Quiz 2 - Properties of Gases | Properties of Gases

At STP, one mole of an ideal gas occupies 22.4 L. Therefore, 2 moles will occupy 2×22.42 \times 22.42×22.4 L = 44.8 L.

Boyle's Law states that the pressure of a gas is inversely proportional to its volume when temperature is held constant (P ∝ ​).

Gases take the shape and volume of their container, meaning they have indefinite shape and indefinite volume.

The Kinetic Molecular Theory states that gas particles are in constant, random motion and that they have elastic collisions with each other and the walls of the container.

Use the Ideal Gas Law PV = nRT

P = $\frac{\mathrm{nRT}}{\mathrm{V}}$ = $\frac{0.5 \mathrm{mol} \times 0.0821 \mathrm{L}.\mathrm{atm}.{\mathrm{K}}^{-1}.{\mathrm{mol}}^{-1} \times 300 \mathrm{K}}{10 \mathrm{L}}$ = 1.23 atm

According to Dalton's Law of Partial Pressures, the total pressure is the sum of the partial pressures of all gases:
P_total = P_N2 + P_O2 + P_Ar = 500 torr + 200 torr + 100 torr = 800 torr

According to Graham's Law of Effusion, the rate of effusion is inversely proportional to the square root of the molar mass:

$\frac{{\mathrm{rate}}_{\mathrm{He}}}{{\mathrm{rate}}_{{\mathrm{N}}_2}}$ = $\sqrt{\frac{{\mathrm{M}}_{{\mathrm{N}}_2}}{{\mathrm{M}}_{\mathrm{He}}}}$ = 

The mole fraction is calculated as:

X_N2 = $\frac{\mathrm{moles} \mathrm{of} {\mathrm{N}}_2}{\mathrm{total} \mathrm{moles}}$ = $\frac{2}{2 + 3}$ =0.4

Ammonia has strong intermolecular hydrogen bonding, causing it to deviate more from ideal behavior compared to the other gases listed.

According to Boyle's Law (P₁V₁ = P₂V₂​), if the volume is halved, the pressure will double:

P₂ = $\frac{{\mathrm{P}}_1{\mathrm{V}}_1}{{\mathrm{V}}_2}$ = $\frac{1.0 \mathrm{atm} \times 4.0 \mathrm{L}}{2.0 \mathrm{L}}$ = 2.0 atm