Chemistry: Sep. 19-23
Chemistry: Sep. 19-23 CHEM 1120
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This 1 page Class Notes was uploaded by Anzlee on Thursday September 22, 2016. The Class Notes belongs to CHEM 1120 at Middle Tennessee State University taught by Ngee S Chong in Fall 2016. Since its upload, it has received 6 views. For similar materials see General Chemistry II in Chemistry at Middle Tennessee State University.
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Date Created: 09/22/16
• Isothermal Process o ∆S = q rev o q rev flow of heat for reversible process • Gibbs Free Energy (G)- maximum energy released that is available to do work o constant temperature and pressure o ∆G = ∆H -T∆S o ∆H = ∆G +T∆S o efficiency = work done divided by energy produced Chapter 13: Chemical Kinetics • Kinetics- rate of the change of concentrations of substances in chemical reactions o Reaction Rate- how quickly reaction occurs; concentration change over time o Reactant molecules must collide with sufficient energy (above activation energy) to form products o Factors effecting rate- physical state, concentration, temperature, and catalysts o Rate constant = k o Rate Law- defmne renationship between rate of reaction and concentrations § k (A) (B) • m and n are reaction order with respect to A and B (usually 1 or 2; never 3 or above) • m + n is the overall order of reaction o Reaction order- number defining dependence of rate on concentration • Photochemical Smog- internal combustion engines produce compounds that interact with sunlight, producing a mixture of gases
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