Ch 06 - Equilibrium11th Chemistry
Dynamic Nature of Equilibrium
Why is chemical and physical equilibrium described as "dynamic" rather than "static"?
Why is chemical and physical equilibrium described as "dynamic" rather than "static"?
Equal Rates: Both the forward and reverse processes continue to occur simultaneously at exactly the same rate.
No Net Change: Because the rates are perfectly balanced, macroscopic properties like concentration, pressure, and color remain strictly constant over time.
Analogy: Running on a treadmill; there is a lot of continuous movement, but no actual change in position.
Prism Memory Hook
Dynamic means DOING work (reactions continue), Static means STOPPED.
Proving Dynamic Chemical Equilibrium
How did Fritz Haber use deuterium () to definitively prove that chemical equilibrium is dynamic and not static?
How did Fritz Haber use deuterium () to definitively prove that chemical equilibrium is dynamic and not static?
The Experiment: Haber established ammonia synthesis equilibrium (). He then set up an identical reaction using heavy hydrogen, , to form .
The Observation: Mixing the two equilibrium mixtures resulted in a "scrambling" of isotopes, producing mixed molecules like and .
The Conclusion: If the reaction were static, no new isotopic combinations would form. Their formation proves bonds are continuously breaking and reforming even at macroscopic equilibrium.
Prism Memory Hook
Deuterium Scrambling proves the system is MINGLING.
Radioactive Tracers in Saturated Solutions
How do radioactive sugar isotopes experimentally prove the dynamic nature of solid-liquid equilibrium in a saturated solution?
How do radioactive sugar isotopes experimentally prove the dynamic nature of solid-liquid equilibrium in a saturated solution?
The Experiment: If you add a small amount of radioactive solid sugar to an already saturated solution of non-radioactive sugar, the solution initially possesses zero radioactivity.
The Observation: Over time, the solution phase becomes measurably radioactive, and simultaneously, the un-dissolved solid sugar at the bottom also exhibits radioactivity.
The Conclusion: This proves that sugar molecules from the solid crystal are continuously exchanging places with the dissolved sugar molecules in the liquid, confirming a dynamic equilibrium where the Rate of Dissolution equals the Rate of Crystallization.
Prism Memory Hook
Radioactive scrambling proves the molecules are dancing (dynamic).
Also in this chapter
46 more cards to study in Prism
- 4Characteristics of Physical Equilibria
- 5Normal Melting Point
- 6Law of Chemical Equilibrium (Kc)
- 7Dissolution of Gases in Liquids (Henry's Law)
- 8Reverse Reaction Equilibrium Constant
- 9Homogeneous vs. Heterogeneous Equilibria
- 10Stoichiometric Multiplier Effect on Kc
- 11Pure Solids and Liquids in Equilibria
- 12Equilibrium Constant for Net Reactions
- 13Units of Equilibrium Constants
- 14Relationship between Kp and Kc
- 15Reaction Quotient (Qc)
- 16Predicting the Extent of a Reaction
- 17Gibbs Energy and Reaction Quotient
- 18Predicting Direction with Qc
- 19Standard Gibbs Energy and Equilibrium Constant
- 20Spontaneity and the Equilibrium Constant
- 21Le Chatelier's Principle
- 22Effect of Concentration Change
- 23Effect of Pressure / Volume Change
- 24Effect of Inert Gas Addition
- 25Effect of Temperature Change
- 26Effect of a Catalyst
- 27Strong vs. Weak Electrolytes
- 28Arrhenius Concept of Acids & Bases
- 29Brönsted-Lowry Concept
- 30Ionic Product of Water (Kw)
- 31Amphoteric (Amphiprotic) Species
- 32pH and pOH Relationship
- 33Lewis Concept of Acids & Bases
- 34Ionization Constant of Weak Acid (Ka)
- 35Relation between Ka and Kb
- 36Polyprotic Acids
- 37pH of Salt of Weak Acid & Weak Base
- 38Factors Affecting Acid Strength
- 39Henderson-Hasselbalch Equation
- 40Common Ion Effect
- 41Solubility Product Constant (Ksp)
- 42Hydrolysis of Salts (SA + SB)
- 43Cationic vs. Anionic Hydrolysis
- 44Buffer Solutions
- 45Percent Dissociation of a Weak Acid
- 46Henderson-Hasselbalch (Basic Buffer)
- 47Net Equilibrium Constant (Polyprotic)
- 48Predicting Precipitation
- 49Effect of pH on Solubility
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