Question

The picture below shows two bulbs connected by a stopcock. The 6.00-L bulb contains nitric oxide at a pressure of 0.400 atm, and the 1.50-L bulb contains oxygen at a pressure of 2.50 atm. After the stopcock is opened, the gases mix and react: Determine which gases remain after the reaction goes to completion and calculate their partial pressures. The temperature at the beginnning and the end of the experiment is 22 °C. Which gases are present at the end of the experiment? What are the partial pressures of the gases? If the gas was consumed completely, put 0 for the answer.

Answer 1

Calculating the number of moles of Nitric Oxide

Calculating the number of moles of Oxygen

                     

Initial             0.099           0.1548

Final                0               0.1053             0.099

Gases present in the mixture are NO2 and O2

All of the NO is consumed in the reaction

Pressure of the Container = (P1V1 + P2V2)/(V1+V2) = (6 * 0.4 + 2.5 * 1.50)/7.50

=> 0.82 atm

Partial Pressure of O2 = 0.1053/(0.1053+0.099) * 0.82 = 0.4226 atm

Partial Pressure of NO2 = 0.82 - 0.4226 = 0.397 atm