$1 \ mol$ of an ideal gas is allowed to expand isothermally and reversibly from $1 \ L$ to $5 \ L$ at $300 \ K$. The change in enthalpy (in $kJ$) is $(R = 8.3 \ J \ K^{-1} \ mol^{-1})$.

Which of the following thermodynamic relations is correct?

Which of the following is not an extensive property?

The work done when $2 \ mol$ of an ideal gas expands reversibly and isothermally from a volume of $1 \ L$ to $10 \ L$ at $300 \ K$ is $(R = 0.0083 \ kJ \ K^{-1} \ mol^{-1})$ (in $kJ$)

Fill in the blanks:
$(i)$ The change in heat energy during a chemical reaction at constant volume is called .......
$(ii)$ During a ....... process,there is no absorption or evolution of heat.
$(iii)$ The equation $\Delta G = \Delta H - T \Delta S$ was proposed by .......

In an irreversible expansion of a gas,the work done by the gas is given by.....