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 ]

For the reaction $$A(g) \rightleftharpoons B(g)$$ at 495 K, $$\Delta$$_rG$$^\circ$$ = $$-$$9.478 kJ mol^$$-$$1.
If we start the reaction in a closed container at 495 K with 22 millimoles of A, the amount of B in the equilibrium mixture is ____________ millimoles.
(Round off to the Nearest Integer). [R = 8.314 J mol^$$-$$1 K^$$-$$1; ln 10 = 2.303]

A homogeneous ideal gaseous reaction $$A{B_{2(g)}} \rightleftharpoons {A_{(g)}} + 2{B_{(g)}}$$ is carried out in a 25 litre flask at 27$$^\circ$$C. The initial amount of AB₂ was 1 mole and the equilibrium pressure was 1.9 atm. The value of K_p is x $$\times$$ 10^$$-$$2. The value of x is _________. (Integer answer)

[R = 0.08206 dm³atm K^$$-$$1mol^$$-$$1]