Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

14. Solutions

Boiling Point Elevation

General Chemistry

14. Solutions

Boiling Point Elevation

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

A glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g of water. Determine the boiling point of the solution. The boiling point elevation constant (Kb) for water is 0.512 °C/m. What is the boiling point of the solution?

99.85 °C

101.02 °C

100.39 °C

100.12 °C

Previous problemNext problem

Verified step by step guidance

Calculate the molar mass of glucose (C6H12O6) using the atomic masses: Carbon (C) = 12.01 g/mol, Hydrogen (H) = 1.01 g/mol, Oxygen (O) = 16.00 g/mol. Use the formula: Molar mass = (6 * 12.01) + (12 * 1.01) + (6 * 16.00).

Determine the number of moles of glucose by dividing the mass of glucose by its molar mass. Use the formula: Moles of glucose = \( \frac{55.8 \text{ g}}{\text{Molar mass of glucose}} \).

Calculate the molality of the solution, which is the moles of solute per kilogram of solvent. Use the formula: Molality (m) = \( \frac{\text{Moles of glucose}}{0.455 \text{ kg of water}} \).

Use the boiling point elevation formula to find the change in boiling point: \( \Delta T_b = K_b \times m \), where \( K_b \) is the boiling point elevation constant (0.512 °C/m) and \( m \) is the molality.

Add the boiling point elevation (\( \Delta T_b \)) to the normal boiling point of water (100 °C) to find the boiling point of the solution: Boiling point of solution = 100 °C + \( \Delta T_b \).