An ideal gas occupies a volume of $2\, m^3$ at a pressure of $3\times10^6\, Pa$. The energy of the gas is

At $27^{\circ}C$ temperature,the kinetic energy of an ideal gas is $E_1$. If the temperature is increased to $327^{\circ}C$,then the kinetic energy would be:

The average kinetic energy of a monatomic molecule is $0.414 eV$ at temperature : (Use $K_{B} = 1.38 \times 10^{-23} J/K$) (in $K$)

An ideal gas in a container of volume $500 \text{ c.c.}$ is at a pressure of $2 \times 10^5 \text{ N/m}^2$. The average kinetic energy of each molecule is $6 \times 10^{-21} \text{ J}$. The number of gas molecules in the container is:

On the basis of the kinetic theory of gases,the mean kinetic energy $(K.E.)$ of $1\, mole$ per degree of freedom is:

If $E$ is the kinetic energy per mole of an ideal gas and $T$ is the absolute temperature,then the universal gas constant is given as