a mixture of gases contains 3.85 moles of neon (ne), 0.92 moles of argon (ar), and 2.59 moles of xenon (xe)…

a mixture of gases contains 3.85 moles of neon (ne), 0.92 moles of argon (ar), and 2.59 moles of xenon (xe). calculate the partial pressure of the gases if the total pressure is 2.50 atm at a certain temperature.

a mixture of gases contains 3.85 moles of neon (ne), 0.92 moles of argon (ar), and 2.59 moles of xenon (xe). calculate the partial pressure of the gases if the total pressure is 2.50 atm at a certain temperature.

Answer

Explanation:

Step1: Calculate the total number of moles

The total number of moles (n_{total}) is the sum of the moles of each gas. [n_{total}=n_{Ne}+n_{Ar}+n_{Xe}] [n_{total}=3.85 + 0.92+2.59] [n_{total}=7.36\space mol]

Step2: Calculate the mole fraction of each gas

  • Mole fraction of (Ne) ((X_{Ne})): [X_{Ne}=\frac{n_{Ne}}{n_{total}}=\frac{3.85}{7.36}\approx0.523]
  • Mole fraction of (Ar) ((X_{Ar})): [X_{Ar}=\frac{n_{Ar}}{n_{total}}=\frac{0.92}{7.36}\approx0.125]
  • Mole fraction of (Xe) ((X_{Xe})): [X_{Xe}=\frac{n_{Xe}}{n_{total}}=\frac{2.59}{7.36}\approx0.352]

Step3: Calculate the partial pressure of each gas using Dalton's law (P_{i}=X_{i}\times P_{total})

  • Partial pressure of (Ne) ((P_{Ne})): [P_{Ne}=X_{Ne}\times P_{total}=0.523\times2.50 = 1.31\space atm]
  • Partial pressure of (Ar) ((P_{Ar})): [P_{Ar}=X_{Ar}\times P_{total}=0.125\times2.50=0.31\space atm]
  • Partial pressure of (Xe) ((P_{Xe})): [P_{Xe}=X_{Xe}\times P_{total}=0.352\times2.50 = 0.88\space atm]

Answer:

  • The partial pressure of (Ne) is (1.31\space atm)
  • The partial pressure of (Ar) is (0.31\space atm)
  • The partial pressure of (Xe) is (0.88\space atm)