Work done during isothermal expansion of one mole of an ideal gas from $10 \,atm$ to $1 \,atm$ at $300 \,K$ is.....$J$

What is the work done when a gas is compressed from $2.5 \times 10^{-2} \ m^3$ to $1.3 \times 10^{-2} \ m^3$ at a constant external pressure of $4.05 \ bar$ (in $J$)?

$6$ 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 $kJ$)

Explain pressure-volume work.

The work done when $2 \, mol$ of an ideal gas expands from $5 \, L$ to $15 \, L$ at a temperature of $300 \, K$ is .............. $kJ$.

One mole of a gas occupying $3 \ L$ volume is expanded against a constant external pressure of $1 \ bar$ to a volume of $15 \ L$. Calculate the work done by the system.