Which one among the following is the correct option for the relationship between $C_{P}$ and $C_{V}$ for one mole of an ideal gas?

The magnitude of work done by a gas that undergoes a reversible expansion along the path $ABC$ shown in the figure is .............. $Joule$.

An ideal gas is expanded from $1 \times 10^{-3} \,m^3$ to $1 \times 10^{-2} \,m^3$ against a constant external pressure of $1 \times 10^5 \,N/m^2$ at $300 \,K$. The work done is

The change in internal energy of a system depends upon

The enthalpy of a reaction at $273 \, K$ is $-3.57 \, kJ$. If $\Delta C_p = 0$,what will be the enthalpy of the reaction at $373 \, K$?

Consider the following statements:
$(1)$ Joule-Thomson experiment is isoenthalpic as well as adiabatic.
$(2)$ $A$ negative value of $\mu_{JT}$ (Joule-Thomson coefficient) corresponds to warming of a gas on expansion.
$(3)$ The temperature at which neither cooling nor heating effect is observed is known as inversion temperature.
Which of the above statements are correct?