7) Consider the following reaction: liter mol-sec 2 HI(g) → H₂(g) + I2 (g) Initially, a flask contained HI at a concentration of 0.670 M. At equilibrium, the concentration of [HI] in the flask was 0.125 M. From this information, answer the following questions: a. What is the equilibrium constant for the above reaction? b. What is the rate constant for the reverse reaction? Note: remember that ratef=rater, and assume this is a one-step mechanism (the reactions shown have the correct molecularity). Answer: 0.6, 0.06 k = 0.0969.

7) Consider the following reaction: liter mol-sec 2 HI(g) → H₂(g) + I2 (g) Initially, a flask contained HI at a concentration of 0.670 M. At equilibrium, the concentration of [HI] in the flask was 0.125 M. From this information, answer the following questions: a. What is the equilibrium constant for the above reaction? b. What is the rate constant for the reverse reaction? Note: remember that ratef=rater, and assume this is a one-step mechanism (the reactions shown have the correct molecularity). Answer: 0.6, 0.06 k = 0.0969.

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

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 12E: Show that the complete chemical equation, the total ionic equation, and the net ionic equation for...

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