Homework Help: Two beakers with volatile solvents in closed system

1. Aug 14, 2008

black_squirrel

1. The problem statement, all variables and given/known data
Beaker A contains a volatile solvent and beaker B contains 10% solution of a non-volatile solute in the same solvent. Both beakers are placed in a closed environment as shown. The question asks what will happen when the system has reached equilibrium. The answer is given that all the solvent will be in beaker B after equilibrium because beaker B will have lower vapor pressure than beaker A. I don't understand why this is true. Isnt this against thermodynamics? isn't entropy decreasing here if that was the case?

http://pics-hosting.com/files/w4zv6fuoasz6vxth3y7.jpg [Broken]

Last edited by a moderator: May 3, 2017
2. Aug 15, 2008

black_squirrel

anyone?

3. Aug 15, 2008

LowlyPion

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Perhaps this link can help you understand the vapor pressure lowering aspect of the solute on the solvent?
http://en.wikipedia.org/wiki/Raoult's_law

Given that the vapor pressure would be lowered with the solute, are you on board with understanding that the liquid on the left would have a greater tendency toward evaporation than the one on the right?

In which case what do you think happens when the pressure of a gas at the surface of a liquid is greater than the vapor pressure of the liquid itself at that temperature and pressure?

http://en.wikipedia.org/wiki/Colligative_properties

Last edited by a moderator: May 3, 2017