Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

9. Solutions

Boiling Point Elevation

GOB Chemistry

9. Solutions

Boiling Point Elevation

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Multiple Choice

Carbon dioxide is dissolved in 722 mL of benzene with a density of 1.59 g/mL. What mass of carbon dioxide would you add to make the boiling point of the solution 104.7ºC?

11 g

500 g

22.9 g

491 g

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Verified step by step guidance

First, identify the boiling point elevation formula: ΔT_b = i * K_b * m, where ΔT_b is the boiling point elevation, i is the van't Hoff factor (which is 1 for non-electrolytes like CO2), K_b is the ebullioscopic constant of benzene, and m is the molality of the solution.

Calculate the boiling point elevation (ΔT_b) by subtracting the normal boiling point of benzene (80.1ºC) from the desired boiling point of the solution (104.7ºC).

Use the calculated ΔT_b and the known K_b value for benzene (2.53 ºC kg/mol) to find the molality (m) of the solution using the formula: m = ΔT_b / (i * K_b).

Convert the volume of benzene (722 mL) to mass using its density (1.59 g/mL) to find the mass of the solvent in kilograms, which is needed to calculate molality.

Finally, use the molality and the mass of the solvent to calculate the mass of CO2 needed. Molality is defined as moles of solute per kilogram of solvent, so rearrange the formula to find the moles of CO2, then convert moles to grams using the molar mass of CO2 (44.01 g/mol).