Question

A mixture of gases consists of 4.00 moles of He, 2.00 moles of H2, 3.00 moles of CO2 and 5.00 moles of Ar. The total pressure of the mixture is 2900 mm. Determine the mole fraction of each gas in the mixture. Determine the mole percent of each gas in the mixture. Determine the partial pressure of each gas in the mixture.

Answer 1

Answer on Question 84125 in General Chemistry

.n (He) = 4 moles

.n (H₂) = 2 moles

.n (CO₂) = 3 moles

.n (Ar) = 5 moles

.p (total) = 29000 mm

.φ (gas) = ?

.φ (gas %) = ?

.p (gas) = ?

Determine the mole fraction of each gas

.φ (He) = $\frac{n(He)}{n(He) + n(H_2) + n(CO_2) + n(Ar)} = \frac{4}{4 + 2 + 3 + 5} = 0.29$

.φ (He %) = 0.29 × 100% = 29%

.φ (H₂) = $\frac{n(H_2)}{n(He) + n(H_2) + n(CO_2) + n(Ar)} = \frac{2}{4 + 2 + 3 + 5} = 0.14$

.φ (H₂ %) = 0.14 × 100 = 14%

.φ (CO₂) = $\frac{n(CO_2)}{n(He) + n(H_2) + n(CO_2) + n(Ar)} = \frac{3}{4 + 2 + 3 + 5} = 0.21$

.φ (CO₂ %) = 0.21 × 100% = 21%

.φ (Ar) = $\frac{n(Ar)}{n(He) + n(H_2) + n(CO_2) + n(Ar)} = \frac{5}{4 + 2 + 3 + 5} = 0.36$

.φ (Ar %) = 0.36 × 100% = 36%

Determine the partial pressure of each gas in the mixture.

.p (He) = p(total) × φ(He) = 29000 × 0.29 = 8410 mm

.p (H₂) = p(total) × φ(H₂) = 29000 × 0.14 = 4060 mm

.p (CO₂) = p(total) × φ(CO₂) = 29000 × 0.21 = 6090 mm

.p (Ar) = p(total) × φ(Ar) = 29000 × 0.36 = 10440 mm

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