What is the Vapor Pressure of a Urea Solution at 24 C?

Thread starter TypeFun
Start date Feb 16, 2011
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Vapor

AI Thread Summary

To calculate the vapor pressure of a urea solution at 24°C, first determine the molality of the solution by dissolving 9 g of urea in 10 mL of water, which has a mass of 10 g. Using Raoult's Law, the vapor pressure of the solution can be found by adjusting the vapor pressure of pure water (22.4 mmHg) based on the mole fraction of the solvent. Since urea is a non-volatile solute, it lowers the vapor pressure of the solution compared to pure water. The final vapor pressure can be calculated by applying Raoult's Law to find the adjusted value.

Feb 16, 2011

TypeFun

Homework Statement

If you dissolve 9 g of urea (60.06 g/mol) in 10 mL of water, what is the vapor pressure of the solution at 24 C? Assume the density of water is 1.00 g/mL and the vapor pressure of pure water at 24 C is 22.4 mmHg.

Homework Equations

Henry's Law, maybe? I'm not sure.

The Attempt at a Solution

I have no clue. Help please.

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Feb 21, 2011

Borek

Mentor

Not Henry's, Raoult's.

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