[SOLVED] Gases Problem Hi Everyone, I was wondering if someone can explain the following question: An apparatus consists of three temperature-jacketed 1.000 L bulbs connected by stopcocks. Bulb A contains a mixture of H2O (g), CO2 (g), and N2 (g) at 25'C and a total pressure of 564 mm Hg. Bulb B is empty and is held at a temperature of -70'C. Bulb C is also empty and is held at a temperature of -190'C. The stopcocks are closed, and the volume of the lines connecting the bulbs is zero. CO2 sublimes at -78'C and N2 boils at -196'C. A. The stopcock between A and B is opened, and the system is allowed to come to equilibrium. The pressure in A and B is now 219 mm Hg. what do bulbs A and B contain? The answer is: Bulb A contains CO2 (g) and N2 (g) Bulb B contains CO2 (g) and N2 (g) and H2O (s). But I have no idea how they got this. I understand that the H2O will become a solid in Bulb B since the temperature is -70'C, but why does the H2O (g) leave bulb A completely? C. Both stopcocks are opened and the system is again allowed to come to equilibrim. The pressure throughout the system is 33.5 mm Hg. What do bulbs A, B, and C contain? The answer is: Bulb A contains N2 (g) Bulb B contains N2 (g) and H2O (s) Bulb C contains N2 (g) and CO2 (s) I'm pretty sure that this question is similar to the previous one, but again, I don't understand why some gases completely leave one of the bulbs. Can someone help?