Statement-1 : The third law of thermodynamics implies that absolute zero cannot be reached.
Statement-2 : `Delta G^(@)` for an ideal gas reaction is a function of temperature.
Statement-3 : The adiabatic expansion of a gas into a vacuum is spontaneous.

Statement -I : There is no change in enthalpy of an ideal gas during compression at constant temperature. Statement-II: Enthalpy of an ideal gas is a function of temperature and pressure.

Select the correct statement for isothermal expansion of an ideal gas

In the adiabetic expansion of an ideal gas, select the incorrect statement.

Statement- 1 : A real gas behaves as an ideal gas at high temperature and low pressure . Statement- 2 : Liquid state of an ideal gas is impossible.

Statement-1: The amount of work done in the isothermal expansion is greater than work done in the adiabatic system for same final volume. Statement-2: In the adiabatic expansion of a gas temperature and pressure both decrease due to decrease in internal energy of the system.

Statement-1: Temperature of gas increases when its container is moved at constant speed. Statement-2: The temperature of the gas is due to the random motion of its molecule.

Statement-1 : In a cyclic process, both Delta H and Delta U are zero. And Statement-2 : Delta H and Delta U are path dependent functions.

Statement-1: If the pressure and temperature of a gas sample are doubled then the volume of the gas will remain unchanged. Statement-2: Molar specific heat for an adiabatic process is zero. Statement-3: Heat energy is a path function.

Statement-1 : All the exothermic reactions are spontaneous. And Statement-2 : For a spontaneous reaction, Delta G must be negative.

Statement-1 : Delta H_(f)^(@) is zero for oxygen (O_(2)) . And Statement-2 : Delta H_(f)^(@) for all the elements at S.T.P. is zero.