temperature, 1.72 moles of A2 and 2.73 moles of B2 are added to a 14.0 L vessel, and allowed to come to equilibrium according to 2A₂B(g) 2A2(g) + B₂(g) At equilibrium 1.78 moles of A₂B are present. What is the equilibrium constant, K, for this reaction?

temperature, 1.72 moles of A2 and 2.73 moles of B2 are added to a 14.0 L vessel, and allowed to come to equilibrium according to 2A₂B(g) 2A2(g) + B₂(g) At equilibrium 1.78 moles of A₂B are present. What is the equilibrium constant, K, for this reaction?

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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Question

At a particular temperature, 1.72 moles of A2 and 2.73 moles of B2 are added to a
14.0 L vessel, and allowed to come to equilibrium according to
2A₂B(g) 2A2(g) + B2(g)
At equilibrium 1.78 moles of A₂B are present. What is the equilibrium constant, K,
for this reaction?

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Step 1: Defining equilibrium constant

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Step 2: Calculation for initial concentration of both the reactants

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Step 3: Calculation for equilibrium concentration of gas A2B

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Step 4: Formation of ICE table for the given reaction

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Step 5: Calculation for the value of equilibrium constant K

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