An ideal gas undergoes a reversible isothermal expansion from state I to state II followed by a reversible adiabatic expansion from state II to state III. The correct plot(s) representing the changes from state I to state III is (are)

(p : pressure, V : volume, T : temperature, H : enthalpy, S : entropy)

In thermodynamics, the p-V work done is given by

$$w = - \int {dV{p_{ext}}} $$

For a system undergoing a particular process, the work done is

$$w = - \int {dV\left( {{{RT} \over {V - b}} - {a \over {{V^2}}}} \right)} $$

This equation is applicable to a

Choose the reaction(s) from the following options, for which the standard enthalpy of reaction of equal to the standard enthalpy of formation.

Which of the following statement(s) is(are) correct regarding the root mean square speed (U_rms) and average translational kinetic energy (E_av) of a molecule in a gas at equilibrium?