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HSC Chemistry
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Module 1: Properties and Structure of Matter1.1 Properties of Matter
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1.2 Atomic Structure and Atomic Mass
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1.3 Periodicity
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1.4 Bonding
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Module 2: Introduction to Quantitative Chemistry2.1 Chemical Reactions and Stoichiometry
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2.2 Mole Concept
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2.3 Concentration and Molarity
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2.4 Gas Laws
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Module 3: Reactive Chemistry3.1 Chemical Reactions
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3.2 Predicting Reactions of Metals
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3.3 Rates of Reactions
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Module 4: Drivers of Reactions4.1 Energy Changes in Chemical Reactions
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4.2 Enthalpy and Hess's Law
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4.3 Entropy and Gibbs Free Energy
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Module 5: Equilibrium and Acid Reactions5.1 Static and Dynamic Equilibrium5 Topics
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5.2 Factors that Affect Equilibrium2 Topics
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5.3 Calculating the Equilibrium Constant2 Topics
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5.4 Solution Equilibria
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Module 6: Acid/Base Reactions6.1 Properties of Acids and Bases7 Topics
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6.2 Using Brønsted–Lowry Theory2 Topics
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6.3 Quantitative Analysis1 Topic
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Module 7: Organic Chemistry7.1 Nomenclature2 Topics
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7.2 Hydrocarbons2 Topics
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7.3 Products of Reactions Involving Hydrocarbons
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7.4 Alcohols1 Topic
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7.5 Reactions of Organic Acids and Bases
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7.6 Polymers2 Topics
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Module 8: Applying Chemical Ideas8.1 Analysis of Inorganic Substances3 Topics
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8.2 Analysis of Organic Substances
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8.3 Chemical Synthesis and Design
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Working ScientificallyWorking Scientifically Overview1 Topic
Lesson 17, Topic 1
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The Equilibrium Constant Expression
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The position or extent of a chemical equilibrium can be expressed quantitatively using the equilibrium constant (Keq).
The equilibrium constant may be written as the following, which is based on the ratio of products to reactants of an equilibrium system at a specific temperature:
K_{\text {eq}} = \frac{ [\text{products}]}{[\text{reactants}] }
But more specifically, it is calculated using the equilibrium constant expression. For the reaction below:
a\text A + b\text B ⇌ c\text C + d\text D
the equilibrium expression is:
K_{\text{eq}} = \frac{[\text C]^c[\text D]^d}{[\text A]^a[\text B]^b}
A change in temperature is the only factor that will cause the equilibrium constant to change. Factors such as pressure, concentration and volume will simply affect the position of equilibrium.