If $\gamma$ is the ratio of molar specific heat at constant pressure to molar specific heat at constant volume for a gas,find the change in internal energy of $1 \, mol$ of the gas when its volume changes from $V$ to $2V$ at constant pressure $P$.

The state of a thermodynamic system changes from $(1)$ $(P_1, V)$ to $(2P_1, V)$ and $(2)$ $(P, V_1)$ to $(P, 2V_1)$. The work done during these two processes is respectively:

$A$ quantity of heat $Q$ is supplied to a monoatomic ideal gas which expands at constant pressure. The fraction of heat that goes into work done by the gas 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 internal energy of a mass of gas,when the volume changes from $V$ to $2V$ at constant pressure $P$,is (where $\gamma$ is the ratio of $C_p$ to $C_v$):

When heat is given to a gas in an isobaric process,then