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 $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$)

When $2 \ g$ of a gaseous substance $A$ is introduced into an initially evacuated flask at $25^{\circ} C$,the pressure is found to be $1 \ atm$. $3 \ g$ of another gaseous substance $B$ is added to it at the same temperature and pressure. The final pressure is found to be $1.5 \ atm$. Assuming ideal gas behaviour,the ratio of molar masses of $A$ and $B$ is:

To an evacuated vessel with a movable piston under an external pressure of $1 \ atm$,$0.1 \ mol$ of $He$ and $1.0 \ mol$ of an unknown compound (vapour pressure $0.68 \ atm$ at $0^{\circ} C$) are introduced. Considering ideal gas behaviour,the total volume (in litres) of the gases at $0^{\circ} C$ is close to:

For an ideal gas,the $V$ vs $T$ plot at constant pressures $P_1$ and $P_2$ is shown in the figure. Which of the following is correct?

At $27^{\circ} C$,$1 \ L$ of $H_2$ with a pressure of $1 \ bar$ is mixed with $2 \ L$ of $O_2$ with a pressure of $2 \ bar$ in a $10 \ L$ flask. What is the pressure exerted by the gaseous mixture in $bar$? (Assume $H_2$ and $O_2$ as ideal gases)

$A$ plot of volume $(V)$ of the gas versus temperature ($T$ in $K$) is shown below. Which of the following options is correct for the plot?