Historically, chromium (Cr) has been used in numerous industrial processes, including leather tanning and metal plating operations. In these applications, if the water is mildly acidic, the Cr is typically present as bichromate (HCrO4) and/or dichromate (Cr2O72-) ions. These ions can be interconverted by the reaction: Cr₂O7²- + H₂O The standard Gibbs energies of formation of HCrO4, Cr₂O7², and H₂O are -764.8, -1301, and -237.18 kJ/mol, respectively. Compute the equilibrium constant for the conversion of HCrO4 to Cr₂O7²-. 2HCrO4
Historically, chromium (Cr) has been used in numerous industrial processes, including leather tanning and metal plating operations. In these applications, if the water is mildly acidic, the Cr is typically present as bichromate (HCrO4) and/or dichromate (Cr2O72-) ions. These ions can be interconverted by the reaction: Cr₂O7²- + H₂O The standard Gibbs energies of formation of HCrO4, Cr₂O7², and H₂O are -764.8, -1301, and -237.18 kJ/mol, respectively. Compute the equilibrium constant for the conversion of HCrO4 to Cr₂O7²-. 2HCrO4
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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