posted by Anonymous
A 19.3L expandible container is filled in a room where the pressure is 761mmHg. It is filled with 600.4mmHg nitrogen, 108mmHg oxygen, 32.1 mmHg water vapor. The rest of the pressure is made up by carbon dioxide. The temperature is 20.3°C
a. What is the partial pressure of carbon dioxide?
b. What is the mass of carbon dioxide?
c. If this container is connected to a sealed 24.0L container that is filled with 761 mmHg of Ne (T = 20.3°) and opened, what is the total pressure inside the combined container and the partial pressure of Ne?
i think A is 20.5mmhg and B is .951 g CO2 are these right and im not sure how to start C
A is right. B is right.
I would calculate n for each of the gases. You know partial pressure of each, V, R, & T from the first container.
Mols Ne can be calculated from P Ne, V of the second container, R & T.
Find total mols, use that with R, & T and total volume to find total pressure when the two containers are connected.
Partial pressure Ne from the combined containers is pNe = XNe*Ptotal. (XNe = mols Ne/total mols)
thank you very much