Density of a gas is found to be $5.46 \, g / dm^3$ at $27^{\circ} C$ at $2 \, bar$ pressure. What will be density at $STP$?

In the equation $PV = nRT$,the number of moles per liter can be expressed as:

For an ideal gas,what is the nature of the $pV$ versus $p$ graph at a constant temperature?

An $LPG$ (Liquefied Petroleum Gas) cylinder weighs $15.0 \ kg$ when empty. When full, it weighs $30.0 \ kg$ and shows a pressure of $3.0 \ atm$. In the course of usage at $27^{\circ}C$, the mass of the full cylinder is reduced to $24.2 \ kg$. The volume of the used gas in cubic metre at the normal usage condition ($1 \ atm$ and $27^{\circ}C$) is (assume $LPG$ to be normal butane and it behaves ideally). (in $m^3$)

At $27\,^{\circ}C$ and $1\,atm$ pressure,the density of a gas is $d$. At what temperature will its density become $0.75d$ if the pressure is kept constant?

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 $, bar$)