The following graph illustrates:

What is the volume of a gas at $1.032 \times 10^5 \ Nm^{-2}$ if it occupies $1 \ dm^3$ of volume at normal temperature and pressure (in $dm^3$)?

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

Find the pressure of neon gas having density $0.9 \ g \ L^{-1}$ at $350 \ K$ temperature. $(R = 8.34 \times 10^{-2} \ bar \ L \ K^{-1} \ mol^{-1})$ (in $bar$)

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):

$A$ vessel contains $3.2 \ g$ of dioxygen gas at $STP$ ($273.15 \ K$ and $1 \ atm$ pressure). The gas is now transferred to another vessel at constant temperature,where pressure becomes one third of the original pressure. The volume of the new vessel in $L$ is $........$ (Given: molar volume at $STP$ is $22.4 \ L$)