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Using the Le Chatelier's principle, predict the shift in the direction of the equilibrium position and changes that will be observed (e.g. color) in each of the following equilibria when the indicated condition is applied. 1. If heat is added to a phase change equation at equilibrium from solid to liquid, which way will the reaction proceed? 2. In this reaction: H2O) = H2O@) how could conditions be manipulated to create more H2O1)?

Using the Le Chatelier's principle, predict the shift in the direction of the equilibrium position and changes that will be observed (e.g. color) in each of the following equilibria when the indicated condition is applied. 1. If heat is added to a phase change equation at equilibrium from solid to liquid, which way will the reaction proceed? 2. In this reaction: H2O) = H2O@) how could conditions be manipulated to create more H2O1)?

Chemistry for Today: General, Organic, and Biochemistry
Chemistry for Today: General, Organic, and Biochemistry
9th Edition
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Chapter8: Reaction Rates And Equilibrium
Section: Chapter Questions
Problem 8.52E: Use Le Chteliers principle to predict the direction of the equilibrium shift in the following...
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Using the Le Chatelier's principle, predict the shift in the direction of the equilibrium position and changes that will be observed (e.g. color) in each of the following equilibria when the indicated condition is applied. 1. If heat is added to a phase change equation at equilibrium from solid to liquid, which way will the reaction proceed? 2. In this reaction: H2O@) = H2O(g) how could conditions be manipulated to create more H2O)?
Transcribed Image Text:Using the Le Chatelier's principle, predict the shift in the direction of the equilibrium position and changes that will be observed (e.g. color) in each of the following equilibria when the indicated condition is applied. 1. If heat is added to a phase change equation at equilibrium from solid to liquid, which way will the reaction proceed? 2. In this reaction: H2O@) = H2O(g) how could conditions be manipulated to create more H2O)?
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