CHEM 102 1nd Edition Lecture 12 Outline of Last Lecture I. Entropy in Solution and SurroundingsII. Boiling PointsIII. Reaction RatesOutline of Current Lecture I. Test ReviewII. Average RateIII. Instantaneous RateIV. Initial RateV. Factors & Reaction RatesCurrent LectureI. Test Reviewa. Normality = equivalentsmolesb. Equivalents are the number of H+ or OH- ions that would be created if the ion were to be separated c. To find ΔE when you have equations with ΔH; use the equation E = H + nrt; therefore in order to determine which E would match H, count the number of moles of gas (n)d. Use the equation Moles of products – moles of reactants to determine nII. Average Ratea. 2 BrNO (g) 2 NO (g) + Br2 (g)i. What is the average rate of BrNO between 50 to 100 secondsii. Where, t = 0, BrNO = 0.10 M; 50, 0.082 M; 100, 0.70 Miii. Average Rate = −12×(0.007−0.0082)50 = 0.12 e-4iv. Original equation can be found in the previous lecture notes ***III. Instantaneous Ratea. Negative slope of the tangent line to the rate line at a specific timeb. If you were presented with a graph, then you must draw a tangent line and determine the slope of the linec. The negative slope would be the instantaneous rateThese 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.IV. Initial Ratea. The instantaneous rate at t = 0 V. Factors & Reaction Ratesa. All of the following increase reaction rates:i. Larger surface areaii. Increase in reactant concentrationiii. Increased tempiv. Presence of
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