One mole of an ideal gas expands at a constant temperature of $300 \, K$ from an initial volume of $10 \, L$ to a final volume of $20 \, L$. The work done in expanding the gas is ...... $J$. $(R = 8.31 \, J/mol \cdot K)$

One mole of ${O_2}$ gas having a volume equal to $22.4 \text{ litres}$ at $0^{\circ}C$ and $1 \text{ atmospheric pressure}$ is compressed isothermally so that its volume reduces to $11.2 \text{ litres}$. The work done in this process is ...... $J$.

$A$ poly-atomic molecule $(C_v = 3R, C_p = 4R$,where $R$ is the gas constant) goes from phase space point $A (P_A = 10^5 \ Pa, V_A = 4 \times 10^{-6} \ m^3)$ to point $B (P_B = 5 \times 10^4 \ Pa, V_B = 6 \times 10^{-6} \ m^3)$ and then to point $C (P_C = 10^4 \ Pa, V_C = 8 \times 10^{-6} \ m^3)$. The path $A$ to $B$ is adiabatic and the path $B$ to $C$ is isothermal. The net heat absorbed per unit mole by the system is:

Can the change in internal energy of an ideal gas be non-zero during an isothermal process?

Write the first law of thermodynamics for an isothermal process in an ideal gas.

In an isothermal process,the volume of an ideal gas is halved. One can say that: