Thermodynamic Definitions
- Macroscopic Properties
- Intensive and Extensive properties
- Systems
- Open system
- Closed Systems
- Isolated systems
- Exothermic
- Endothermic
- Work
- Internal Energy
- Enthalpy
- Heat of formation
- Heat of reaction
Solutions Links
Hess’s Law Explanation and Problems
- Calorimeter and problems
- Hess’s Law and problems
- Heat of solution lab#1
- Enthalpy of neutralization – Validation of Hess’s Law lab #2
Thermodynamics Topics For SCH4U
• Open system (examples needed for all systems)
• Closed system
• Isolated system
• Surroundings
• Intensive and Extensive properties examples
• Macroscopic and microscopic properties
• How will you express work done by a system due to expansion or contraction ‘w’ and PΔV
• First law of thermodynamics ΔE = q ± w
• Calorimetry problems on q = mcΔT, heat lost = heat gained
• Mathematical equation that represents the first law of thermodynamics and simple problems
• Terms used to represent heat change and sign convention
• Internal energy and enthalpy
• Difference between internal energy and enthalpy
• Under what conditions does internal energy become equal to enthalpy
• Heat of formation
• Heat of reaction
• Exothermic and endothermic reactions sign convention and graphing
• Difference between heat of reaction and heat of formation
• Different types of heat of formation or enthalpy of formation
• Convention for representing heat (Enthalpy) of formation and heat of reaction
• Exothermic changes and endothermic changes
• Graphical representation of exothermic and endothermic reactions, simple problems can be expected here
• Potential energy diagrams for the formation of a Hydrogen like molecule, graph and diagram
• Factors that determine the formation of a molecule (Attractive and Repulsive)
• Bond energy and bond dissociation energy
• Bond length – definition
• STP and SATP conditions
• Writing thermochemical equations using conventions.
• Hess’s Law statement and problems
o Equation method problems
o Heat of formation of products – reactants problems
• Calculation of heat of reaction or enthalpy of reaction
• Calculation of enthalpy of formation of compounds using Hess’s law
• Relation between bond energies and enthalpy changes during chemical reactions
• Calculation of enthalpy change from bond energies, problems
• Born Haber Cycle – Represent graphically the formation of ionic compounds or molecular compounds. Problems based on Born Haber Cycle
• Application of thermochemistry in real life situation Hot packs, Cold packs , recycling energy
• Nuclear chemistry, how energy is released due to fission and fusion – Remember Nuclear Brochure, Calculation of energy released using the equation E = mc2 , where ‘m’ is the mass defect due to fission or fusion.
• Spontaneity in chemical reaction
• Predicting entropy of chemical and physical changes
• Conditions for spontaneity
• Problems based on Gibbs Helmholtz equationΔG = ΔH -TΔS
• Free energy and equilibrium constant problems ΔG = -RTlnKc
• Predicting feasibility of reactions
• Calculating temperature of feasibility
• Units of energy
• Practice all the different types of problems that we have done in class and assigned from the text.
• Read your text book and review before your test