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

Henry's Law Calculations

GOB Chemistry

9. Solutions

Henry's Law Calculations

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Multiple Choice

The atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry's Law Constant for oxygen in water at this temperature is 5.3 x 10^-5 M/atm.

1.4×10^–3 g

6.9×10^–5 g

0.055 g

0.034 g

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Verified step by step guidance

First, calculate the partial pressure of oxygen gas using the given percentage. Since oxygen contributes 62% of the atmospheric pressure, multiply the total pressure (1.3 atm) by 0.62 to find the partial pressure of oxygen.

Next, apply Henry's Law to find the concentration of dissolved oxygen in water. Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. Use the formula: \( C = k \cdot P \), where \( C \) is the concentration, \( k \) is the Henry's Law constant (5.3 x 10^{-5} M/atm), and \( P \) is the partial pressure of oxygen calculated in the previous step.

Once you have the concentration of oxygen in molarity (M), convert this concentration to moles of oxygen dissolved in the given volume of water (25 L). Use the formula: \( ext{moles} = C \cdot ext{volume} \), where \( C \) is the concentration in M and volume is in liters.

Convert the moles of oxygen to grams using the molar mass of oxygen. The molar mass of oxygen (O_2) is approximately 32 g/mol. Use the formula: \( ext{mass} = ext{moles} \cdot ext{molar mass} \).

Finally, compare the calculated mass of dissolved oxygen to the given options to identify the correct answer.