Part AA certain first-order reaction has a rate constant of 3.00 x 102s at 19 °C. What is the value of k at 61 °C if E, -76.5 kJ/mol ?Express your answer in reciprocal seconds to three significant figures.15. ΑΣΦΑk=SubmitPart BBequest AnswerSubmitAnother first-order reaction also has a rate constant of 3.00 x 102s¹ at 19°C. What is the value of k at 61 "Cif E₂-131 kJ/mol ?Express your answer in reciprocal seconds to three significant figures.15. ΑΣΦΑ?Request Answer?8-1

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Part A A certain first-order reaction has a rate constant of 3.00 x 10-2s¹ at 19 °C. What is the value of k at 61 °C i E, = 76.5 kJ/mol ? Express your answer in reciprocal seconds to three significant figures. 197| ΑΣΦ Submit Bequest Answer Part B Submit ? Another first-order reaction also has a rate constant of 3.00 x 10 at 19 °C. What is the value of k at 61 "C# E₂-131 kJ/mol? Express your answer in reciprocal seconds to three significant figures. 195] ΑΣΦΑ Request Answer 8 ?

Part A A certain first-order reaction has a rate constant of 3.00 x 10-2s¹ at 19 °C. What is the value of k at 61 °C i E, = 76.5 kJ/mol ? Express your answer in reciprocal seconds to three significant figures. 197| ΑΣΦ Submit Bequest Answer Part B Submit ? Another first-order reaction also has a rate constant of 3.00 x 10 at 19 °C. What is the value of k at 61 "C# E₂-131 kJ/mol? Express your answer in reciprocal seconds to three significant figures. 195] ΑΣΦΑ Request Answer 8 ?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 75E: One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a...

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The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
Ammonium cyanate, NH4NCO, rearranges in water to give urea, (NH2)2CO. NH4NCO(aq) (NH2)2CO(aq) Using the data in the table: (a) Decide whether the reaction is first-order or second-order. (b) Calculate k for this reaction. (c) Calculate the half-life of ammonium cyanate under these conditions. (d) Calculate the concentration of NH4NCO after 12.0 hours.
The decomposition of azomethane, (CH3)2N2, to nitrogen and ethane gases is a first-order reaction, (CH3)2N2(g)N2(g)+C2H6(g). At a certain temperature, a 29-mg sample of azomethane is reduced to 12 mg in 1.4 s. (a) What is the rate constant k for the decomposition at that temperature? (b) What is the half-life of the decomposition? (c) How long will it take to decompose 78% of the azomethane?
The initial concentration of the reactant in a tirst-order reaction A —» products is 0.64 rnol/L and the half-life is 30.0 s. Calculate the concentration of the reactant exactly 60 s after initiation of the reaction. How long would it take for the concentration of the reactant to drop to one-eighth its initial value? How long would it take for the concentration of the reactant to drop to 0.040 mol/L?
Would the slope of a ln(k) versus 1/T plot (with temperature in kelvin) for a catalyzed reaction be more or less negative than the slope of the ln(k) versus 1/T plot for the uncatalyzed reaction? Explain. Assume both rate laws are first-order overall.
For a first order gas phase reaction A products, k = 7.2 104s1 at 660. K and k = 1.7 102s1 at 720. K. If the initial pressure of A is 536 torr at 295C, how long will it take for the pressure of A to decrease to 268 torr?