Consider the equilibrium between molecular iodine and atomic iodine in the gaseous state. For this endothermic reaction at 727°C, Kc = 3.8 x 10-5. a. Are reactants or products favored at 727°C? How do you know? b. Which way will the reaction shift (toward reactants or products?) to reach equilibrium if the reaction vessel (at 727°C) contains 1.0 M I2 (g) and 0.2 M I(g)? How do you know? c. What is one change you could make to shift the reaction toward products? Why/how does that change work?
Consider the equilibrium between molecular iodine and atomic iodine in the gaseous state. For this endothermic reaction at 727°C, Kc = 3.8 x 10-5. a. Are reactants or products favored at 727°C? How do you know? b. Which way will the reaction shift (toward reactants or products?) to reach equilibrium if the reaction vessel (at 727°C) contains 1.0 M I2 (g) and 0.2 M I(g)? How do you know? c. What is one change you could make to shift the reaction toward products? Why/how does that change work?
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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Consider the equilibrium between molecular iodine and atomic iodine in the gaseous state. For this endothermic reaction at 727°C, Kc = 3.8 x 10-5.
a. Are reactants or products favored at 727°C? How do you know?
b. Which way will the reaction shift (toward reactants or products?) to reach equilibrium if the reaction vessel (at 727°C) contains 1.0 M I2 (g) and 0.2 M I(g)? How do you know?
c. What is one change you could make to shift the reaction toward products? Why/how does that change work?
Transcribed Image Text:I2(g) = 21(g)
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