$A$ $10.0 \, L$ flask contains $64 \, g$ of oxygen at $27^{\circ} C$. (Assume $O_2$ gas is behaving ideally). The pressure inside the flask in bar is $.....$
(Given $R = 0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$)

At constant temperature, a gas occupies a volume of $200 \text{ mL}$ at a pressure of $500 \text{ mm Hg}$. What will be its volume at $800 \text{ mm Hg}$ pressure (in $\text{ mL}$)?

By what other name is the ideal gas equation known? Why?

If two identical containers $X$ and $Y$ containing $O_2$ gas are subjected to expansion from volume $V$ to $2V$ under identical isothermal conditions by applying pressure changes of $\Delta P$ and $0.2 \Delta P$ respectively,then the ratio of the mass of $O_2$ gas in container $X$ to container $Y$ is

The volume of a gas is $4 \ dm^3$ at $0^{\circ} C$. Calculate the new volume at constant pressure when the temperature is increased by $10^{\circ} C$. (in $dm^3$)

At a given temperature,the density of gas $x$ is twice that of gas $y$. The molar mass of $x$ is one-third of the molar mass of $y$. What is the ratio of their pressures $(P_x / P_y)$?