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How do you calculate ΔG° using ΔH° and ΔS°?
Use the equation: ΔG° = ΔH° - TΔS°, where T is the temperature in Kelvin.
How do you calculate ΔG° using standard free energies of formation?
Use the equation: ΔG°rxn = ΣnΔG°f(products) - ΣnΔG°f(reactants)
Define 'thermodynamic favorability'.
The tendency of a reaction to occur spontaneously.
Define a 'spontaneous reaction'.
A reaction that occurs on its own without external energy input.
Define 'enthalpy change (ΔH°)'.
The heat change in a reaction at constant pressure.
Define 'entropy change (ΔS°)'.
The change in the disorder or randomness of a system.
Define 'Gibbs Free Energy (ΔG°)'.
A measure of the spontaneity of a reaction, combining enthalpy and entropy.
Define an 'exothermic reaction'.
A reaction that releases heat to the surroundings (ΔH° < 0).
Define an 'endothermic reaction'.
A reaction that absorbs heat from the surroundings (ΔH° > 0).
What is the effect of a negative ΔG°?
The reaction is spontaneous (exergonic).
What is the effect of a positive ΔG°?
The reaction is nonspontaneous (endergonic).
What is the effect of ΔH° < 0 and ΔS° > 0 on spontaneity?
The reaction is always spontaneous.
What is the effect of ΔH° > 0 and ΔS° < 0 on spontaneity?
The reaction is never spontaneous.
What is the effect of high temperature on a reaction with ΔH° > 0 and ΔS° > 0?
The reaction becomes spontaneous.
What is the effect of low temperature on a reaction with ΔH° < 0 and ΔS° < 0?
The reaction becomes spontaneous.