Consider the following processes :

	H (kJ/mol)
1/2A $$ \to $$ B	+150
3B  $$ \to $$ 2C + D	-125
E + A  $$ \to $$ 2D	+350

For B + D $$ \to $$ E + 2C, $$\Delta $$H will be

If the enthalpy change for the transition of liquid water to steam is 30 kJ mol^$$-$$1 at 27^oC, the entropy change for the process would be

Enthalpy change for the reaction,
4H_(g)  $$ \to $$  2H_2(g) is $$-$$869.6 kJ
The dissociation energy of H $$-$$ H bond is

Which of the following is correct option for free expansion of an ideal gas under adiabatic condition ?