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4. The following reaction takes place: A₂B ⇒ 2A + B + heat. If 3.00 moles of A₂B are added into a 1.00 L container, it is found that 27.0 % of the reactant dissociates to reach equilibrium. Create an ICE table and solve for the Keg of this reaction. Note: Show all calculations, follow the rules of significant figures, and box your final answer.

4. The following reaction takes place: A₂B ⇒ 2A + B + heat. If 3.00 moles of A₂B are added into a 1.00 L container, it is found that 27.0 % of the reactant dissociates to reach equilibrium. Create an ICE table and solve for the Keg of this reaction. Note: Show all calculations, follow the rules of significant figures, and box your final answer.

Chemistry
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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24. The following reaction takes place: A₂B ⇒ 2A + B + heat. If 3.00 moles of A₂B are added into a 1.00 L container, it is found that 27.0 % of the reactant dissociates to reach equilibrium. Create an ICE table and solve for the Keg of this reaction. Note: Show all calculations, follow the rules of significant figures, and box your final answer.
Transcribed Image Text:24. The following reaction takes place: A₂B ⇒ 2A + B + heat. If 3.00 moles of A₂B are added into a 1.00 L container, it is found that 27.0 % of the reactant dissociates to reach equilibrium. Create an ICE table and solve for the Keg of this reaction. Note: Show all calculations, follow the rules of significant figures, and box your final answer.
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