2NOCl(g) $$\rightleftharpoons$$ 2NO(g) + Cl_{2}(g)

In an experiment, 2.0 moles of NOCl was placed in a one-litre flask and the concentration of NO after equilibrium established, was found to be 0.4 mol/L. The equilibrium constant at 30$$^\circ$$C is ______________ $$\times$$ 10^{$$-$$4}.

40% of HI undergoes decomposition to H_{2} and I_{2} at 300 K. $$\Delta$$G$$^\Theta $$ for this decomposition reaction at one atmosphere pressure is __________ J mol^{$$-$$1}. [nearest integer]

(Use R = 8.31 J K^{$$-$$1} mol^{$$-$$1} ; log 2 = 0.3010, ln 10 = 2.3, log 3 = 0.477)

The standard free energy change ($$\Delta$$G$$^\circ$$) for 50% dissociation of N_{2}O_{4} into NO_{2} at 27$$^\circ$$C and 1 atm pressure is $$-$$ x J mol^{$$-$$1}. The value of x is ___________. (Nearest Integer)

[Given : R = 8.31 J K^{$$-$$1} mol^{$$-$$1}, log 1.33 = 0.1239 ln 10 = 2.3]

PCl_{5} dissociates as

PCl_{5}(g) $$\rightleftharpoons$$ PCl_{3}(g) + Cl_{2}(g)

5 moles of PCl_{5} are placed in a 200 litre vessel which contains 2 moles of N_{2} and is maintained at 600 K. The equilibrium pressure is 2.46 atm. The equilibrium constant K_{p} for the dissociation of PCl_{5} is __________ $$\times$$ 10^{$$-$$3}. (nearest integer)

(Given : R = 0.082 L atm K^{$$-$$1} mol^{$$-$$1}; Assume ideal gas behaviour)