The work done by a gas is maximum when it expands from a volume $V_1$ to $V_2$. This expansion is:

An ideal diatomic gas is heated at constant pressure. The ratio of the work done to the heat supplied is

$A$ frictionless piston-cylinder based enclosure contains some amount of gas at a pressure of $400 \text{ kPa}$. Heat is transferred to the gas at constant pressure in a quasi-static process. The piston moves up slowly through a height of $10 \text{ cm}$. If the piston has a cross-sectional area of $0.3 \text{ m}^2$, the work done by the gas in this process is: (in $\text{ kJ}$)

The change in the internal energy of $3$ moles of a gas heated at constant volume from $20^{\circ}C$ to $40^{\circ}C$ is $1080 \ J$. The molar specific heat of the gas at constant volume in $J \ mol^{-1} \ K^{-1}$ is:

$A$ monoatomic ideal gas is heated at constant pressure. The percentage of total heat used in changing the internal energy is (in $\%$)

$A$ monoatomic gas $(\gamma = 5/3)$ expands at constant pressure when heat is supplied. What percentage of the heat supplied is converted into internal energy and work, respectively?