7) Consider the following reaction: liter mol-sec 2 HI(g) → H₂(g) + 12 (g) k = 0.0969. 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).
7) Consider the following reaction: liter mol-sec 2 HI(g) → H₂(g) + 12 (g) k = 0.0969. 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).
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![7) Consider the following reaction:
liter
mol-sec
2 HI(g) → H₂(g) + 12 (g)
k = 0.0969.
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 rate= rater, and assume this is a one-step mechanism (the
reactions shown have the correct molecularity).
Answer: 0.6, 0.06](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1077e877-4e25-45d6-8c49-9aaf109d8b6e%2F1062444f-a814-445d-ad1d-262289ac5905%2Fsp2hi7g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:7) Consider the following reaction:
liter
mol-sec
2 HI(g) → H₂(g) + 12 (g)
k = 0.0969.
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 rate= rater, and assume this is a one-step mechanism (the
reactions shown have the correct molecularity).
Answer: 0.6, 0.06
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