Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H+ (aq) + Hg(!) → H2 (s) + Hg²+(aq) From the table of standard reduction potentials: E/H₂ E = 0.855 V Hg2+/Hg = =0.000 V, Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AG° for this reaction would be than zero.

Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H+ (aq) + Hg(!) → H2 (s) + Hg²+(aq) From the table of standard reduction potentials: E/H₂ E = 0.855 V Hg2+/Hg = =0.000 V, Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AG° for this reaction would be than zero.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.44QE: For each of the reactions, calculate E from the table of standard potentials, and state whether the...

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