At constant volume,the temperature of a gas is increased. Then:

An ideal gas is kept in a cylinder of volume $3 \,m^3$ at a pressure of $3 \times 10^5 \,Pa$. The energy of the gas is

The mean kinetic energy of the molecules of an ideal gas at $399^{\circ} C$ is $E$. The temperature at which the mean kinetic energy of its molecules will be $E/2$ is: (in $^{\circ} C$)

$A$ flask contains Hydrogen and Argon in the ratio $2:1$ by mass. The temperature of the mixture is $30^{\circ} C$. The ratio of average kinetic energy per molecule of the two gases $(K_{\text{argon}} / K_{\text{hydrogen}})$ is: (Given: Atomic weight of $Ar = 39.9$)

What is the kinetic energy of one gram mole of a gas at standard temperature and pressure? $(R = 8.31 \ J/mol \cdot K)$

Write the equation of pressure of an ideal gas in terms of its density.