A mixture of 1 mol of He and 1 mol of CO$_2$ is contained in a vessel of volume V at 20°C. If the mixture behaves ideally, what is the pressure exerted by He?

The pressure of gas having 2 mole in $44.8{\rm{litre}}$ vessel at $540{\rm{K}}$ is:

At constant temperature, the pressure of an ideal gas is doubled. What happens to its volume?

The temperature at which the second virial coefficient of a real gas is zero is called

$5\,{\rm{g}}$ each of the following gases at 87\,^\circ C and $750\,{\rm{mm}}$ pressure are taken. Which of them will have the least volume?

At a constant pressure, what should be the percentage increase in the temperature in Kelvin for a $10\%$ increase in volume?

A rigid container of volume 25.0 L contains 160 g of oxygen gas at $546.3\ K$. If the oxygen behaves ideally, determine the pressure inside the container in bar. (Given $R = 0.0831\ L\ bar\ K^{-1}\ mol^{-1}$)

The temperature of 20 L of nitrogen was increased from 10 K to 30 K at a constant pressure. Change in volume will be

380 mL of a gas at 27\,^\circ C , 800 mm of Hg weighs 0.455 g. The molecular weight of gas is

The density of ${N_2}$ gas at 0.821 atmospheric pressure and ${7^0}C$

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of 1 atm but also a concentration of $1{\rm{mol}}\,\,{\rm{litr}}{{\rm{e}}^{ - 1}}$ ? $(\;R = 0.082$ litre atm ${\rm{mo}}{{\rm{l}}^{ - 1}}{\deg ^{ - 1}})$