Which of the following equations does $NOT$ represent Charles's law for a given mass of gas at constant pressure?

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

The pressure exerted by a non-reactive gaseous mixture of $6.4 \ g$ of methane and $8.8 \ g$ of carbon dioxide in a $10 \ L$ vessel at $27^{\circ} C$ is .............$kPa$.
(Round off to the Nearest Integer).
[Assume gases are ideal,$R = 8.314 \ J \ mol^{-1} K^{-1}$
Atomic masses $: C = 12.0 \ u, H = 1.0 \ u, O = 16.0 \ u]$

$A$ vessel of volume $24.6 \ L$ contains $1.5 \ moles$ of $H_2$ and $2.5 \ moles$ of $N_2$ at $300 \ K$. Calculate the partial pressure of $N_2$ in the vessel. (in $atm$)

Which one of the following is the correct $PV$ vs $P$ plot at constant temperature for an ideal gas? ($P$ and $V$ stand for pressure and volume of the gas respectively)

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of $1 \, atm$ but also a concentration of $1 \, mol \, L^{-1}$ $(R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1})$?