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]

Consider the reaction

$$N_{2}O_{4}\left( g\right) \rightleftharpoons 2NO_{2}\left( g\right) $$

The temperature at which K_C = 20.4 and K_P = 600.1, is ____________ K. (Round off to the Nearest Integer). [Assume all gases are ideal and R = 0.0831 L bar K^$$-$$1 mol^$$-$$1]

0.01 moles of a weak acid HA (K_a = 2.0 $$\times$$ 10^$$-$$6) is dissolved in 1.0 L of 0.1 M HCl solution. The degree of dissociation of HA is __________ $$\times$$ 10^$$-$$5 (Round off to the Nearest Integer).

[Neglect volume change on adding HA. Assume degree of dissociation <<1 ]