$6$ moles of an ideal gas expand isothermally and reversibly from a volume of $1$ litre to a volume of $10$ litres at $27\,^oC$. What is the maximum work done (in $, kJ$)?

$6$ moles of an ideal gas expand isothermally and reversibly from a volume of $1 \ L$ to a volume of $10 \ L$ at $27 \ ^oC$. What is the maximum work done? (in $kJ$)

One mole of a gas expands from $1 \, L$ to $5 \, L$ against a constant external pressure of $1 \, atm$. How much work is done in Joules (in $, J$)? $(1 \, L \cdot atm = 101.3 \, J)$

Under isothermal condition,a gas at $300 \; K$ expands from $0.1 \; L$ to $0.25 \; L$ against a constant external pressure of $2 \; bar$. The work done by the gas is .... [Given that $1 \; L \; bar = 100 \; J$]

$1 \ mol$ 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 $(R = 8.3 \ J \ K^{-1} \ mol^{-1})$.

The maximum work done in expanding $16 \, g$ of $O_2$ gas isothermally at $300 \, K$ from an initial volume of $5 \, dm^3$ to a final volume of $25 \, dm^3$ is: