The density of oxygen gas at $5 \text{ atm}$ and $127^{\circ} C$ will be (in $\text{ g/L}$)

$A$ 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 $25 \, torr$.)

In order to increase the volume of a gas by $10 \%$,the pressure of the gas should be

$n$ moles of an ideal gas at temperature $T$ (in kelvin) occupy $V \ L$ of volume,exerting a pressure of $P$ atmospheres. What is the concentration (in $mol / L$)?

$A$ monoatomic ideal gas,initially at temperature $T_1$,is enclosed in a cylinder fitted with a frictionless piston. The gas is allowed to expand adiabatically to a temperature $T_2$ by releasing the piston suddenly. $L_1$ and $L_2$ are the lengths of the gas columns before and after the expansion,respectively. The ratio $\frac{T_2}{T_1}$ is:

$A$ $5.75 \ g$ sample of a gas occupies $3.5 \ L$ at $55 \ ^oC$ and $0.940 \ atm$ pressure. What is the molecular weight of the gas?