onsider the following equilibrium system: MnO4− + 4 H+ + 3 e− ⇌ MnO2(s) + 2 H2O(l) (a) Calculate the pEo value. (HINT: Consult this standard reduction potential table (b) Calculate the actual pE of a 50.0-L neutral aqueous solution containing 10.0 g of potassium permangante (KMnO4). Assume that only chemistry in the equilibrium system above determines the pE. (HINTS: In an equilibrium constant (K) or reaction quotient (Q) expression, pure solids and liquids behave has if they have values of 1. Concentrations in these expressions must be in mol L−1.)
onsider the following equilibrium system: MnO4− + 4 H+ + 3 e− ⇌ MnO2(s) + 2 H2O(l) (a) Calculate the pEo value. (HINT: Consult this standard reduction potential table (b) Calculate the actual pE of a 50.0-L neutral aqueous solution containing 10.0 g of potassium permangante (KMnO4). Assume that only chemistry in the equilibrium system above determines the pE. (HINTS: In an equilibrium constant (K) or reaction quotient (Q) expression, pure solids and liquids behave has if they have values of 1. Concentrations in these expressions must be in mol L−1.)
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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Chapter #10, Question #10-1:
Consider the following equilibrium system: MnO4− + 4 H+ + 3 e− ⇌ MnO2(s) + 2 H2O(l)
(a) Calculate the pEo value. (HINT: Consult this standard reduction potential table
(b) Calculate the actual pE of a 50.0-L neutral aqueous solution containing 10.0 g of potassium permangante (KMnO4). Assume that only chemistry in the equilibrium system above determines the pE. (HINTS: In an equilibrium constant (K) or reaction quotient (Q) expression, pure solids and liquids behave has if they have values of 1. Concentrations in these expressions must be in mol L−1.)
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