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

At a constant temperature,two different gases $G_1$ and $G_2$ are kept in separate flasks. The molar mass of $G_2$ is three times that of $G_1$,while the density of $G_1$ is two times that of $G_2$. What is the ratio of the pressure exerted by $G_2$ to that of $G_1$ in their respective flasks?

The correct value of the gas constant $R$ is close to

$A$ 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 value of the universal gas constant $R$ is:

An ideal gas expands isothermally and reversibly from $10 \ m^{3}$ to $20 \ m^{3}$ at $300 \ K$ performing $5.187 \ kJ$ of work on surroundings. Calculate the number of moles of gas undergoing expansion? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$