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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The Henry's law constant (k H) for O2 in water at 20°C is 1.28 x 10 -3 mol/L•atm. How many grams of O2 will dissolve in 1.75 L of H 2O in contact with air, where the partial pressure of O2 is 1.32 atm?A. 0.0541 gB. 0.0473 gC. 0.0946 gD. 0.0270 gE. 0.946 g

Solution: The Henry's law constant (k H) for O2 in water at 20°C is 1.28 x 10 -3 mol/L•atm. How many grams of O2 will dissolve in 1.75 L of H 2O in contact with air, where the partial pressure of O2 is 1.32 atm

Problem

The Henry's law constant (k H) for O2 in water at 20°C is 1.28 x 10 -3 mol/L•atm. How many grams of O2 will dissolve in 1.75 L of H 2O in contact with air, where the partial pressure of O2 is 1.32 atm?

A. 0.0541 g

B. 0.0473 g

C. 0.0946 g

D. 0.0270 g

E. 0.946 g

Solution

We’re being asked to determine the mass of O2 that will dissolve in 1.75 L H2O.


Recall that the solubility of a gas is given by Henry’s law:


Sgas=kH·Pgas


where:

 Sgas = solubility of the gas (in mol/L or M)

kH = Henry’s law constant for the gas

Pgas = partial pressure of the gas


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