The gas phase reaction of iodine with silane takes place according to a second-order reaction: I2(9) +SiH4(9) HI(g) +SiH3I(9) The activation energy is Ea = 83.2 kJ mol-¹. At 271°C, the reaction rate constant is 3.73 L mol-1 s-1. (a) Calculate the Arrhenius factor A for this reaction. (b) Calculate the rate constant for this reaction at 253°C. L mol-1 s-1 L mol-1 s-1

The gas phase reaction of iodine with silane takes place according to a second-order reaction: I2(9) +SiH4(9) HI(g) +SiH3I(9) The activation energy is Ea = 83.2 kJ mol-¹. At 271°C, the reaction rate constant is 3.73 L mol-1 s-1. (a) Calculate the Arrhenius factor A for this reaction. (b) Calculate the rate constant for this reaction at 253°C. L mol-1 s-1 L mol-1 s-1

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The gas phase reaction of iodine with silane takes place according to a second-order reaction:
I2(9) +SiH4(9) HI(g) +SiH3I(g)
The activation energy is Ea= 83.2 kJ mol-¹. At 271°C, the reaction rate constant is 3.73 L
mol-1 s-1.
(a) Calculate the Arrhenius factor A for this reaction.
(b) Calculate the rate constant for this reaction at 253°C.
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