Ask Question
26 June, 18:25

The total pressure of a gas mixture in a particular container is 43.2 atm. The Flask contains 2.87 mol of argon, 7.40 mol of chlorine and 15.2 mol of xenon. Determine the partial pressure of each gas.

+4
Answers (1)
  1. 26 June, 20:32
    0
    The ideal gas equation shows that the number of gas moles present is directly proportional to the pressure exerted by the gas. Since the gas sample contains different elements consisting of different moles and the amounts are given in the problem, the mole fraction can be used to determine the partial pressure of each gas after careful rearrangement of the ideal gas equation. The total moles of the gas mixture is 25.47 moles, getting the mole fraction and multiplying it with the total gas pressure, the partial pressures of the following gases were determined: 4.867 atm for Argon, 12.551 atm for Chlorine, 25.781 atm for Xenon, respectively.
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “The total pressure of a gas mixture in a particular container is 43.2 atm. The Flask contains 2.87 mol of argon, 7.40 mol of chlorine and ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers