An evacuated glass vessel weighs $40.0 \ g$ when empty,$135.0 \ g$ when filled with a liquid of density $0.95 \ g \ mL^{-1}$ and $40.5 \ g$ when filled with an ideal gas at $0.82 \ atm$ at $250 \ K$. The molar mass of the gas in $g \ mol^{-1}$ is .... .
(Given : $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$ )

The density of a gas $A$ is three times that of a gas $B$. If the molecular mass of $A$ is $M$,the molecular mass of $B$ is:

If $N_2$ gas is compressed at $2 \text{ atm}$ from $9.0 \text{ L}$ to $3.0 \text{ L}$ at $300 \text{ K}$, find the final pressure at the same temperature. (in $\text{ atm}$)

What is the effect of temperature change on the Boyle's law isotherm graph?

If $P$,$V$,$M$,$T$ and $R$ are pressure,volume,molar mass,temperature and gas constant respectively,then for an ideal gas,the density is given by

Starting out on a trip into the mountains,you inflate the tires on your automobile to a recommended pressure of $3.21 \times 10^5 \ Pa$ on a day when the temperature is $-5.0 \ ^\circ C$. You drive to the beach,where the temperature is $28 \ ^\circ C$. Assume that the volume increased by $3 \%$. What is the final pressure in the tires?