An ideal gas is allowed to expand from $2 \ dm^3$ to $6 \times 10^{-3} \ m^3$ against a constant external pressure of $1 \ bar$. The work done in $kJ$ is (in $kJ$)

Find the work done on $2 \ mol$ of an ideal gas at $27^{\circ} C$ if it is compressed reversibly and isothermally from $5.05 \times 10^6 \ Nm^{-2}$ to $1.01 \times 10^5 \ Nm^{-2}$ pressure. (in $kJ$)

$A$ state function is .......

Calculate the work done during compression of $2 \ mol$ of an ideal gas from a volume of $1 \ m^3$ to $10 \ dm^3$ at $300 \ K$ against a constant external pressure of $100 \ kPa.$

The heat $Q$ for a reaction at constant volume is equal to

At $T(K)$,$2 \ mol$ of an ideal gas is allowed to expand reversibly and isothermally from a pressure of $10 \ atm$ to $1 \ atm$. The work done (in $kJ$) is $(R=8.3 \ J \ K^{-1} \ mol^{-1})$.