At $1 \text{ atm}$ pressure and $0 \, ^oC$,a certain mass of a gas occupies $0.4 \, L$. Keeping the pressure constant,if the temperature is increased to $273 \, ^oC$,what will be its final volume (in $, L$)?

$A$ glass vessel weighs $50.0 \, g$ when empty. When filled with a liquid of density $0.98 \, g \cdot mL^{-1}$,it weighs $148.0 \, g$. When filled with an ideal gas at $760 \, mm$ of $Hg$ pressure and $300 \, K$ temperature,it weighs $50.5 \, g$. Calculate the molar mass of the gas in $u$.

For a fixed amount of gas at a constant temperature,which of the following is true?

The density of nitrogen monoxide $(NO)$ at $S.T.P.$ is ......... $g \ L^{-1}$.

What is the numerical value of gas constant $R$ in terms of $L \ atm \ K^{-1} \ mol^{-1}$?

$A$ gas has a volume of $3.4 \ L$ at $25^{\circ} C$. What is the final temperature if the volume increases to $10.2 \ L$ at constant pressure (in $K$)?