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Calculating Vapor Pressure & Its Lowering: Urea in Water at 35°C
Chapter 12, Problem 12.7(choose chapter or problem)
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?
Questions & Answers
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:Step 1 of 3
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