A. Using the Le Chatelier's principle, predict the shift in the direction of the equilibriumposition and changes that will be observed (e.g. color) in each of the following equilibriawhen the indicated condition is applied.|1. Ifheat is added to a phase change equation at equilibrium from solid to liquid, whichway will the reaction proceed?2. In this reaction:H2Om = H2Ohow could conditions be manipulated to create more H2Qa?3. Which side is heat on in this reaction (photosynthesis):6COX + 6H2O@= C¢H12O620) + 60z)4. Heat + Co+Ca+ 4 Claq) = COC4 ²- caq) when the equilibrium mixture is cooled.(exothermic)pinkcolorlessblue5. Fet)6SCNa)- Fe(SCN)6 *w when Fe³+ is added to the equilibriummixture.browncolorlessred

A. 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: H:Om = H2O , how could conditions be manipulated to create more H:Qn? 3. Which side is heat on in this reaction (photosynthesis): 6COX + 6H2O¤ = C&H12O630) + 602

A. 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: H:Om = H2O , how could conditions be manipulated to create more H:Qn? 3. Which side is heat on in this reaction (photosynthesis): 6COX + 6H2O¤ = C&H12O630) + 602

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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I Review | Constants | Periodic Table Part B When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K. The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: The following system is at equilibrium:A(s) + 4B(g) = C(g)Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help If a stress is applied to a reaction mixture at equilibrium,…
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