Some standard electrode potentials includeCut + e- → Cu (s) EO = 0.520 VCu²+ + e- → Cut Eº = 0.159 VCu2+ + 2e- → Cu (s)Eº = 0.340 V[Cu(CN)2] EO = 1.12 VUse the information above to calculate the formation constant for [Cu(CN)2], whichis the equilibrium constant for the reaction:Cu2+ + 2CN + e-Cut + 2CN [Cu(CN)2]→4Include two significant figures in your answer.Note: Your answer is assumed to be reduced to the highest power possible.Your Answer:x10

Here, reduction potential different redox processes are given and we have to use to establish the…

Some standard electrode potentials include Cut + e- → Cu (s) E° = 0.520 V Cu2+ + e- → Cut Eº = 0.159 V Cu2+ + 2e- → Cu (s) Eº = 0.340 V Cu2+ + 2CN + e- → [Cu(CN)₂] EO = 1.12 V Use the information above to calculate the formation constant for [Cu(CN)₂], which is the equilibrium constant for the reaction: Cut + 2CN [Cu(CN)₂] Include two significant figures in your answer. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10

Some standard electrode potentials include Cut + e- → Cu (s) E° = 0.520 V Cu2+ + e- → Cut Eº = 0.159 V Cu2+ + 2e- → Cu (s) Eº = 0.340 V Cu2+ + 2CN + e- → [Cu(CN)₂] EO = 1.12 V Use the information above to calculate the formation constant for [Cu(CN)₂], which is the equilibrium constant for the reaction: Cut + 2CN [Cu(CN)₂] Include two significant figures in your answer. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10

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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Calculate the cell potential, E, for the given reactions at 25.00 "C using the ion concentrations provided. Then, determine if th cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E). Pt(s) + Fe²(aq) = P² (aq) + Fe(s) [Fe²*1 = 0.0064 M E= incorrect -4761 E= Cu(s) + 2 Ag* (aq) = Cu² (aq) + 2 Ag(s) |Cu²+1 = 0.027 M Ag1=0.027 M E [P1²*1 = 0.067 M Co² (aq) + Ti (aq) — Co¹ (aq) + Ti² '(aq) Co²1 = 0.055 M Co= 0.030 M ITP 1 = 0.0070 M T² = 0.0107 M mam V The cell is not spontaneous spontaneous. The cell is spontaneous not spontaneous. incorrect The cell is spontaneous not spontaneoux.
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