The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=74.0 kJ/mol. If the rate constant of this -1 reaction is 1.6 × 10² M¹s at 295.0 °C, what will the rate constant be at 387.0 °C? Round your answer to 2 significant digits. -1 1 k= ・M²¹. X S ? ·S

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=74.0 kJ/mol. If the rate constant of this -1 reaction is 1.6 × 10² M¹s at 295.0 °C, what will the rate constant be at 387.0 °C? Round your answer to 2 significant digits. -1 1 k= ・M²¹. X S ? ·S

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 69E: The activation energy for the reaction NO2(g)+CO(g)NO(g)+CO2(g) is 125 kJ/mol, and E for the...

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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.
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Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
A catalyst reduces the activation energy of a reaction from 215 to 206 kJ. By what factor would you expect the reaction-rate constant to increase at 25 C? Assume that the pre-exponential term (A) is the same for both reactions. (Hint: Use the formula ln k = ln A Ea/RT.)
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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.