At $300 \ K$,$22 \ g$ of $CO_2$ gas exerts a pressure of $5 \ atm$. What is the volume of the gas at the same temperature (in $dm^3$)? $(R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1})$

$A$ flask of $1 \ L$ capacity is heated from $25 \ ^oC$ to $35 \ ^oC$. What volume of air (in $mL$) will be expelled from the flask?

$A$ $10 \, L$ cylinder contains $0.4 \, g$ of helium,$1.6 \, g$ of oxygen,and $1.4 \, g$ of nitrogen at $27 \, ^\circ C$. Calculate the total pressure of the mixture and the partial pressure of helium gas. Assume ideal gas behavior. $(R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1})$

Calculate the volume occupied by $8.8 \,g$ of $CO_{2}$ at $31.1^{\circ} C$ and $1 \,bar$ pressure.
( $R=0.083 \,bar \,L \,K^{-1} \,mol^{-1}$ )

At what temperature in $^\circ C$ will the volume of a gas become double its volume at $0\,^\circ C$?

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?