The work done when $2 \ mol$ of an ideal gas expands reversibly and isothermally from a volume of $1 \ L$ to $10 \ L$ at $300 \ K$ is $(R = 0.0083 \ kJ \ K^{-1} \ mol^{-1})$ (in $kJ$)

In which of the following processes does the internal energy of a system remain constant?

For a change in state of $1 \, \text{mole}$ of a non-ideal gas,the change in internal energy is $\Delta U = 30.0 \, \text{L} \cdot \text{atm}$. The state changes from $(2.0 \, \text{atm}, 3.0 \, \text{L}, 95 \, \text{K})$ to $(4.0 \, \text{atm}, 5.0 \, \text{L}, 245 \, \text{K})$. What is the change in enthalpy $(\Delta H)$ in $\text{L} \cdot \text{atm}$?

Which of the following are extensive properties?
$(A)$ Heat capacity
$(B)$ Entropy
$(C)$ Gibbs' energy
$(D)$ Concentration
$(E)$ Vapour pressure

Evaporation of water is

What is the internal energy change when $2$ moles of an ideal gas at $25^{\circ} C$ is compressed isothermally and reversibly from $1.0 \ bar$ to $10.0 \ bar$?