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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
In Progress
Lesson 14 of 31
In Progress
4.3 Entropy and Gibbs Free Energy
How can enthalpy and entropy be used to explain reaction spontaneity?
Inquiry Question
Overview
- Analyse the differences between entropy and enthalpy
- Use modelling to illustrate entropy changes in reactions
- Predict entropy changes from balanced chemical reactions to classify as increasing or decreasing entropy
- Explain reaction spontaneity using terminology, including:
- Gibbs free energy
- Enthalpy
- Entropy
- Solve problems using standard references and \Delta G\degree = \Delta H\degree - T\Delta S\degree (Gibbs free energy formula) to classify reactions as spontaneous or nonspontaneous
- Predict the effect of temperature changes on spontaneity