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A. One mole of acetic acid, CH3COOH, and 1 mole of ethanol, C2H5OH, were reacted in one- liter vessel and allowed to attain equilibrium at 25°C. The equilibrium mixture was then titrated with standard base and was found to contain 0.667 moles of acetic acid after the following reaction has taken place to form ethyl acetate and water. Supply the table and calculate the equilibrium constant (Kc) CH3COOH(soln) + C2H5OH(soln) C2H5OOCCHsoln) H2O (). Initial 1.000 M 1.000 M Concentration Change in Concentration Equilibrium Concentration -0.667 M 0.333 М

A. One mole of acetic acid, CH3COOH, and 1 mole of ethanol, C2H5OH, were reacted in one- liter vessel and allowed to attain equilibrium at 25°C. The equilibrium mixture was then titrated with standard base and was found to contain 0.667 moles of acetic acid after the following reaction has taken place to form ethyl acetate and water. Supply the table and calculate the equilibrium constant (Kc) CH3COOH(soln) + C2H5OH(soln) C2H5OOCCHsoln) H2O (). Initial 1.000 M 1.000 M Concentration Change in Concentration Equilibrium Concentration -0.667 M 0.333 М

Chemistry
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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III Calculations Involving the Equilibrium Constant A. One mole of acetic acid, CH3COOH, and 1 mole of ethanol, C2H5OH, were reacted in one- liter vessel and allowed to attain equilibrium at 25°C. The equilibrium mixture was then titrated with standard base and was found to contain 0.667 moles of acetic acid after the following reaction has taken place to form ethyl acetate and water. Supply the table and calculate the equilibrium constant (Kc) CH3COOH(soln) + C2H5OH(soln) C2H5OOCCHsoln). H2O (1) Initial 1.000 M 1.000 М Concentration Change in Concentration -0.667 M Equilibrium Concentration 0.333 M + 2NH3 (g), Ke = 2.4 x 10-3 at 1000K. If 0.30 mole B. For the reaction, 3H2 (g) + N2(g) H2, 0.10 mole N2, and 0.20 mole NH3 are placed in an empty 1.0-liter vessel at 1000K, toward which direction will the reaction proceed? %3D
Transcribed Image Text:III Calculations Involving the Equilibrium Constant A. One mole of acetic acid, CH3COOH, and 1 mole of ethanol, C2H5OH, were reacted in one- liter vessel and allowed to attain equilibrium at 25°C. The equilibrium mixture was then titrated with standard base and was found to contain 0.667 moles of acetic acid after the following reaction has taken place to form ethyl acetate and water. Supply the table and calculate the equilibrium constant (Kc) CH3COOH(soln) + C2H5OH(soln) C2H5OOCCHsoln). H2O (1) Initial 1.000 M 1.000 М Concentration Change in Concentration -0.667 M Equilibrium Concentration 0.333 M + 2NH3 (g), Ke = 2.4 x 10-3 at 1000K. If 0.30 mole B. For the reaction, 3H2 (g) + N2(g) H2, 0.10 mole N2, and 0.20 mole NH3 are placed in an empty 1.0-liter vessel at 1000K, toward which direction will the reaction proceed? %3D
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