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Unit 4: Equilibrium - Coggle Diagram
Unit 4: Equilibrium
Theory
Le Chatelier's Principle - An equilibrium equation will always try to counteract an external stress done on it
Examples of stress: Addition of a product/reactant.
Volume Changes
Pressure Changes
Temperature Changes
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Equilibrium Constant (K)
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RICE Tables - a type of problem solver very useful in equilibrium problems, helps determine concentrations
Equilibrium - When the forward reaction and the reverse reaction equal each other in rate. System Must be closed with constant pressure and temperature
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Connection to Unit 2: Thermo and Rates. In a concentration time graph of a reaction the products and the reactants both stay at a constant after some time. When they are constant, this is at Equilibrium
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The Haber Process (N2 (g) + 3H2 (g) ⇌ 2NH3 (g) ) Was a great development as it was one of the first fertilizers that's used
Connection to Unit 1: Properties of solids. In equilibrium we learned about the Haber process. We also learned that in the process lowering the temperature in the system allows us to yield more ammonia, this is because ammonia has Non-Polar bonds versus the Atomic Molecules Nitrogen and Hydrogen, this means it turns to liquid at a higher temperature which means you can yield more NH3 and allow the reaction to occur faster in the products direction
Connection to Unit 2: Thermo and Rates. If you apply energy to an Exothermic reaction the reaction would shift to the reactants, if you apply energy to an Endothermic reaction the reaction would shift to the products. This then shows that the Haber Process is an Exothermic reaction because taking energy away (Lowering temperature) Favors the products side.
Application
Solubility
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This is a RICE table for solublity
Acid and Base Titrations
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Arrhenius Definition - OH- or H+
Qualitative Observations of Acids: Sour Taste, Soluble in water, Turns Litmus Red
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Qualitative Observations of Bases: Bitter Taste, Soluble in water (Can be insoluble), Turns Litmus Blue
Connection to Unit 5: Bases can conduct electricity in water if they are soluble Means they are electrolytes
pH is a number on a scale that represents the concentration of [H3O+] Ions. pH = -log([H3O+]. 7 is neutral, below 7 is acidic, above 7 is basic
pOH is a number on a scale that represents the concentration of [OH-] Ions. pH = -log([OH-]. 7 is neutral, below 7 is Basic, above 7 is Acidic
pH indicators can be used to tell the acidity of a solution. Certain ones are better some applications than others. Preferably you should use the ones that go from no color to color
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This is a RICE table for Titration