Chem 162-2011 Lecture 3 Part II

Chem 162-2011 Lecture 3 Part II - CHEMISTRY 162-2011...

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CHEMISTRY 162-2011 Lecture 3: 12.8-12.10; 13.1-13.3 ANNOUNCEMENTS E-MAIL ATTENDANCE Sign in QUIZ Recitation quiz this week  Chapter 12.1 – 13.3 MISCELLANEOUS Chem 162-2011 Lecture 3 1
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PLAN FOR TODAY : DO LECTURE 2 LECTURE 3 PHYSICAL PROPERTIES OF SOLUTIONS Solutions of electrolytes Colloids CHEMICAL KINETICS Chemical Kinetics – A Preview The meaning of reaction rate Measuring reaction rates Chem 162-2011 Lecture 3 2
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LECTURE 3     :       FORMULAS     ET: Rate = speed. Using a diagram with Y being 100 lbs and 110 lbs, and days 0 to 5, show that the increase in weight = slope = (Y 2 – Y 1 )/(X 2 – X 1 ) = +2lb/day. Decrease in weight = -increase in weight = -slope = -(Y 2 – Y 1 )/(X 2 – X 1 ) = -2lb/day. ET: Point out that table in middle of page contains the key formulas in kinetics. Discuss these formulas at beginning of recitation, focusing on 1 o reaction. C 12 H 22 O 11 (sucrose) + H 2 O → 2 C 6 H 12 O 6 (glucose) Rate of sucrose disappearance = -(∆ [sucrose])/(∆ time) = -([sucrose f ] - [sucrose i ])/(t f - t i ) Rate of glucose appearance = 2 x Rate of sucrose disappearance aA + bB → cC + dD General rate of reaction = -(1/a)(∆[A]/∆t) = -(1/b)(∆[B]/∆t) = (1/c)(∆[C]/∆t) = (1/d)(∆[D]/∆t) Determination of order of reaction through method of initial rates: For a single reactant: Rate 1 = k[A 1 ] m Rate 2 = k[A 2 ] m (Rate 1/Rate 2) = (k[A 1 ] m )/(k[A 2 ] m ) = ([A 1 ]/[A 2 ]) m For two reactants: Rate1 = k[A 1 ] m [B 1 ] n Rate2 = k[A 2 ] m [B 1 ] n (Rate1/Rate2) = (k[A 1 ] m [B 1 ] n )/(k[A 2 ] m [B 1 ] n ) = (A 1 /A 2 ) m Integrated Reaction Differentiated rate law k Order Reaction Rate** RATE LAW*** (y = mx + b) Half-life * units 0 Avg Rate = -(C 2 -C 1 )/(t 2 -t 1 ) Inst Rate = k[C] o =k [C] t = -kt + [C] o t 1/2 = [C] o /2k M 1 s -1 1 Avg Rate = -(C 2 -C 1 )/(t 2 -t 1 ) Inst Rate = k[C] 1 ln[C] t = -kt + ln[C] o t 1/2 = 0.693/k M o s -1 2 Avg Rate = -(C 2 -C 1 )/(t 2 -t 1 ) Inst Rate = k[C] 2 1/[C] t = kt + 1/[C] o t 1/2 = 1/(k[C] o ) M -1 s -1 ** Rate of appearance = +slope; rate of disappearance = -rate of appearance = -slope. *** Differentiated Rate Law may be for more than one component, e.g., Rate = k[C] 1 [D] 2 *Half-lives : For a zero order reaction, each successive half-life is ½ the time of the preceding one. For a first order reaction, each successive half-life is equal in time to the preceding one.
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This document was uploaded on 11/02/2011 for the course GEN CHEM 162 at Rutgers.

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Chem 162-2011 Lecture 3 Part II - CHEMISTRY 162-2011...

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