If we represent the equilibrium as: 2 NO2(g)= N½0¼(g) We can conclude that: |1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. | 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. |3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

If we represent the equilibrium as: 2 NO2(g)= N½0¼(g) We can conclude that: |1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. | 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. |3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

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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C2. Subject Chemistry
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Calculating an equilibrium composition...
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