If $∆{\mathrm{H}}_{\mathrm{f}}^{°}$(C₂H₄) and $∆{\mathrm{H}}_{\mathrm{f}}^{°}$(C₂H₆) are x₁ and x₂ kcal/mol then heat of hydrogenation of C₂H₄ is :-

(1) x₁ + x₂

(2) x₁ - x₂

(3) x₂ - x₁

(4) x₁ + 2x₂

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