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Calculating Vapor Pressure & Its Lowering: Urea in Water at 35°C

Chapter 12, Problem 12.7

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QUESTION:

Calculate the vapor pressure of a solution made by dissolving 82.4g of urea (molar mass = 60.06 g/mol) in 212 mL of water at \(35^{\circ} \mathrm{C}\). What is the vapor-pressure lowering?

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QUESTION:

Calculate the vapor pressure of a solution made by dissolving 82.4g of urea (molar mass = 60.06 g/mol) in 212 mL of water at \(35^{\circ} \mathrm{C}\). What is the vapor-pressure lowering?

ANSWER:

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According to the Raoult's law vapor pressure of the solution can be calculated by the following formula;

\(P_{1}=X_{1} P_{1}^{o}\)

\(X_{1}\) = Mole fraction of the solvent

\(P_{1}\)  = Pressure of the solution

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Calculating Vapor Pressure & Its Lowering: Urea in Water at 35°C
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Explore the intriguing process of determining the vapor pressure of a urea-water solution at 35°C. Using Raoult's law we'll calculate the mole fraction of water and urea leading to the solution's vapor pressure. Learn how the solution's composition affects vapor-pressure lowering


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