The volume occupied by $1.8 \; g$ of water vapour at $374^{\circ} C$ and $1 \; bar$ pressure will be $....... \; L$ : [Use $R=0.083 \; bar \; L \; K^{-1} \; mol^{-1}$]

Calculate the pressure of $HCl$ gas having a density of $8 \, kg \, m^{-3}$ at a temperature of $-40 \, ^oC$. (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$,Molar mass of $HCl = 36.5 \, g \, mol^{-1} = 0.0365 \, kg \, mol^{-1}$)

$A$ gas obeys Charles's law in the temperature range $0-500 \ K$ at a given pressure. Its volume changes to zero at a temperature of:

Calculate the temperature of $4.0 \, mol$ of a gas occupying $5 \, dm^{3}$ at $3.32 \, bar$.
$(R = 0.083 \, bar \, dm^{3} \, K^{-1} \, mol^{-1})$

When $48 \, L$ of dry $N_2$ gas is passed through $36 \, g$ of $H_2O$ at $27 \, ^oC$,the weight of water decreases by $1.20 \, g$. What is the vapor pressure of water in $atm$?

Calculate the number of moles of the gas having volume $2.5 \ L$ at $300 \ K$ and $4.5 \ atm$? $(R=0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1})$