Question

If 12 mg of ethanol are dissolved in 25 mL of water

a. what are the mol fractions of the two liquids in the mix

b.the vapor pressures of pure ethanol and water at 25 C are respectively 58.9 and 23.8 Torr. Calculate the vapor pressure of the mix, assuming ideality

c. once the liquid has reached equilibrium with the vapor, what will the mol fraction of the two liquids in the vapor phase be?

Answer #1

Part A
If 0.560 mol of a nonvolatile nonelectrolyte are
dissolved in 3.40 mol of water, what is the vapor pressure
PH2O of the resulting solution? The vapor pressure of pure
water is 23.8 torr at 25 ∘C .
Part B
A solution is composed of 1.90 mol cyclohexane
(P∘cy=97.6 torr) and 2.80 mol acetone (P∘ac=229.5
torr). What is the total vapor pressure Ptotal above this
solution?

Part A. If 0.680 mol of a nonvolatile nonelectrolyte are
dissolved in 3.90 mol of water, what is the vapor pressure PH2O of
the resulting solution? The vapor pressure of pure water is 23.8
torr at 25 ∘C .
Part B. A solution is composed of 1.00 mol cyclohexane
(P∘cy=97.6 torr) and 2.50 mol acetone (P∘ac=229.5
torr). What is the total vapor pressure Ptotal above this
solution?

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