Work done when $2 \ mol$ of an ideal gas is compressed from a volume of $5 \ m^{3}$ to $2.5 \ m^{3}$ at $300 \ K$, under a constant external pressure of $100 \ kPa$ is: (in $kJ$)

What is the constant external pressure of an ideal gas when expanded from $2 \times 10^{-2} \ m^3$ to $3 \times 10^{-2} \ m^3$,if the work done by the gas is $-5.09 \ kJ$?

What will be the difference in heat at constant pressure and constant volume for the combustion of carbon monoxide at $27 \, ^oC$ in $cal$?

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 $\text{L} \cdot \text{atm}$?

The number of extensive and intensive properties in the following list is respectively: Mass,temperature,pressure,enthalpy,heat capacity,internal energy,density.

Which of the following statements is not correct?