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See attached- Thermodynamics doesn't render well in plain text!
The definition of the Gibbs free energy change is:
∆G = ∆H - T∆S,
where ∆H is the enthalpy change of the system, T is the temperature in Kelvin, and ∆S is the entropy change of the system. One of the key concepts here is the division between system and surroundings.
The system, here, consists of whatever little part of the universe you're looking at in the lab (like a flask full of reacting chemicals, for ...
This solution provides a step-by-step explanation of how to derive a relationship between ∆Suniv and ∆G using the 2nd law of thermodynamics and the definition of the Gibbs free energy.