$A$ 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?

An open vessel at $27\,^oC$ is heated such that $\frac{3}{5}$ of the air in it is expelled. Assuming the volume of the vessel remains constant,calculate the temperature in $K$ to which the vessel was heated.

In a closed vessel,an ideal gas at $1 \, atm$ is heated from $27^{\circ} C$ to $327^{\circ} C$. The final pressure of the gas will approximately be $..... \, atm$

The isotherms of an ideal gas at $T_1, T_2, T_3$ along with their slopes $(m)$ are shown in the graph. If $T_1 > T_2 > T_3$,then the correct order of slopes of these isotherms is:

$A$ bubble is at the bottom of a lake of depth $h$. As the bubble rises to the surface,its radius increases by a factor of $3$. If the atmospheric pressure is equal to the pressure exerted by a water column of height $\ell$,then $h$ is equal to:

If the density of a gas at $27\,^{\circ}C$ and $2\, atm$ is $5.46\, g/L$,then calculate the density of the gas at $STP$. (in $, g/L$)