The equation of state for $2 \ g$ of oxygen at a pressure $P$ and temperature $T$,when occupying a volume $V$,will be:

$A$ metre-long narrow bore held horizontally (and closed at one end) contains a $76 \; cm$ long mercury thread,which traps a $15 \; cm$ column of air. What happens if the tube is held vertically with the open end at the bottom?

An open glass tube is immersed in mercury such that a length of $8 \ cm$ extends above the mercury level. The open end of the tube is then closed and sealed,and the tube is raised vertically by an additional $46 \ cm$. What will be the length of the air column above the mercury in the tube now? (Atmospheric pressure = $76 \ cm$ of $Hg$)

$4$ moles of an ideal gas is at $0^\circ C$. At constant pressure,it is heated to double its volume. Its final temperature will be ...... $^\circ C$.

The temperature of a gas at $-173^{\circ} C$ is $1 \text{ atm}$ at constant volume. Up to what temperature should the gas be heated so that the pressure becomes $2 \text{ atm}$ (in $^{\circ} C$)?

An ideal gas at temperature $T$,pressure $p$ occupies a volume $V$. If its temperature is halved and pressure doubled,what is its new volume?