$22 \, g$ of dry ice is placed in a $600 \, mL$ empty container at $25 \, ^\circ C$ and sealed tightly. If all the $CO_2$ evaporates,what will be the final pressure inside the container in $atm$?

What is the temperature of $4$ moles of a gas occupying $5 \ L$ volume at $3.32 \ bar$ (in $K$)? $\left(R=0.083 \ bar \ L \ K^{-1} \ mol^{-1}\right)$

Which of the following equations does $NOT$ represent Charles's law for a given mass of gas at constant pressure?

$2 \times 10^6$ molecules of $N_2$ gas enter into a vessel having a volume of $400 \, mL$ at $400 \, K$ temperature. Find the pressure in $atm$ and $bar$. $[R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}]$,$[1 \, atm = 1.013 \, bar]$

$A$ dry gas occupies $136.5 \, cm^3$ at $STP$. If the same mass of gas is collected over water at $27 \, ^oC$ and a total pressure of $725 \, torr$,what volume will it occupy in $cm^3$? (Vapour pressure of water at $27 \, ^oC$ is $25 \, torr$.)

The temperature of a flask is increased from $27\,^{\circ}C$ to $277\,^{\circ}C$. If $0.1\,dm^{3}$ of gas bubbles out from the flask at $277\,^{\circ}C$,calculate the volume of the flask. (in $,dm^{3}$)