$2$ moles of an ideal gas expands isothermally from $5$ $dm^3$ to $10$ $dm^3$ at a constant external pressure of $1.5$ bar. Calculate the work done.

For the process to occur under adiabatic conditions,the correct condition is:

In an endothermic reaction,the value of $\Delta H$ is

If $0.75 \ mol$ of an ideal gas expands isothermally at $27 \ ^{\circ}C$ from $15 \ L$ to $25 \ L$,the maximum work obtained is ...... $J$. (in $.5$)

Which of the following is not a state function?

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