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

$A$ gas of volume $100 \ cc$ is kept in a vessel at pressure $10^4 \ Pa$ maintained at temperature $24 \ ^oC$. If now the pressure is increased to $10^5 \ Pa$,keeping the temperature constant,then the volume of the gas becomes ............. $cc$.

An ideal gas on isothermal reversible compression from $10 \ L$ to $5 \ L$ performs $1730 \ J$ of work at $300 \ K$. Calculate the number of moles of gas involved in the compression? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

What is the temperature of $4$ moles of a gas occupying $5 \ L$ volume at $3.32 \ bar$ (in $K$)? $\left(R=0.083 \ bar \ L \ K^{-1} \ mol^{-1}\right)$

What is the density of one mole of $He$ (molar mass $= 4 \ g \ mol^{-1}$) at $300 \ K$ and a pressure of $0.82 \ atm$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$

Two closed bulbs of equal volume $V$ containing an ideal gas initially at pressure $P_i$ and temperature $T_1$ are connected through a narrow tube of negligible volume as shown in the figure below. The temperature of one of the bulbs is then raised to $T_2$. The final pressure $P_f$ is: