When the applied pressure is $16 \ atm$,the temperature is $27 \ ^oC$,and the volume is $9 \ L$,what will be the weight of $CH_4$ gas in $gm$? (Given $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$)

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

On a ship sailing in the Pacific Ocean where the temperature is $23.4^{\circ} C$,a balloon is filled with $2 \ L$ of air. What will be the volume of the balloon when the ship reaches the Indian Ocean,where the temperature is $26.1^{\circ} C$ (in $L$)?

For a fixed amount of gas at constant pressure,provide the plot of volume $(V)$ versus temperature $(T)$ in Kelvin. What does it represent?

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?

In the gas equation $PV = nRT$,the universal gas constant $R$ depends on: