At $400 \ K$, an ideal gas is enclosed in a $0.5 \ m^3$ vessel at a pressure of $203 \ kPa$. What is the change in temperature required (in $K$), if it occupies a volume of $0.2 \ m^3$ under a pressure of $304 \ kPa$? (Nearest integer)

At $STP$,$2 \ mol$ of $N_2$ gas in a $50 \ L$ container exhibits:

To an evacuated vessel with a movable piston under an external pressure of $1 \ atm$,$0.1 \ mol$ of $He$ and $1.0 \ mol$ of an unknown compound (vapour pressure $0.68 \ atm$ at $0^{\circ} C$) are introduced. Considering ideal gas behaviour,the total volume (in litres) of the gases at $0^{\circ} C$ is close to:

If the volume of a gas is $V \ L$ at $P \ atm$ pressure and $27 \ ^oC$ temperature,what will be the volume of the gas at $-173 \ ^oC$ temperature and $P \ atm$ pressure if the amount of gas is doubled?

The density of a gas is equal to ...... ($P =$ pressure,$V =$ volume,$T =$ temperature,$R =$ gas constant,$n =$ number of moles,and $M_w =$ molecular weight):

The volume of a gas at $0^{\circ} C$ is $2 \ dm^3$. What is its volume if the temperature is decreased by $272^{\circ} C$?