Using the standard reduction potentials., calculate the equilibrium constant for each of the fol-lowing reactions at 298 K:(a) Cu(s) + 2 Ag*(aq) → Cu² (aq) + 2 Ag(s)(b) 3 Ce**(aq) + Bi(s) + H2O(I) → 3 Ce* (aq) +BiO*(aq) + 2 H*(aq)(c) N,H3 (aq) + 4 Fe(CN) (aq) → Nz(8) +5H*(aq) + 4 Fe(CN),

Interpretation - To calculate the equilibrium constant using standard reduction potentials.

Answered: Using the standard reduction…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

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Chapter18: Electrochemistry

Section: Chapter Questions

Problem 150CP: Given the following two standard reduction potentials, solve for the standard reduction potential of...

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At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)
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Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)
An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.00 M separated by a porous disk from a compartment with a copper metal electrode immersed in a solution of 10.00 M NH3 that also contains 2.4 103 M Cu(NH3)42+. The equilibrium between Cu2+ and NH3 is: Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013 and the two cell half-reactions are: Assuming Ag+ is reduced, what is the cell potential at 25C?

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