At 2300 K, the equilibrium constant for the formation of NO (g), is K = 1.7 x 10-3 . N2 (g) + O2 (g) NO 2 NO (g) (a) The analysis shows that the concentrations of N2 and O2 are both 0.25 mol L-1, and that of NO is 0.0042 mol L-1, under certain conditions. Is the system in balance? In case affirmative or negative, substantiate your answer. (b) If the system is not in equilibrium, in which direction should the reaction proceed? (c) When the system is in equilibrium, what are the equilibrium concentrations?
At 2300 K, the equilibrium constant for the formation of NO (g), is K = 1.7 x 10-3 . N2 (g) + O2 (g) NO 2 NO (g) (a) The analysis shows that the concentrations of N2 and O2 are both 0.25 mol L-1, and that of NO is 0.0042 mol L-1, under certain conditions. Is the system in balance? In case affirmative or negative, substantiate your answer. (b) If the system is not in equilibrium, in which direction should the reaction proceed? (c) When the system is in equilibrium, what are the equilibrium concentrations?
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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At 2300 K, the equilibrium constant for the formation of NO (g), is K = 1.7 x 10-3
.
N2 (g) + O2 (g) NO 2 NO (g)
(a) The analysis shows that the concentrations of N2 and O2 are both 0.25 mol L-1, and that of
NO is 0.0042 mol L-1, under certain conditions. Is the system in balance? In case
affirmative or negative, substantiate your answer.
(b) If the system is not in equilibrium, in which direction should the reaction proceed?
(c) When the system is in equilibrium, what are the equilibrium concentrations?
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