Calculate the volume of $6.022 \times 10^{21}$ molecules of $CO_2$ at $300 \ K$ temperature and $2 \ bar$ pressure. $[R = 8.314 \times 10^{-2} \ bar \ L \ K^{-1} \ mol^{-1}]$ (in $mL$)

What will be the effect on the density of $0.09 \ mol$ of a gas at $300 \ K$ if its pressure is increased?

The volume of $1 \ g$ of methane $(CH_4)$,ethane $(C_2H_6)$,propane $(C_3H_8)$,and butane $(C_4H_{10})$ is measured at $350 \ K$ and $1 \ atm$ pressure. What will be the volume of butane in $cm^3$?

$A$ vessel contains $1.6 \ g$ of dioxygen at $STP$ ($273.15 \ K$,$1 \ atm$ pressure). The gas is now transferred to another vessel at constant temperature,where pressure becomes half of the original pressure. Calculate
$(A)$ volume of the new vessel.
$(B)$ number of molecules of dioxygen.

The density of Neon will be highest at

Derive the relation between the density of gases and their molecular mass using Avogadro's law.