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Chemistry Module 4: Drivers of Reactions - Coggle Diagram
Chemistry Module 4: Drivers of Reactions
Energy Changes
Reactions
Exothermic
e.g. Combustion
Endothermic
e.g. Dissociation (Typically Endo)
Heat Capacity
Q=mc∆T
∆H=Q/moles
(check ± value of ∆H is right at the end)
Energy Profile Diagrams
Enthalpy changes
Activation Energy (Eₐ)
Reduced with catalyst
Type
Exothermic
Negative ∆H
Endothermic
Positive ∆H
Enthalpy & Hess' Law
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Enthalpy
Energy required to break bonds, energy released making bonds
Law of Conservation of Energy
Energy taken & released from surroundings/environment
Hess' Law
Total ∆H is the sum of all step reaction's ∆H
Total ∆H will be the same regardless of what step reactions are taken
Entropy & Gibbs Free Energy
Entropy (∆S)
Definition
The degree of disorder in a system
Identified by:
State
increases from solid to liquid to gas
Number of moles
increases as moles decreases
Temperature
Increases as temperaure increases
Gibbs Free Energy
∆G = ∆H - T∆S
Spontaneity
Spontaneous when ∆G < 0
Equalibrium when ∆G = 0
Not spontaneous when ∆G > 0
