Free Energy and Equilibrium
Sophie Anderson
6 min read
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Study Guide Overview
This study guide covers the kinetic and thermodynamic definitions of equilibrium, including the significance of equal reaction rates and minimum free energy (G). It explains the relationship between ΔG°, ΔG, K, and Q, with equations and qualitative insights. It also provides practice questions and tips for the final exam, focusing on interpreting free energy diagrams and calculating these values.
#Equilibrium: Kinetic vs. Thermodynamic Views ⚖️
Hey there, future AP Chem master! Let's break down equilibrium, connecting kinetics and thermodynamics. This is a big topic, so let's make sure you've got it down cold for tomorrow!
#Kinetic and Thermodynamic Definitions of Equilibrium
# Kinetic Definition of Equilibrium 🏃
- Equilibrium is when the forward and reverse reaction rates are equal.
- This means that the concentrations of reactants and products remain constant over time.
Remember: Equilibrium does not mean reactions stop; they just proceed at the same rate in both directions.
# Thermodynamic Definition of Equilibrium ⚡
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Equilibrium is the point of minimum free energy (G).
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A reaction proceeds spontaneously (ΔG < 0) until it reaches this equilibrium point.
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After equilibrium, the reaction requires energy input (ΔG > 0) to continue forming products.
Think of a ball rolling down a hill. It spontaneously rolls down (negative ΔG) until it reaches the bottom (equilibrium). To get it back up, you need to push it (positive ΔG).
#Visualizing Free Energy 📉
Let's look at those graphs again. They're super important for understanding how free energy changes during a reaction:
#Spontaneous Reaction (ΔG° < 0)
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