Thermodynamics ...

Consider the following reactions at 1100°C
(I) 2C + O₂ → 2CO, ∆G° = - 460 kJ mol^-1
(II) 2Zn + O₂ → 2 ZnO, ∆G° = - 360 kJ mol^-1
Based on these, select correct alternate.

For which reaction change of entropy will be positive ?

The value of log K_c for a reaction
A ⇌ B is (Given, ∆_r H° 298 K = - 54.07 kJ mol^-1 , ∆_r S ° 298 K =10 JK^-1 mol^-1 and R = 8.314 JK^-1 mol^-1 2.303 × 8.314 × 298 = 5705)

Enthalpy is equal to

In an irreversible process taking place at constant T and p and in which only pressure-volume work is being done, the change in Gibbs free energy (dG) and change in entropy (dS ), satisfy the criteria.

For the reaction at 298 K
A(g) + B(g) ⇌ C(g) + D(g)
∆H° = - 29.8 kcal , ∆S° = - 0.100 kcal K^-1
What is the value of ∆G° ?

The direct conversion of A to B is difficult, hence it is carried out by the following shown path

The internal energy of one mole of a monoatomic gas is

The correct relationship between ∆H and ∆E for an ideal gas at constant temperature is

You are given the following two reactions:
(i)CH₄(g) + 20₂(g) → CO₂ (g) + 2H₂O(g), ∆H = - 890.4 kJ.
(ii)2HgO(s) → 2Hg(l) + O₂(g) – 181.6 kJ
Which one of the following statements is correct