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

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?

It is a general principle that the less energy a system contains,it is:

Find the work done $W_{ABC}$ for the process $A$ $\rightarrow B$ $\rightarrow C$ in $L \cdot atm$.

If $\Delta H$ is the change in enthalpy,$\Delta U$ is the change in internal energy,$N_P$ is the number of moles of products,and $N_r$ is the number of moles of reactants,then which of the following is correct for a gaseous reaction?

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