At a temperature of $300 \ K$,if the pressure of $0.09 \ mol$ of a gas is halved,what will be its volume?

An ideal gas at constant temperature and pressure expands,then its

At a given temperature,the density of gas $x$ is twice the density of gas $y$. If the molar mass of $y$ is three times the molar mass of $x$,find the ratio of their pressures $(P_x/P_y)$.

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 $, g/L$)

What will be the molar volume of nitrogen $(N_2)$ and argon $(Ar)$ at $273.15 \ K$ and $1 \ atm$?

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?