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11) A compound containing only boron, nitrogen, and hydrogen was found to be 40.3% B, 52.2% N, and 7.5% H by mass. When 3.301 g of this compound is dissolved in 50.00 g of benzene, the solution produced freezes at 1.30 °C. The freezing point of pure benzene is 5.48 °C; Kb for benzene is 5.12 °C m¹. What is the molecular weight of this compound? a) Determine the molecular weight of the solid. b) Determine the molecular formula of the solid c) Determine the mole fraction of the solid in the solution d) If the density of this solution is 0.8989 g/mL, calculate the molarity of the solution?

11) A compound containing only boron, nitrogen, and hydrogen was found to be 40.3% B, 52.2% N, and 7.5% H by mass. When 3.301 g of this compound is dissolved in 50.00 g of benzene, the solution produced freezes at 1.30 °C. The freezing point of pure benzene is 5.48 °C; Kb for benzene is 5.12 °C m¹. What is the molecular weight of this compound? a) Determine the molecular weight of the solid. b) Determine the molecular formula of the solid c) Determine the mole fraction of the solid in the solution d) If the density of this solution is 0.8989 g/mL, calculate the molarity of the solution?

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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11) A compound containing only boron, nitrogen, and hydrogen was found to be 40.3% B, 52.2% N, and 7.5% H by mass. When 3.301 g of this compound is dissolved in 50.00 g of benzene, the solution produced freezes at 1.30 °C. The freezing point of pure benzene is 5.48 °C; Kb for benzene is 5.12 °C m¹. What is the molecular weight of this compound? a) Determine the molecular weight of the solid. b) Determine the molecular formula of the solid c) Determine the mole fraction of the solid in the solution d) If the density of this solution is 0.8989 g/mL, calculate the molarity of the solution?
Transcribed Image Text:11) A compound containing only boron, nitrogen, and hydrogen was found to be 40.3% B, 52.2% N, and 7.5% H by mass. When 3.301 g of this compound is dissolved in 50.00 g of benzene, the solution produced freezes at 1.30 °C. The freezing point of pure benzene is 5.48 °C; Kb for benzene is 5.12 °C m¹. What is the molecular weight of this compound? a) Determine the molecular weight of the solid. b) Determine the molecular formula of the solid c) Determine the mole fraction of the solid in the solution d) If the density of this solution is 0.8989 g/mL, calculate the molarity of the solution?
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