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At an unknown temperature a solution made of (5.3400x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.70x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (5.030x10^1) g/mol.

At an unknown temperature a solution made of (5.3400x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.70x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (5.030x10^1) g/mol.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter10: Solutions
Section: Chapter Questions
Problem 73QAP: Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol,...
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At an unknown temperature a solution made of (5.3400x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.70x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (5.030x10^1) g/mol. Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.
Transcribed Image Text:At an unknown temperature a solution made of (5.3400x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.70x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (5.030x10^1) g/mol. Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.
A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of 80.0 mm Hg) and ChemicalB (with a pure vapor pressure of 100.0 mm Hg). The solution has a total vapor pressure of (9.66x10^1) mm Hg. If the solution is known to be made from 3.00 mol of A, how many moles of B must there be in the solution? HINT: The total pressure is the sum of each chemical's partial pressure: Pt = PA + PB. Use PA = XA PA° for both the partial pressure of chemicals A and B. Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.
Transcribed Image Text:A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of 80.0 mm Hg) and ChemicalB (with a pure vapor pressure of 100.0 mm Hg). The solution has a total vapor pressure of (9.66x10^1) mm Hg. If the solution is known to be made from 3.00 mol of A, how many moles of B must there be in the solution? HINT: The total pressure is the sum of each chemical's partial pressure: Pt = PA + PB. Use PA = XA PA° for both the partial pressure of chemicals A and B. Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.
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