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Wednesday and Thursday 4/2 and 4/2

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As you enter the classroom Sit in your assigned seat Get out your homework – we’re going to go over the answers together Reminder: 1) don’t turn your brains off, we are learning today 2) please ask questions today if you don’t understand – see if your classmates can answer

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Reminder The TRY 2 ticket for the Acid Base Test will be posted by Friday night. The Try 2 and Try 3 window is Monday-Wednesday. Check the website Friday evening for more information.

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Homework Answers 3. Molecularity of elementary reactions a. uni b. bi c. bi d. bi e. uni

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4. a. There are two intermediates, B and C b. There are 3 transition states (the peaks) c. The fast step is C D (the activation energy is lowest) d. Endothermic (Products are higher in E than reactants)

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5. a. two peaks indicate 2 elementary reaction b. One intermediate c. The second step is rate-limiting (because the activation energy is higher) d. exothermic

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7. a. rate = k[H 2 O 2 ][I] rate = k[IO][H 2 O 2 ] b. 2H 2 O 2 + I 2H 2 O + O 2 + I c. IO is an intermediate d. rate = k[H 2 O 2 ][I] (I omitted charges because I was being lazy. I hope you included them)

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Write down your homework (I won’t be doing the weebly) Packet questions: 9, 10, 15, 21 Please do your homework – remember that you’re preparing for a mock AP and the real AP

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Starting with the person who has longest hair Go around the table stating the three parts of collision theory

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Take Notes (I won’t be posting this ) What affects the rate of a reaction? There are a few… In your group, try to come up with at least 3 Share with the class…

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You don’t have to write down fun facts… 1. Temperature of the system – Heat ‘em up speed ‘em up! – Rule of thumb: 10 K rise in temp usually doubles the rate – Fun fact: refrigeration works to slow the rate of biological reactions that cause spoiling

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Temperature continued At a higher temperature, a larger fraction of the molecules are moving faster and thus meet the energy requirement for a successful reaction (have enough E to overcome the activation energy barrier) The Y axis is % of molecules with a given speed/KE Maxwell-Boltzman distribution:

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2. Chemical nature of reactants – Inherent tendencies of atoms/molecules/ions to undergo changes in chemical bonds – Fun fact: sodium exposed to air tarnishes (loses electrons) almost instantly, potassium is slower and tarnishes (loses electrons) easier with moisture in the air

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3. Ability of reactants to meet – Most reactions involve the collision of reactants – Homogeneous (reactants are in the same state, like both being liquid or both being gases) vs heterogeneous (one reactant might be solid while the other is aqueous) – Surface area! Increasing surface area increases the rate of a reaction Fun fact: liquid gas burns rapidly but gasoline vapor explodes

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4. Concentrations of the reactants – Most reaction rates slow as the reactants are used up – Fewer molecules mean few collisions mean few reactions This is the reason we study the INITIAL rate of a reaction – Exception: if a reaction is zero order for a reactant, changing its concentration should not affect the rate

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5. Presence of catalysts – Substances which increase the rates of reactions without being used up – Important: they do this by creating a NEW pathway that has a transition state with less energy; the activation energy of the new pathway is less

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More on Catalysts 3 classes of catalysts I want you to know about: 1.Acid-base catalysts Reactant either gains or loses a proton which changes the rate of the reaction 2.Surface catalysts (more on this on next slide) 3.Enzymes (more on this on next slide)

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Surface catalyst either a new reaction intermediate is formed or the probability of successful collisions is modified, changing the rate of the reaction In the diagram, the surface helps reactants come together (both reactants sit on surface and are therefore more likely to find each other than running around in 3 dimensions)

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Enzymes some bind to a reactant in a way that lowers Ea; others react with the reactant to form a new intermediate In the diagram, the enzyme helps with orientation to speed the reaction rate

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With your face partner, answer the following: (groups of 3, just rotate around) Rally robin (go back and forth), starting with partner A, to answer the following: – What are 5 things that effect the rate of a reaction Partner B answers this question: what does the maxwell-boltman distribution show? Partner A answers this question: when does concentration have no effect on the rate? Starting with partner B, rally robin to answer this question: what are the 3 types of catalysts

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Acid Base Try 1 You will now work as a team to do corrections to the acid base test you took last week Each team will get one fresh copy of the test Alternate scribes between all 4 people – The purpose is learning, so you’re only jipping yourself if you allow teammates to write answers that you don’t understand – Answer all 3 parts for #4 and write two answers for #5c When you’re done, hand in your individual tests and the group test (2 separate stacks) – Start your HW if the bell hasn’t rung You may use your notes. DO NOT HAVE A CELL PHONE OUT!!! Try 2 ticket posted by Friday night. Retakes Monday-Wednesday.

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Friday 4/4/14 Put desks into groups for class Put groups back into rows at end of class

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As you enter the classroom Sit in your assigned seat Get out your homework – we’re going to go over the answers together Reminder: 1) don’t turn your brains off, we are learning today 2) please ask questions today if you don’t understand – see if your classmates can answer

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Reminder The TRY 2 ticket for the Acid Base Test will be posted by Friday night. The Try 2 and Try 3 window is Monday-Wednesday. Check the website Friday evening for more information.

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Let’s go over homework

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New stuff: Integrated Rate Laws A third method to determine the order of a reactant (we already learned about reaction mechanisms and the method of initial rates) You need a graphing calculator!!!

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Graphs Can Give Us Orders If a reaction is zero order for a given reactant, the graph of [ ] vs time will be linear k=-slope

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If a reaction is first order for a given reactant, the graph of ln[ ] vs time will be linear k=-slope Since the reaction is NOT zero order, the graph of [ ] vs time is NOT linear

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If a reaction is second order for a given reactant, the graph of 1/[ ] vs time will be linear k=slope Since the reaction is NOT zero order, the graph of [ ] vs time is NOT linear Since the reaction is NOT first order, the graph of ln[ ] vs time is NOT linear

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Let’s create a summary chart orderLinear graphk= 0[ ] vs time-slope 1ln[ ] vs time-slope 21/[ ] vs timeslope We’ll fill in the last column later

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Data from an experiment on the reaction A B is graphed. Based on the experimental data, the rate law is most likely: a.rate = k[A] 0 b.rate = k[A] 1 c.rate = k[A] 2 d.Not enough information

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Data from an experiment on the reaction A B is graphed. Based on the experimental data, the rate law is most likely: a.rate = k[A] 0 b.rate = k[A] 1 c.rate = k[A] 2 d.Not enough information

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Instead of graphs, I could just give you data and you could use your calculator to do 3 linear regressions….get your calc Whichever R 2 value is closest to one indicates the order First, turn your diagnostics on: – Go to catalog – Scroll to diagnosticON and hit enter until your screen says DONE Please help your teammates as we go through this problem

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Example problem – jot this info down before continuing to next slide A reaction A B is studied in order to determine the order of the reaction. a)Indicate the order of the reaction by writing the rate law b)Calculate the rate constant

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Data time (seconds)[A] 00.01000 10000.00625 18000.00476 28000.00370 36000.00313 Insert time into L1 of your calculator. Enter [A] into list 2. Continue to next slide when students have data entered.

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We need to compare time to [ ] to see if it’s zero order, but we also need to compare time to ln[ ] (first order) and time to 1/[ ] It’s all about staying organized: L1 = time L2 = [ ] L3 = ln[ ] L4 = 1/[ ] The quick trick to filling L3 is to scroll over and highlight L3. Then, type ln(L2). Hit enter and it will calculate everything for you. For L4, highlight L4 and type in 1/L2. Help your neighbor! Tell the sub when you’re ready

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We need to run 3 separate linear regressions, making note of the R 2 value each time. Reminder on linear regressions: – Stat, Calc, #4 – When this appears on your screen: LinReg(ax+b) type in the red portion: LinReg(ax+b)L1,L2 – Write down R 2 Do the linear regressions 2 more times (write down R 2 ), but make them look like this: – LinReg(ax+b)L1,L3 – LinReg(ax+b)L1,L4 Tell the sub when you have the 3 R 2 values, click on when the kids are ready

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Here’s how I keep myself organized Analyzing my results. Since the most linear set of data is time and 1/[ ], this indicates that the reaction is second order. Therefore, the rate law is: rate = k[A] 2 Now to solve for k….click on when the kids are ready.

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Refer back to your chart For a second order reaction, k=slope. Make sure the linear regression for L1 and L4 is still on your screen. If so, ‘a’ is the slope and is equal to k. k=0.0610 What units would it have? Rearrange the rate law to find out: k = rate/[A] 2, so k has units of s -1 ·M -1 So k = 0.0610 s -1 ·M -1 We’ve now answered both questions (rate law and k)!

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One last thing to add. These equations are from your yellow equation chart. Get that out now and fill these in. orderLinear graphk= Equation 0[ ] vs time-slope 1ln[ ] vs time-slope ln[A] t – ln[A] 0 = -kt 21/[ ] vs timeslope Find the version for 1/[ ] on your sheet and write it here [A] t means the concentration at time t (which is the time you would use for t). [A] 0 means the initial concentration (which you can get from time 0 in the data table)

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Let’s answer one last question about the example problem we’ve already been using What will the concentration of A be at 6215 seconds? Since it’s second order, use the equation your wrote down in your chart. – [A] t is the unknown – [A] 0 = 0.01000 (from time zero, look in your lists) – k=0.0610 – t=6215 – SOLVE for the unknown. I got: 0.00209 M

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Begin your homework! Packet #28, 29, 36 Acid Base Try 2 and 3 Monday-Wednesday

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Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.

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