chem quesition?

Question

16. What is the equilibrium partial pressure of water vapor above a mixture of 24.0 g H2O and 48.0 g CH3CH2OH at 25 °C. The partial pressure of pure water at 25.0 °C is 23.8 mm Hg. Assume ideal behavior for the solution.

a. 0.561 mm Hg
b. 7.93 mm Hg
c. 10.4 mm Hg
d. 11.9 mm Hg
e. 13.4 mm Hg

how do you get the answer?

Answer 1

Work out the mole fraction of water: moles H2O = 24/18 and moles ethanol = 48/46. Add up the total moles, and work out what fraction is water. Then simply multiply this by 23.8.

Answer 2

D. You find the mole fraction of water, you do that by dividing the number of grams in this mixture (24.0) by the gram weight of H2O (18.0) and do the same with...that, (I dont feel like figuring out its name) then the formula is simply

Mols of H2O / Mols of H2O + Mols of the other substance.

Now take that number and multiply it by 23.8.

Sorry if I missed some points, Im only 7th grade

Answer 3

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