The pressure $P$,volume $V$,and temperature $T$ of a gas in jar $A$ are given. Another gas in jar $B$ has pressure $2P$,volume $V/4$,and temperature $2T$. The ratio of the number of molecules in jar $A$ to jar $B$ is:

If the volume of a given mass of a gas is increased four times,and the temperature is raised from $27^{\circ}C$ to $127^{\circ}C$,what happens to its elasticity?

From the following $P-T$ graph,what inference can be drawn?

$A$ 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):

What is the nature of the $P$ versus $1/V$ graph at a constant temperature?

$10 \ g$ of a gas at $STP$ occupies a volume of $2 \ L$. At what temperature will the volume be doubled,if pressure and amount of the gas remain constant?