StudentLecture_05

# StudentLecture_05 - Announcements CHM 11600 Office hour...

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Announcements CHM 11600 1/26/2010 Office hour this week: Thursday, 2:30 Lab this week: A Chemical Oscillation Reaction. HW03 is due on Friday Exam 1, 8:00 PM, Monday, Feb. 7. Hall of Music. Covers Lectures 1 – 7, HW 1- 4, Labs from weeks 2 and 3. Old exams are on Blackboard.

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_____________ of reaction & ____ are found by experiment. The Method of Initial Rates Run # Initial [A] ([A] 0 ) Initial [B] ([B] 0 ) Initial Rate (v 0 ) 1 1.00 M 1.00 M 1.25 x 10 -2 M/s 2 1.00 M 2.00 M 2.5 x 10 -2 M/s 3 2.00 M 2.00 M 2.5 x 10 -2 M/s What is the rate constant for this reaction? First, determine the order of ______________.
Calculating Rate Constants rate = _____________________ Now, the rate constant can be determined from any of the experimental runs. From run # 3 rate = ___________________ k = 1.25 x 10 -2 s -1 Now that we have the rate constant and order, the initial rate at any concentration can be calculated!

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Math Crib if log a = x, a = 10 x if ln a = y, a = e y e = 2.718 log a = 2.303 ln a ln (a x b x c) = ln a + ln b + ln c ln (a/b) = ln a – ln b a = b m ln a = m x ln b ln a / ln b = m Take the log (or ln) of both sides to isolate the exponent
Calculating Rate Constants Run # [A] 0 [B] 0 [C] 0 rate 0 1 0.151 M 0.213 M 0.398 M 0.480 M/s 2 0.251 M 0.105 M 0.325 M 0.356 M/s 3 0.151 M 0.213 M 0.525 M 1.102 M/s 4 0.151 M 0.250 M 0.480 M 0.988 M/s What is the initial rate of the reaction when all the reactants are at 0.100 M concentrations? Note to Self: Keep oncamera

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Calculating Rate Constants rate = k [A] a [B] b [C] c The ratio of the initial rates of runs 1 and 3 ( only [C] changes) is then: _________________ ln ln
Calculating Rate Constants rate = k [A]

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StudentLecture_05 - Announcements CHM 11600 Office hour...

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