Biogeochemistry

2.

Chemical Foundations

2.1.

2.1.1.

First Law of Thermodynamics

2.1.2.

Second Law of Thermodynamics

2.1.3.

Gibbs Free Energy

2.1.3.1.

Standard Free Energy

2.1.3.2.

Free Energy and Equilibrium

2.1.3.3.

Temperature and Pressure Effects

2.1.4.

Chemical Equilibrium

2.1.4.1.

Equilibrium Constants

2.1.4.2.

Le Chatelier's Principle

2.1.4.3.

Activity vs Concentration

2.1.5.

Spontaneity of Reactions

2.1.5.1.

Predicting Reaction Direction

2.1.5.2.

Coupling of Reactions

2.2.

Reaction Kinetics

2.2.1.

Rate Laws and Rate Constants

2.2.2.

Factors Affecting Reaction Rates

2.2.2.1.

Temperature Effects

2.2.2.2.

Concentration Effects

2.2.2.3.

2.2.3.

Enzyme Kinetics

2.2.3.1.

Michaelis-Menten Kinetics

2.2.3.2.

Enzyme Inhibition

2.2.3.3.

Environmental Controls on Enzyme Activity

2.2.4.

Surface Reactions

2.2.4.1.

Heterogeneous Catalysis

2.2.4.2.

Mineral Surface Interactions

2.3.

Acid-Base Chemistry

2.3.1.

2.3.2.

2.3.2.1.

Carbonate Buffer System

2.3.2.2.

Phosphate Buffer System

2.3.2.3.

Organic Acid Buffers

2.3.3.

Acid-Base Reactions in Natural Waters

2.3.3.1.

Carbonic Acid System

2.3.3.2.

2.3.3.3.

Mineral Acid-Base Reactions

2.4.

Redox Chemistry

2.4.1.

Electron Transfer Processes

2.4.2.

2.4.3.

Electron Activity and pe

2.4.4.

Redox Potential (Eh)

2.4.4.1.

Standard Electrode Potentials

2.4.4.2.

Nernst Equation

2.4.4.3.

Environmental Eh Measurements

2.4.5.

2.4.5.1.

Oxic Environments

2.4.5.2.

Suboxic Environments

2.4.5.3.

Anoxic Environments

2.4.5.4.

Sulfidic Environments

2.4.6.

Electron Acceptor Hierarchy

2.4.6.1.

Oxygen Reduction

2.4.6.2.

Nitrate Reduction

2.4.6.3.

Manganese Reduction

2.4.6.4.

2.4.6.5.

Sulfate Reduction

2.4.6.6.

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1. Introduction to Biogeochemistry

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3. Geological Foundations