The density of oxygen at $STP$ is $1.43 \, g \, L^{-1}$. What will be its density at $27 \, ^\circ C$ temperature and $700 \, torr$ pressure?

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?

At $27\,^{\circ}C$ temperature and $4\, bar$ pressure,$CO_2$ is filled in a $2\, L$ vessel. Find the pressure if it is filled in a $4\, L$ vessel at $77\,^{\circ}C$ temperature. (in $, bar$)

What is the density of one mole of $He$ (molar mass $= 4 \ g \ mol^{-1}$) at $300 \ K$ and a pressure of $0.82 \ atm$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$

At constant temperature, a gas occupies a volume of $200 \text{ mL}$ at a pressure of $500 \text{ mm Hg}$. What will be its volume at $800 \text{ mm Hg}$ pressure (in $\text{ mL}$)?

If $P$,$V$,and $T$ represent the pressure,volume,and temperature of a gas respectively,which is the correct representation of Boyle's Law?