Part 2: (+)-Carvone (C10H14O) is a principal component of caraway and dill seed and is used as a food flavoring agent.Calculate the molality of a solution that contains 1.73 g carvone in 13.4 mL of ethanol (density 0.7893 g/mL). Assume that carvone is nonvolatile at the normal boiling point of ethanol and that it is a nonelectrolyte.Molality = ...................... m ### Boiling Point Elevation CalculationUsing your answer from Part 2, calculate the change in boiling point and the actual boiling point for the solution. The normal boiling point of ethanol is 78.24°C, and \( K_b \) for this solvent is equal to 1.22°C/m.\[ \Delta T_b \text{ for the solution} = \_\_\_\_\_\_ \ °C \]\[ \text{and} \quad T_b = \_\_\_\_\_\_ \ °C \]*Explanation:*- **ΔTb** indicates the change in the boiling point of the solution induced by the solute.- **Tb** is the new boiling point of the solution, after taking the change into consideration. To find ΔTb, you would:1. Use the equation: \[ \Delta T_b = K_b \times m \] where \( m \) is the molality of the solution.2. Add this ΔTb to the normal boiling point of the solvent (ethanol) to find the actual boiling point (Tb) for the solution.If further details are required:- **Graph Instructions (if any):** There are no graphs included in this content.- **Diagram Instructions (if any):** There are no diagrams included in this content.

Part2 Given that: Mass of carvone = 1.73g Volume of ethanol = 13.4ml Density of ethanol =…

Answered: Using your answer from Part 2,…

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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Part 2: (+)-Carvone (C₁₀H₁₄O) is a principal component of caraway and dill seed and is used as a food flavoring agent.

Calculate the molality of a solution that contains 1.73 g carvone in 13.4 mL of ethanol (density 0.7893 g/mL). Assume that carvone is nonvolatile at the normal boiling point of ethanol and that it is a nonelectrolyte.

Molality = ...................... m

### Boiling Point Elevation Calculation

Using your answer from Part 2, calculate the change in boiling point and the actual boiling point for the solution. The normal boiling point of ethanol is 78.24°C, and \( K_b \) for this solvent is equal to 1.22°C/m.

\[ \Delta T_b \text{ for the solution} = \_\_\_\_\_\_ \ °C \]

\[ \text{and} \quad T_b = \_\_\_\_\_\_ \ °C \]

*Explanation:*
- **ΔTb** indicates the change in the boiling point of the solution induced by the solute.
- **Tb** is the new boiling point of the solution, after taking the change into consideration.

To find ΔTb, you would:
1. Use the equation:
\[ \Delta T_b = K_b \times m \]
where \( m \) is the molality of the solution.

2. Add this ΔTb to the normal boiling point of the solvent (ethanol) to find the actual boiling point (Tb) for the solution.

If further details are required:
- **Graph Instructions (if any):** There are no graphs included in this content.
- **Diagram Instructions (if any):** There are no diagrams included in this content.

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