Given the following equilibrium constants at 427°C:O₂(g) + 4Na(1) 2Na₂O(s)O₂(g) + 2Na(1) 2NaO(g)O₂(g) + 2Na(1) ⇒ Na₂O₂(s)O₂(g) + Na(1) NaO₂ (s)2.00×10-¹2K₁ = 2.50x1049You are correct.Your receipt no. is 153-9292 ?K₂ = 2.50×10⁹What would be the value of the equilibrium constant for each of the following reactions, at 427°C?K3 = 2.00×10282Na₂O(s) +O₂(g) = 2NaO(g) + Na₂O₂(s)Submit Answer Tries 0/99K4 = 3.33x1013Previous TriesNaO(g) + NaO₂(s) Na₂O(s) + O₂(g)

Answered: Image /qna-images/answer/649d089c-4b61-4138-9da9-f2da71f611e0.jpg

Given the following equilibrium constants at 427°C: O₂(g) + 4Na(1) 2Na₂O(s) K₁ = O₂(g) + 2Na(1) 2NaO(g) O₂(g) + 2Na(1) Na₂O₂(s) O₂(g) + Na(1) NaO₂ (s) 2.50×1049 K₂ = 2.50x10⁹ 2.00×10-12 K3 = 2.00×1028 K4 = 3.33x1013 What would be the value of the equilibrium constant for each of the following reactions, at 427°C? 2Na₂O(s) + O₂(g) 2NaO(g) + Na₂O₂(s)

Given the following equilibrium constants at 427°C: O₂(g) + 4Na(1) 2Na₂O(s) K₁ = O₂(g) + 2Na(1) 2NaO(g) O₂(g) + 2Na(1) Na₂O₂(s) O₂(g) + Na(1) NaO₂ (s) 2.50×1049 K₂ = 2.50x10⁹ 2.00×10-12 K3 = 2.00×1028 K4 = 3.33x1013 What would be the value of the equilibrium constant for each of the following reactions, at 427°C? 2Na₂O(s) + O₂(g) 2NaO(g) + Na₂O₂(s)

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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