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(1-11) Chemistry - Science (Dr. Bob222)

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Liquid chloroform (CHCl3) is placed in a closed container and allowed to equilibrate with chloroform vapor. With the temperature held constant, additional chloroform is introduced into the system, and the vapor-liquid equilibrium is reestablished. Following this, the chloroform vapor pressure will:

a) be higher
b) be lower
c) be the same if both liquid and vapor phases are present
d) be lower if the heat of vaporization is positive
e) be higher if the heat of vaporization is positive

The correct answer is C but I don't quite get it why so? Could you please explain? Thank you

  • (1-11) Chemistry - Science (Dr. Bob222) -

    Yes, the answer is C. Any liquid placed in a closed system will come to equilibrium with its vapor at a particular temperature. The vapor pressure then is say x. Adding more liquid will NOT make the liquid evaporate more which would, of course, increase the vapor. The vapor pressure is a function of the temperature. Those molecules with sufficient energy will be able to jump out of the liquid and that depends upon T. Increasing T will give them more energy and increase the vapor pressure but that's the only way to increase p. You may say "but increasing volume will give it more room to evaporate" and that is very true, however, more molecules will enter the vapor phase but when the vapor pressure reaches equilibrium it will be the SAME it was at the smaller volume

  • (1-11) Chemistry - Science (Dr. Bob222) -

    Will the Le Chatelier's principle work here? Because pure liquid has no effect on the equilibrium position, it will not move towards products; thus, chloroform vapor will not form.

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