Calculate the density of $CO_2$ at $100\, ^oC$ and $800\, mm\, Hg$ of pressure in $g/L$.

Find the pressure of a $CO_2$ gas when $6.022 \times 10^{22}$ molecules are placed in a $2 \ L$ vessel at $27 \ ^oC$ temperature. (in $bar$)

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

At constant pressure,the temperature of $20 \ L$ of helium gas is increased from $100 \ K$ to $300 \ K$. What will be the change in volume in $L$?

$A$ $10.0 \, L$ flask contains $64 \, g$ of oxygen at $27^{\circ} C$. (Assume $O_2$ gas is behaving ideally). The pressure inside the flask in bar is $.....$
(Given $R = 0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$)

For an ideal gas,the volume-temperature graph at constant mass is shown below. What is the correct order of pressure?