Question

what is the mole fraction and partial pressure of ch₄ in a sample of gas that contains 1.25 moles of co₂, 1.49 moles of ch₄, and 3.31 moles of he, in which the total pressure is 5.78 atm?
x = select
pch₄ = select atm

Explanation:

Step1: Calculate total moles

Total moles \( n_{total} = n_{CO_2} + n_{CH_4} + n_{He} = 1.25 + 1.49 + 3.31 = 6.05 \) moles.

Step2: Calculate mole fraction of \( CH_4 \)

Mole fraction \( \chi_{CH_4} = \frac{n_{CH_4}}{n_{total}} = \frac{1.49}{6.05} \approx 0.246 \).

Step3: Calculate partial pressure of \( CH_4 \)

Partial pressure \( p_{CH_4} = \chi_{CH_4} \times P_{total} = 0.246 \times 5.78 \approx 1.422 \) atm.

Answer:

Mole fraction of \( CH_4 \) is approximately \( 0.246 \), partial pressure of \( CH_4 \) is approximately \( 1.42 \) atm (rounded to two decimal places).