n a kinetic experiment a chemist places crystals of iodine in closed reaction vessel. She then introduces a given quantity of hydrogen gas, and obtains data to calculate the rate of hydrogen iodide formation. In a second experiment, she uses the same amounts ofjodine and hydrogen, but she first warms the flask to 130°C, a temperature above the sublimation point of iodine. at higher rate? State the rationale behind your answer. which of these two experiments does the reaction proceed wing kinctic data Ime (hours)

n a kinetic experiment a chemist places crystals of iodine in closed reaction vessel. She then introduces a given quantity of hydrogen gas, and obtains data to calculate the rate of hydrogen iodide formation. In a second experiment, she uses the same amounts ofjodine and hydrogen, but she first warms the flask to 130°C, a temperature above the sublimation point of iodine. at higher rate? State the rationale behind your answer. which of these two experiments does the reaction proceed wing kinctic data Ime (hours)

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 10E: In the PhET Reactions tab to observe how multiple atoms and molecules interact under varying...

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Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.
In the PhET Reactions tab to observe how multiple atoms and molecules interact under varying conditions. Select a molecule to pump into the chamber. Set the initial temperature and select the current amounts of each reactant. Select Show bonds under Options. How is the rate of the reaction affected by concentration and temperature?
A proposed mechanism for the gas-phase chlorination of methane is Cl2+CH4CH4Cl+ClCH4ClCH3+HClCH3+Cl2CH3Cl+ClCl+CH4CH3+HCl Suppose the first step is the RDS. What is the expected rate law in terms of the original reactants, Cl2 and CH4? How would you determine if this mechanism might be a potentially correct or, for that matter, a potentially incorrect one?
At low temperatures, the rate law for the reaction CO(g)+NO2(g)CO2(g)+NO(g)is as follows: rate=(constant)[ NO2 ]2. Which of the following mechanisms is consistent with the rate law? (a) CO+NO2CO2+NO(b) 2NO2N2O4(fast) N2O4+2CO2CO2+2NO(slow) (c) 2NO2NO3+NO(slow) NO3+CONO2+CO2(fast) (d) 2NO22NO+O2(slow) O2+2CO2CO2(fast)
11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
The hypothetical reaction X(g)+12Y(g)productsis first-order in X and second-order in Y. The rate of the reaction is 0.00389 mol/L min when [X] is 0.150 M and [Y] is 0.0800 M. (a) What is the value for k? (b) At what concentration of [Y] is the rate 0.00948 mol/L min and [X] is 0.0441 M? (c) At what concentration of [X] is the rate 0.0124 mol/L min and [ Y ]=2[ X ]?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
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Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
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