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

Enthalpy and entropy change for a chemical reaction are –2.5 × 10³ cal and 7.4 cal deg^–1 respectively. Reaction at 298 K is -

(1) Spontaneous

(2) Reversible

(3) Irreversible

(4) Non-spontaneous

The entropy changed involved in the conversion of 1 mole of liquid water at 373 K to vapour at the same temperature will be $[\Delta H_{\text{vap}}=2.257kJ/gm]$ [MP PET 2002]

(1) 0.119 kJ

(2) 0.109 kJ

(3) 0.129 kJ

(4) 0.120 kJ

When a liquid boils, there is [JIPMER 2002]

(1) An increase in entropy

(2) A decrease in entropy

(3) An increase in heat of vaporization

(4) An increase in free energy