If 0.600 mol of a nonvolatile nonelectrolyte are dissolved in 3.60 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 . Express your answer with the appropriate units. View Available Hint(s) Hint 1. Determine the mole fraction of wateropened hint What is the mole fraction of water, XH2O, in this solution?

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BatteringRam BatteringRam · Answer 1 · 2021-06-26T03:46:30+02:00

Answer: The vapor pressure of water in the resulting solution is 20.4 torr

Explanation:

Mole fraction is defined as the moles of a component present in the total moles of a solution. It is given by the equation:

[tex]\chi_A=\frac{n_A}{n_A+n_B}[/tex] .....(1)

where n is the number of moles

We are given:

Moles of a non-volatile non-electrolyte = 0.600 moles

Moles of water = 3.60 moles

Putting values in equation 1, we get:

[tex]\chi_{H_2O}=\frac{3.60}{3.60+0.600}\\\\\chi_{H_2O}=0.857[/tex]

Equation used to calculate the vapor pressure of substance A in a solution is given by:

[tex]\text{Vapor pressure in solution}=\text{Pure vapor pressure}\times \text{Mole fraction}[/tex]

We are given:

Vapor pressure of pure water = 23.8 torr

[tex]\text{Vapor pressure in solution}=23.8 torr\times 0.857\\\\\text{Vapor pressure in solution}=20.4torr[/tex]

Hence, the vapor pressure of water in the resulting solution is 20.4 torr