For an ideal gas,the number of moles per litre in terms of its pressure $P$,gas constant $R$,and temperature $T$ is:

At what pressure will a quantity of gas,which occupies $100 \ mL$ at a pressure of $720 \ mm$,occupy a volume of $84 \ mL$?

The volume of $2.8 \ g$ of $CO$ at $27^{\circ} C$ and $0.821 \ atm$ pressure is (Given: $R = 0.08210 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $L$)

$A$ bubble of air is underwater at temperature $15^\circ C$ and the pressure $1.5 \ bar$. If the bubble rises to the surface where the temperature is $25^\circ C$ and the pressure is $1.0 \ bar$,what will happen to the volume of the bubble?

The $log \, T$ vs $log \, V$ curve is plotted for an ideal gas as shown. Which of the following is true for the gas?

If $20 \ cm^3$ of gas at $1 \ atm$ is expanded to $50 \ cm^3$ at constant $T$,what is the final pressure?