol^$$-$$1)

2SO₂(g) + O₂(g) $$\rightleftharpoons$$ 2SO₃(g)

In an equilibrium mixture, the partial pressures are

P_SO3 = 43 kPa; P_O2 = 530 Pa and P_SO2 = 45 kPa. The equilibrium constant K_P = ___________ $$\times$$ 10^$$-$$2. (Nearest integer)

The gas phase reaction $$2A(g) \rightleftharpoons {A_2}(g)$$ at 400 K has $$\Delta$$G^o = + 25.2 kJ mol^-1.

The equilibrium constant K_C for this reaction is ________ $$\times$$ 10^$$-$$2. (Round off to the Nearest Integer).

[Use : R = 8.3 J mol^$$-$$1 K^$$-$$1, ln 10 = 2.3 log₁₀ 2 = 0.30, 1 atm = 1 bar]

[antilog ($$-$$0.3) = 0.501]