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 15.2 mol of xenon. Determine the partial pressure of each gas.

Answer 1

The ideal gas equation shows that the number of gas molecules 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.

Answer 2

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.