chem103b test 1

chem103b test 1 - 1 Chemistry Spring Exam1 r 12:30pm Feb...

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Chemistry 1 r) Spring 12:30pm Exam 1 - .. Feb. 14th. 2008 Write vour name at the top of this page Write vour initials on the bottom of the other pages Count the number of pages now (in case you are missing some) Full credit is only given when you Show ALL of vour work and use the correct number of siqnificant fiqures. Second Order Kinetics 1/[A]t-1l[A]o=P1 4t l/Pcut"-r Zero Order Kinetics d 'v'-a/t' tAlt - tAl" = - k t /.ltt cAtbs3v at Half Life f , +^^ IAIw= lzlA]o fft'J ?//6r Equilibrium d.. Equf Dnum a ., / for tne general reaction: DZL*n/ aA + bB a cC + dD /o,1,,.6t Universal qas constant (R): R=8.314 J/(molx K) R=8.206 x 10-2 (atm x L)/(molx K) First Order Kinetics In ([A]" / [A],) = 11 & = [Cl"* [Dll* [A]""q [B]o"q Sa'*-tL //P rt r Q" (at equilibrium) = 6" 97 ta Z / Ko = K" (RT; Ante""l p2tt zl van't Hoff Equation zt;r '4 D2t f fn (K2lK1)= (- AH,"/R)x(11T2- 1n1) Forms of the Arrhenius Equation [=]Fe;/R-D-- 1n 1 = (-Ea / R)x(1/T) + InA ln (kzlkr) = (-EalR) (11T2- 1fi1) The Quadratic Equation is available on the white board '/'/ 4l /o /." 7t, '03 bz ii"s, Question# Points 6 -.--- | ..-4 i ---5 tl,.a\ -- A b''" '-- 7 e(%-a _-. ..-.9 .-1o tl /08) /10) /10) /10) ,08) /10) /10) /09 ) /10) /10) /10) \t:
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Question #1 (8 poinrs.4 points each) @9 n"" /t' +tv /s;'u /'-o A) Express the rate of reaction in terms ofthe change in concentration of each of the reactants and products. 2A(s) ---+ B(S) + c(s) /'' -' lA7 = t('k = "l "fr B) When [Cl is increasing at 2 (mol)i(Lxs), how fast is [4 decreasing? "* '!' Jcl # =ruqe;[email protected]/.4- , u*'=. a Question #2 (10 points) @Qc/ B dsr For the reaction 4AG) + 3BG) ----'--- zc(s) the following data were obtained at constant temperatue: Initial [A] Initial [B] Initial Rate Experiment (molll) (mol.zl) (motlL.min) 0.100 0.100 2 0.300 0.100 3 0.100 0.200 4 0.300 0.200 (a) What is the order with respect to each reactant?
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chem103b test 1 - 1 Chemistry Spring Exam1 r 12:30pm Feb...

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