A gaseous mixture at a total pressure of 1.50 atm contains equal molar amounts of He, Ne, and Ar. At constant temperature CO₂ gas is added to the mixture until the total pressure is 3.00 atm. Which of the following is a correct statement concerning partial pressures after the CO₂ addition? A) The partial pressure of Ar has doubled. B) The partial pressure of CO₂ is three times that of Ne. C) All four gases have equal partial pressures. D) More than one correct response. E) No correct response.

Question

Quizplus · Accepted Answer

The initial partial pressure of each gas (He, Ne, Ar) is 0.50 atm (since they are in equal molar amounts and total pressure is 1.50 atm). When CO2 is added to double the total pressure to 3.00 atm, the partial pressures of He, Ne, and Ar remain 0.50 atm each, and the partial pressure of CO2 is 1.50 atm. Thus, the partial pressure of CO2 is three times that of Ne (0.50 atm).

A Gaseous Mixture at a Total Pressure of 1