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Ch.14 - Chemical EquilibriumWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch.17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Intro to Chemical Equilibrium
Equilibrium Constant (K)
Equilibrium Constant Calculations
Kp and Kc
Using Hess's Law To Determine K
Calculating K For Overall Reaction
Le Chatelier's Principle
ICE Charts
Reaction Quotient

Most chemical reactions never go to completion, instead reach a chemical equilibrium.

Chemical Equilibrium

Concept #1: Intro to Chemical Equilibrium Concept 1

A reaction reaches equilibrium once the rate of the forward reaction equals the rate of the reverse reaction. Once at equilibrium there is no net change in the concentration of reactants or products.

Example #1: Describe what happens when reaction reaches chemical equilibrium.

a) reaction stops

b) reactants form products as fast as products form reactants

c) the collision frequencies of products and reactants are identical

d) rates of forward and reverse reactions are equal to zero

Practice: Which of the following does not represent a heterogenous equilibrium?  

I) CH4(g) + 2 O2(g) ⇌ CO2(g) + 2 H2O(g)                  
II) CO2(g) + C(s) ⇌ 2 CO(g)
III) 2 H2O(l) ⇌ 2 H2(g) + O2(g)
IV) CH3COOH(aq) + H2O(l) ⇌ CH3COO(aq) + H3O+(aq)