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?

Two moles of ideal helium gas are in a rubber balloon at ${30^ \circ }C$. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to ${35^ \circ }C$. The amount of heat required in raising the temperature is nearly (take $R = 8.31J/mol.K$)

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 ${\left( {{\rm{mol^\circ C}}} \right)^{ - 1}}$

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)

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

One mole of an ideal gas requires 207 J heat to raise the temperature by 1K, when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same range, the heat required will be ($R = 8.3{\rm{Jmo}}{{\rm{l}}^{ - 1}}{{\rm{K}}^{ - 1}})$)

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

For a gas, the difference between the two principle specific heats is 4150 ${\rm{Jk}}{{\rm{g}}^{ - 1}}{{\rm{K}}^{ - 1}}$.What is the specific heat of the gas at constant volume if the ratio of specific heat is 1.4?

One mole of an ideal monoatomic gas is heated at a constant pressure of 1 atm from ${0^ \circ }C$ to ${100^ \circ }C$. Work done by the gas is