Lec-41-FinalExamReview-2

Lec-41-FinalExamRevi - Lec-41-FinalExamReview-2 Lec-41 Final Exam Review Final Exam Tue Dec 15th 8:15 10:45 PM No one will be permitted to leave

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Lec-41-FinalExamReview-2 12/11/2009 Chemical Kinetics. Chemical Equilibrium. Solutions. Acid-Base equilibrium. Electrochemistry. Complexes. 1 Lec-41: Final Exam - Review 1 Final Exam, Tue., Dec. 15 th , 8:15 – 10:45 PM No one will be permitted to leave the exam before 9:45 PM. Solar ID Room 000000000 – 106573523 Old Chemistry 116 106573524 – 106646096 Javits 101 106646097 – 999999999 Earth & Space Science 001 Review Final Exam Sunday Dec. 13, 3:00 − 6:00 PM Old Chemistry 116 Rate of a Chemical Reaction           = CD A B 1 aver 11 age rat 1 e t t tt a t b t t cd    + A B ab 2
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Lec-41-FinalExamReview-2 12/11/2009 Chemical Kinetics. Chemical Equilibrium. Solutions. Acid-Base equilibrium. Electrochemistry. Complexes. 2 The Rate Law It is frequently found (but by no means always) that for a given reaction       reactanct conc rate con entratio s ns tant rate rate l A aw B mn k The exponents m, n, … can be integers or fractions (positive or negative). m: order of the reaction with respect to substance A. n: order of the reaction with respect to substance B. order of the reaction          1 order of the react 1 o 1 1 in mol mol time units of k tim m e ol  3 The Integrated Rate Law   rate A k     0 A A t t k e 1 A ln mol t    0 1 A ln mol slope k    2 rate A k     0 1 A 1 A t t k 1 A t t Slope= k 0 1 A   0 A rate kk     0 A A t k t A t Slope=- k 0 A 4
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Lec-41-FinalExamReview-2 12/11/2009 Chemical Kinetics. Chemical Equilibrium. Solutions. Acid-Base equilibrium. Electrochemistry. Complexes. 3 Half-Life The half-life of the reaction t ½ is the time required for the concentration of the reactant species to decrease to half of its initial value.     1 2 0 A A / 2 t t 5 For a first order reaction:   1 2 ln 2 / k t 1 A ln mol t    0 1 A ln mol slope k  1 A t t Slope= k 0 1 A For a second order reaction:     0 1 2 1 A / t k Dependence of the rate constant with temperature The Arrhenius Equation More energy is available to the reaction system as the temperature increases. E a is the activation energy (units of energy, kJ mol –1 ) R is the gas constant (kJ K –1 mol –1 ) T is the temperature (K) 6   frequency factor (same u rate nits constant as ) a k E RT A e kT This leads to a temperature dependence of the rate constant . Experimentally Arrhenius found:
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Lec-41-FinalExamReview-2 12/11/2009 Chemical Kinetics. Chemical Equilibrium. Solutions. Acid-Base equilibrium.
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This note was uploaded on 01/05/2010 for the course CHE 132 taught by Professor Hanson during the Fall '08 term at SUNY Stony Brook.

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Lec-41-FinalExamRevi - Lec-41-FinalExamReview-2 Lec-41 Final Exam Review Final Exam Tue Dec 15th 8:15 10:45 PM No one will be permitted to leave

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