hand05 - Chemistry 008 Handout #5 Mrs. Harriet Smithline...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Chemistry 008 Handout #5 Mrs. Harriet Smithline Spring 2005 Chapters 13 and 14 Review Guide Lectures 2/8 and 2/10 Spontaneity of Chemical Processes and Kinetics I Entropy and The Second Law of Thermodynamics - A. The Second Law of Thermodynamics - in any spontaneous process there is always an increase in the total entropy of the universe. The total entropy change is the sum of the entropy change of the system and the entropy change of the surroundings. B. Entropy Change of the Surroundings - For reactions that occur at constant pressure, the entropy change of the surroundings is given by the following: S surr = - H sys T S univ = S sys - H sys rearrangement gives –T S univ = H sys -T S sys T II. Free Energy (G) - the usable energy produced (or consumed) by a chemical reaction. The free energy is related to the absolute temperature, enthalpy and entropy of a system according to the relationship: G = H - TS. The change in free energy is given by: G = H - T S, where T must be in kelvins. This is the equation in part I B above where –T S univ is defined as G. The spontaneity of a reaction can be determined by the value of G . When G < 0, the reaction goes spontaneously forward from reactants to products. When G > 0, the forward reaction is non- spontaneous and going from products back to reactants is spontaneous. When
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 2

hand05 - Chemistry 008 Handout #5 Mrs. Harriet Smithline...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online