$A$ sample of gas occupies $100 \ mL$ at $27 \ ^oC$ and $740 \ mm$ pressure. What will be the temperature of the gas in $^oC$ if its volume is changed to $80 \ mL$ at $740 \ mm$ pressure?

The equation for Boyle's law is:

$A$ $100 \ L$ cylinder containing $H_2$ exerted a pressure of $4 \ atm$ at $300 \ K$. It was accidentally opened and some $H_2$ escaped. When it was closed,it exerted a pressure of $3 \ atm$ at $300 \ K$. The number of moles of $H_2$ remaining in the cylinder is equal to (Assume $H_2$ as an ideal gas; $R=$ gas constant)

What is the density of $N_2$ gas at $227\,^\circ C$ and $5.00\ atm$ pressure? (Given: $R = 0.082\ L\ atm\ K^{-1}\ mol^{-1}$)

Two vessels are filled with ideal gases $A$ and $B$ and are connected through a pipe of zero volume as shown in the figure. The stop cock is opened and the gases are allowed to mix homogeneously and the temperature is kept constant. The partial pressures of $A$ and $B$ respectively (in $atm$) are:

Volume of $0.5 \ mole$ of a gas at $1 \ atm$ pressure and $273 \ K$ is ............. $litres$.