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SP. 7 A student in chemistry 2 laboratory measured 75 g of a unknown compound with molar mass of 92 g/mol and dissolved in 100 g of water (H₂O). What is the expected total boiling point of the solution? (The normal boiling point of water is 100°C, boiling point elevation constant of water is 0.51°C/mol)

SP. 7 A student in chemistry 2 laboratory measured 75 g of a unknown compound with molar mass of 92 g/mol and dissolved in 100 g of water (H₂O). What is the expected total boiling point of the solution? (The normal boiling point of water is 100°C, boiling point elevation constant of water is 0.51°C/mol)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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SP. 8 Calculate the boiling point of a solution that contains 45.5 g of glycerol C3H5(OH)3, a non-volatile, non- dissociating solute in 200 g of water (H₂O). SP. 9 What is the boiling point of a solution prepared by adding 29.3 g of methol (C10H200) to 0.0590 kg of chloroform?
Transcribed Image Text:SP. 8 Calculate the boiling point of a solution that contains 45.5 g of glycerol C3H5(OH)3, a non-volatile, non- dissociating solute in 200 g of water (H₂O). SP. 9 What is the boiling point of a solution prepared by adding 29.3 g of methol (C10H200) to 0.0590 kg of chloroform?
2A. Boiling Point Elevation Boiling point elevation occurs when the boiling point of a solution becomes higher than the boiling point of a pure solvent. The temperature at which the solvent boils is increased by adding any non-volatile solute. The amount of boiling point elevation can be calculated using the Clausius-Clapeyron equation and Raoult's law. For an ideal dilute solution: Boiling Point total (Tb) = Boiling Pointsolvent (Tbsolv) + AT AT₁ = K₂m where: AT = boiling point elevation Kb = boiling point elevation constant m = molality of solute constants for some common solvents: Solvent Water Benzene Chloroform Normal Boiling Point, °C 100°C 80.1°C 61.3°C Bp elevation const., °C/mol 0.51 °C/mol 2.53 °C/mol 3.63 °C/mol SP. 7 A student in chemistry 2 laboratory measured 75 g of a unknown compound with molar mass of 92 g/mol and dissolved in 100 g of water (H₂O). What is the expected total boiling point of the solution? (The normal boiling point of water is 100°C, boiling point elevation constant of water is 0.51°C/mol)
Transcribed Image Text:2A. Boiling Point Elevation Boiling point elevation occurs when the boiling point of a solution becomes higher than the boiling point of a pure solvent. The temperature at which the solvent boils is increased by adding any non-volatile solute. The amount of boiling point elevation can be calculated using the Clausius-Clapeyron equation and Raoult's law. For an ideal dilute solution: Boiling Point total (Tb) = Boiling Pointsolvent (Tbsolv) + AT AT₁ = K₂m where: AT = boiling point elevation Kb = boiling point elevation constant m = molality of solute constants for some common solvents: Solvent Water Benzene Chloroform Normal Boiling Point, °C 100°C 80.1°C 61.3°C Bp elevation const., °C/mol 0.51 °C/mol 2.53 °C/mol 3.63 °C/mol SP. 7 A student in chemistry 2 laboratory measured 75 g of a unknown compound with molar mass of 92 g/mol and dissolved in 100 g of water (H₂O). What is the expected total boiling point of the solution? (The normal boiling point of water is 100°C, boiling point elevation constant of water is 0.51°C/mol)
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