For the reaction, X₂O₄(l) $\to$2XO₂(g)

$∆$U = 2.1 kcal, $∆$S = 20 cal K^-1 at 300 K. Hence, $∆$G is

(1) 2.7 kcal

(2) -2.7 kcal

(3) 9.3 kcal

(4) -9.3 kcal

The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0°C is

(a) 10.52 cal/(mol K)

(b) 21.04 cal/(mol K)

(c) 5.260 cal/(mol K)

(d) 0.526 cal/(mol K)

The enthalpy and entropy change for the reaction :

Br₂(l)+Cl₂(g) $\to$ 2BrCl(g) are 30 kJ mol^-1 and 105 JK^-1 mol^-1 respectively.

The temperature at which the reaction will be in equilibrium is :

1. 285.7 K

2. 273 K

3. 450 K

4. 300 K

The temperature of the system decreases in an

(1) Adiabatic compression

(2) Isothermal compression

(3) Isothermal expansion

(4) Adiabatic expansion

Mark the correct statement 

(1) For a chemical reaction to be feasible, ΔG should be zero

(2) Entropy is a measure of order in a system

(3) For a chemical reaction to be feasible, ΔG should be positive

(4) The total energy of an isolated system is constant

Which of the following is not a state function 

(1) Internal energy

(2) Enthalpy

(3) Work

(4) Entropy

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at 25°C is 

(1) -$2.303\times 298\times 0.082\log 2$

(2) -$298\times {10}^7\times 8.31\times 2.303\log 2$

(3)- $2.303\times 298\times 0.082\log 0.5$

(4) $8.31\times {10}^7\times 298-2.303\log 0.5$

An ideal gas expands in volume from 1 × 10^–3 m³ to 1 × 10^–2 m³ at 300 K against a constant pressure of 1 × 10⁵ Nm^–2. The work done is [AIEEE 2004]

(1) 270 kJ

(2) –900 kJ

(3) –900 J

(4) 900 kJ

Mixing of non-reacting gases is generally accompanied by

(1) Decrease in entropy

(2) Increase in entropy

(3) Change in enthalpy

(4) Change in free energy

An irreversible process occuring isothermally in an isolated system leads to

(1) Zero entropy

(2) An increase in the total entropy of the system

(3) A decrease in the total entropy of the system

(4) None of these