A 1.37 L vessel contains He at a temperature of 24.5°C and a pressure of 205 mmHg. A 721 mL vessel contains Ne at a temperature of 36.2°C and a pressure of 0.185 atm. Both of these gases are placed in a 2.00 L vessel at 302 K. What is the final pressure (in atm) in the 2.00 L vessel?

Question

Quizplus · Accepted Answer

The correct answer is A because the total pressure in the final vessel is the sum of the partial pressures of He and Ne. The partial pressure of He is (205 mmHg / 760 mmHg/atm) * (1.37 L / 2.00 L) * (302 K / 297 K) = 0.187 atm. The partial pressure of Ne is (0.185 atm) * (721 mL / 2.00 L) * (302 K / 309 K) = 0.063 atm. The total pressure is 0.187 atm + 0.063 atm = 0.250 atm.

A 137 L Vessel Contains He at a Temperature of 24