The reaction,
2A_(g) + B_(g) $$\rightleftharpoons$$ 3C_(g) + D_(g)
is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measuread and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression

For vaporization of water at 1 atmospheric pressure, the values of $$\Delta $$H and $$\Delta $$S are 40.63 kJ mol^$$-$$1 and 108.8 J K^$$-$$1 mol^$$-$$1, respectively. The temperature when Gibb's energy change ($$\Delta $$G) for this transformation will be zero, is

The following two reactions are known

Fe₂O_3(s) + 3CO_(g) $$ \to $$ 2Fe_(s) + 3CO_2(g); $$\Delta $$H = $$-$$ 26.8 kJ

FeO_(s) + CO(g) $$ \to $$  Fe_(s) + CO_2(g); $$\Delta $$H = $$-$$ 16.5 kJ

The value of $$\Delta $$H for the following reaction

Fe₂O_3(s) + CO_(g) $$ \to $$  2FeO_(s) + CO_2(g) is

Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be