The amount of heat required to raise the temperature of $2$ moles of helium gas from $0^{\circ}C$ to $100^{\circ}C$ at constant volume and constant pressure,respectively,is:

The specific heat capacities of an ideal gas at constant pressure and at constant volume are $620 \ J \ kg^{-1} \ K^{-1}$ and $420 \ J \ kg^{-1} \ K^{-1}$ respectively. The density of the gas at $STP$ is approximately, (in $kg \ m^{-3}$)

What is the relationship between the internal energy $U$ of an ideal gas and its pressure $P$ and volume $V$?

For a gas if $\gamma = 1.4$,then atomicity,${C_p}$ and ${C_v}$ of the gas are respectively

The specific heat of Argon at constant volume is $0.075 \ kcal/kg \ K$. The value of its atomic weight is..... [$R = 2 \ cal/mol \ K$]

To raise the temperature of a certain mass of gas by $50^{\circ} C$ at a constant pressure,$160$ calories of heat is required. When the same mass of gas is cooled by $100^{\circ} C$ at constant volume,$240$ calories of heat is released. How many degrees of freedom does each molecule of this gas have (assume gas to be ideal)?