CHEM 122 1st Edition Lecture 33 Outline of Last LectureI. Predicting the sign of Change in EntropyII. 2nd Law of ThermodynamicsIII. Calculating the Entropy ChangesIV. Third Law of Thermodynamics Outline of Current Lecture I. Entropy Change in the SurroundingsII. Gibbs Free EnergyCurrent LectureEntropy Change in the Surroundings:-∆ Ssurr=−∆ HsysT-what is the significance of this equation ? it can be replaced into the spontaneous processEquation and eliminate the surrounding part.oT ∆ Suniv=−∆ Hsys+T ∆ SsysGibbs Free Energy: ties these thermodynamic parameters together- G= H-TS- Free Energy: the portion of the energy change that is available to do useful work.- Change in Free Energy: ∆ G=∆ H−T ∆ S∨−T ∆ Sunivo∆ G Is negative then the reaction is spontaneouso : ∆ G is zero then the reaction is at equilibriumo : ∆ G is positive then the reaction is spontaneous in the reverse direction- Standard Free energy change: free energy change for the conversion of reactions in theirstandard states to productso∆ G°=∆ H°−T ∆ S°o Calculate ∆ H°∧∆ S° by using the enthalpy change equationThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best Used as a supplement to your own notes, not as a substitute.onS(products)−¿∑mS(reactants)∆ S=∑¿ Replace the S’s with H’s and then you have your ∆ H° equation This can also be used to find the values of ∆ G°o Definition of ∆ Gf°: free energy change for formation for one more of a substance from the elements in their standard
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