When an ideal gas undergoes unrestrained expansion,no cooling occurs because the molecules

Calculate the total pressure in a mixture of $8 \,g$ of dioxygen and $4 \,g$ of dihydrogen confined in a vessel of $1 \,dm^{3}$ at $27^{\circ} C$. $(R = 0.083 \,bar \,dm^{3} \,K^{-1} \,mol^{-1})$

The density of a gas $A$ is three times that of a gas $B$. If the molecular mass of $A$ is $M$,the molecular mass of $B$ is:

The compressibility factor for an ideal gas is

$A$ $10 \, L$ cylinder contains $0.4 \, g$ of helium,$1.6 \, g$ of oxygen,and $1.4 \, g$ of nitrogen at $27 \, ^\circ C$. Calculate the total pressure of the mixture and the partial pressure of helium gas. Assume ideal gas behavior. $(R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1})$

The graph of $V$ versus $T$ for an ideal gas at constant pressures $P_1$ and $P_2$ is shown below. Which of the following is correct?