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Unformatted text preview: MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms . 31.1 5.111 Lecture 31 Kinetics Topics: Rates of Chemical Reactions and Rate Law Chapter 13.1-13.5 When considering a chemical reaction, one must ask whether the reaction will go (thermodynamics), and how fast the reaction will go (kinetics). A kinetics experiment measures the rate at which the concentration of a substance taking part in a chemical reaction changes with time. Oxidation of Glucose C 6 H 12 O 6 + 6O 2 6CO 2 + 6H 2 O G = H - T S H = -2816 kJ/mol T S or S is (+) G = -2,885 kJ/mol Thermodynamically favorable. But to be useful as an energy source, the oxidation of glucose must be fast enough. Glucose oxidation is slow. Body uses protein catalysts called enzymes to speed up the reactions. Factors affecting rates of reactions 1. 2. 3. 4. 5. 31.2 Measuring reaction rates Consider: NO 2 (g) + CO (g) NO (g) + CO 2 (g) [NO] (M) 0.0288 0.0160 50....
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This note was uploaded on 11/27/2011 for the course CHEMICAL E 20.410j taught by Professor Rogerd.kamm during the Spring '03 term at MIT.

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lecnotes31 - MIT OpenCourseWare http://ocw.mit.edu 5.111...

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