Given that bond energies of H—H and CI—CI are 430 kJ mol^-1 and 240 kJ mol^-1. respectively and ΔH_f for HCI is

-90 kJ mol^-1.  Bond enthalpy of HCI is

Given the following entropy values (in JK^-1 mol^-1) at 298 K and 1 atm : H₂(g) : 130.6, CI₂(g) : 223.0, HCI(g) : 186.7.  The entropy change (in Jk^-1 mol^-1) for the reaction

H₂(g) + CI₂(g) → 2HCI(g), is

Heat of combustion ΔH^o for C(s), H₂(g) and CH₄(g) are -94, -68 and -213 kcal/mol.  Then, ΔH^o for C(s) + 2H₂(g)→ CH₄ (g) is

Consider the following reactions

(i)  H⁺ (aq) + OH^- (aq) = H₂O(l)                 -  x₁ kJ mol^-1

(ii)  H₂(g) + O₂ (g) = H₂O (l)                     x₂ kJ mol^-1

(iii)  CO₂ (g) + H₂ (g) = CO (g) + H₂O(l)       -x₃ kJ mol^-1

(iv)  C₂H₂(g) + O(g) = 2CO₂ (g) + H₂O (l)    + x₄ kJ mol^-1

Enthalpy of formation of H₂O(l) is

If ΔE is the heat of reaction for

C₂H₅OH(I) + 3O₂(g) → 2CO₂ (g) + 3H₂O(I)

at constant volume, the ΔH (heat of reaction at constant pressure), then the correct relation is

Identify the correct statement for change of Gibb's energy for a system (ΔG_system ) at constant temperature and pressure.

The work done during the expansion of a gas from a volume of 4 dm³ to 6 dm³ against a constant external pressure of 3 atm, is

If ΔH is the change in enthalpy and ΔE, the change in internal energy accompanying a gaseous reaction, then

For the reaction,

C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(l) at constant temperature, H - E is

The densities of graphite and diamond at 298 K are 2.25 and 3.31 g cm^-3 , respectively.  If the standard free energy difference (ΔG^o ) is equal to 1895 J mol^-1, the pressure at which graphite will be transformed into diamond at 298 K is