The density of oxygen gas at $1.0 \, atm$ pressure and $27 \, ^oC$ temperature is ............. $g/L$.

For $0.09 \, \text{mol}$ of $CO_2$ at $300 \, K$,the volume is $112.0 \times 10^{-3} \, m^3$ at a pressure of $2.0 \times 10^4 \, Pa$. What will be the volume at a pressure of $4.0 \times 10^4 \, Pa$?

The $\log \, T$ vs $\log \, V$ curve is plotted for an ideal gas as shown. Which of the following is true for the gas?

$3.4$ moles of an ideal gas occupies a volume of $68 \ mL$ at $300 \ K$. What would be the pressure of the gas? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

$A$ $100 \ L$ cylinder containing $H_2$ exerted a pressure of $4 \ atm$ at $300 \ K$. It was accidentally opened and some $H_2$ escaped. When it was closed,it exerted a pressure of $3 \ atm$ at $300 \ K$. The number of moles of $H_2$ remaining in the cylinder is equal to (Assume $H_2$ as an ideal gas; $R=$ gas constant)

Define the gas constant $R$ in terms of work.