A diatomic ideal gas undergoes a thermodynamic process in which its molar heat capacity is $C = \frac{3R}{2}$. Which of the following processes could this represent?

Value of two principle specific heats of a gas in cal ${\left( {{\rm{mol K}}} \right)^{ - 1}}$ determined bt different students are given. Which is most reliable?

One mole of an ideal monatomic gas undergoes a reversible process described by $PV^2 = ext{constant}$. The molar heat capacity of the gas during this process is:

One mole of an ideal gas expands adiabatically from an initial temperature ${T_1}$to a final temperature ${T_2}$.The work done by the gas would be

If for hydrogen ${C_p} - {C_v} =$ $m$ and for the nitrogen ${C_p} - {C_v} =$ $n$, where ${C_p},{C_v}$ refer to specific heats per unit mass respectively at constant pressure and constant volume, the relation between $m$ and $n$ is

A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is gain reduced to half. Then:

A container having 1 mole of a gas at a temperature ${27^0}C$ has a movable piston which maintains at constant pressure in container of 1 atm. The gas is compressed until temperature becomes ${127^0}C$. The work done is ( C for gas is 7.03 cal / mol – K)

Calculate change in internal energy when 5 mole of hydrogen is heated to ${20^ \circ }C$from ${10^ \circ }C$, specific heat of hydrogen at constant pressure is 8 cal ${\left( {{\rm{mol^\circ C}}} \right)^{ - 1}}$

Boyle’s law holds for an ideal gas during

A gas expands under constant pressure P from volume ${V_1}$ to ${V_2}$. The work done by the gas is

An ideal gas undergoes a cyclic process as shown in the $P-V$ diagram. The work done by the gas in the complete cycle is: