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Ch.14 - Chemical Kinetics

Chapter 14, Problem 37b

Consider the gas-phase reaction between nitric oxide and bromine at 273 C: 2 NO1g2 + Br21g2¡2 NOBr1g2. The following data for the initial rate of appearance of NOBr were obtained: Experiment 3no4 1M 2 3br2 4 1M 2 Initial Rate 1M,s2 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 (b) Calculate the average value of the rate constant for the appearance of NOBr from the four data sets.

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everyone. So we're giving the following reaction below In the initial right for their parents of C. Was measured. Were asked based on the data what is the average value of the rate? Counsel for the appearance of C. We know that the right law equation is right equals the rate constant construction A. For the power of X. And X. Is ordered with respect to a concentration of B. The power of why and why is the order with respect to be? We need to first determine the order with respect to A. And B. We have to find the right order for A. We're gonna use our 2nd and 4th experiment, 0.80-9 per second. Because the right concept from 0.041 smaller. R 0.024 Smalling the power of Y. We have 1.6059 mother per second. It was the right constant. From 0.082 Smalling the power of x. smaller part of why? And I was gonna cancel out and this as well. So we're left with 0.5. The power of X. X. It was one a. Its first border to find the right order for B. Use that 3rd and 5th experiments, You have 1.3230 mother per second. It was the right constant from 0.038. Waller. The power of x. to the power of Y. 5.29 20/s. Because the right concept from 0.038 smaller R. X. From 0.064 smaller part of Why? Yeah that's gonna cancel that. And this as well. 0.25 equals 0.5. They're part of why But why? It was two and B. The second order. And for our rate at the rate constant times contract in A. Which is first order sounds concentration of B. Which is second order. So that's gonna be squared. And now we can erase this to find our rate constant. It's gonna be right by by the concentration of A. As construction of the sport. So now we need to find the right concept for each government experiment one. Alright constant. 0.7442 per second. got about 0.038 Baller from 0.024 smaller square. We get 34,000 .37 Mueller. The negative power from second to the -1. Power for experiment two For the rate constant. And 1.6059 Mueller for a second. By by 0.082 smaller. 0.024 Smalling Square. You get 34,000 Solar to power come second to the make of one. Power for experiment three for the rate constant. We get 5.29-0 dollar per second. By by 0.038 smaller. 0.064 smaller square. I get 0.79 smaller to negative power from second to negative one Power Experiment for for the right constant 0.80-9 miles per second. five x 0.04. one smaller. From 0.024 smaller square. Get 33,998. What for smaller two mega to power from second to mega one. Power for experiment five for the right Carson We have 1.3230 mother per second By by 0.038 Moeller. 0.032 mother square. Get 33,000 999. Smalling to 90 power from 2nd to 91 power Before average That 34,000 0.37. That's 34,000. Like two sides. That's 33,000 0.79 plus 33,998 0.14 plus 33,999 0.79. Good Bye Bye five. So for the average We get 3.4 house into the four baller to the negative two. Power one second to the negative one. Power, thanks for watching my video and I hope it was up for
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Textbook Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl- + I- → OI- + Cl- . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4 (c) Calculate the rate when [OCl-] = 2.0 * 10-3 M and [I-] = 5.0 * 10 - 4 M.

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Textbook Question

The following data were measured for the reaction 

(b) What is the overall order of the reaction?

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Textbook Question

The following data were measured for the reaction 

(c) Calculate the rate constant with proper units?

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Textbook Question

Consider the reaction of peroxydisulfate ion 1S2O82-2 with iodide ion 1I - 2 in aqueous solution: S2O8 2 - 1aq2 + 3 I - 1aq2¡2 SO42 - 1aq2 + I3- 1aq2 At a particular temperature, the initial rate of disappearance of S2O82 - varies with reactant concentrations in the following manner: Experiment 3S2o8 24 1M 2 3I4 1M 2 Initial Rate 1M,s2 1 0.018 0.036 2.6 * 10-6 2 0.027 0.036 3.9 * 10-6 3 0.036 0.054 7.8 * 10-6 4 0.050 0.072 1.4 * 10-5 (a) Determine the rate law for the reaction and state the units of the rate constant.

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Textbook Question

(a) For the generic reaction A S B what quantity, when graphed versus time, will yield a straight line for a first-order reaction?

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Textbook Question
The decomposition of sodium bicarbonate (baking soda), NaHCO31s2, into Na2CO31s2, H2O1l2, and CO21g2 at constant pressure requires the addition of 85 kJ of heat per two moles of NaHCO3. (b) Draw an enthalpy diagram for the reaction.
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