$A$ closed vessel contains $8\,g$ of oxygen and $7\,g$ of nitrogen. The total pressure is $10\,atm$ at the given temperature. If all the oxygen is removed from the system without permitting any change in temperature,then the pressure will become (in atmosphere):

For an ideal gas with pressure $P$,temperature $T$,and volume $V$,where the mass of each molecule is $m$,what is the density of the gas? ($k$ is the Boltzmann constant)

For a perfect gas,two pressures $P_{1}$ and $P_{2}$ are shown in the figure. The graph shows:

An insulated cylinder of volume $60\,cm^{3}$ is filled with a gas at $27^{\circ}C$ and $2$ atmospheric pressure. Then the gas is compressed making the final volume $20\,cm^{3}$ while allowing the temperature to rise to $77^{\circ}C$. The final pressure is . . . . . . atmospheric pressure.

$A$ gas at $27^\circ C$ temperature and $30$ atmospheric pressure is allowed to expand to atmospheric pressure. If the volume becomes $10$ times its initial volume,then the final temperature becomes ...... $^\circ C$.

Two spheres are connected to each other as shown in the figure. The volume of sphere $I$ is twice the volume of sphere $II$. They contain an ideal gas at temperatures $100 K$ and $200 K$,respectively. If the mass of the gas in sphere $I$ is $m$,what is the mass of the gas in sphere $II$?