Use the data in Standard Electrode (Half-Cell) Potentials to calculate equilibrium constants for the following reactions. Assume 298.15 K if no temperature is given. (a) AgCl(s) = Ag*(aq) + Cl (aq) (b) CdS(s) = Cd²+(aq) + S²-(ag) at 377 K (c) Hg2+ (aq) + 4Br" (aq) = [HBr]?- (aq) (d) H2O(1) = + (aq) + OH(aq) at 25°C %3D

Use the data in Standard Electrode (Half-Cell) Potentials to calculate equilibrium constants for the following reactions. Assume 298.15 K if no temperature is given. (a) AgCl(s) = Ag*(aq) + Cl (aq) (b) CdS(s) = Cd²+(aq) + S²-(ag) at 377 K (c) Hg2+ (aq) + 4Br" (aq) = [HBr]?- (aq) (d) H2O(1) = + (aq) + OH(aq) at 25°C %3D

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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