Chapter 14 - Equilibrium
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32 Terms
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Equilibrium
A state where reactants and products exist simultaneously, with reversible reactions shifting back and forth between them.
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Weak Acids in Equilibrium
They can partially dissociate into ions but may also remain undissociated.
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Insoluble Ionic Compounds and K
They are not truly insoluble; only a small amount dissolves.
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Strong Acids and Equilibrium
Strong acids do not reach equilibrium; they completely convert reactants into products.
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Weak Acids and Equilibrium
Weak acids reach equilibrium, where both reactants and products are present.
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Rate Laws in Equilibrium
Both reactions are treated as elementary, with equal rates for forward and reverse processes.
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Calculating K
K is calculated using the molarity of solutions or partial pressure of gases, not for solids or liquids.
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Characteristics of K
K is always positive, dimensionless, and sensitive to temperature changes.
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Kp vs Kc
Kp and Kc are equal only when their reaction coefficients are the same.
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K < 100
The reaction favors products, indicating a larger concentration of products than reactants.
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K > 0.01
The reaction favors reactants, indicating a larger concentration of reactants than products.
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Haber Process
An equilibrium process that fixes nitrogen, traditionally involving three bonds reduced to one.
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Q (Reaction Quotient)
Q indicates the ratio of products to reactants at any point and is used to assess if a reaction is at equilibrium.
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Q vs K
Q is used for reactions not at equilibrium, while K reflects equilibrium conditions.
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Q returns to K
Q shifts to one side of the reaction to achieve equilibrium, represented by K.
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Effect of Q < K
Reactants convert to products to increase Q until it equals K.
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Effect of Q > K
Products convert to reactants to decrease Q until it equals K.
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Le Chatelier's Principle
A principle stating that a system at equilibrium will shift to counteract an imposed change.
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Adding A to Equilibrium
The reaction will shift away from A.
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Removing A from Equilibrium
The reaction will shift back towards A.
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Heating a Reaction
Heating a reaction is akin to adding energy to the system.
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Cooling a Reaction
Cooling a reaction is akin to removing energy from the system.
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Energy in Exothermic Reactions
Energy is positioned on the products side of the reaction.
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Heating an Exothermic Reaction
The reaction shifts to favor the reactants side.
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Cooling an Exothermic Reaction
The reaction shifts to favor the products side.
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Energy in Endothermic Reactions
Energy is positioned on the reactants side of the reaction.
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Heating an Endothermic Reaction
The reaction shifts to favor the products side.
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Cooling an Endothermic Reaction
The reaction shifts to favor the reactants side.
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Changing Gas Pressure in A(g) ⇌ B(g)
No effect on equilibrium due to equal moles of gas.
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Changing Gas Pressure in A(g) ⇌ 2 B(g)
Changing pressure alters the equilibrium due to unequal moles of gas.
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Increasing Pressure in Equilibrium
The reaction shifts towards the side with fewer gas moles.
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Decreasing Pressure in Equilibrium
The reaction shifts towards the side with more gas moles.
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