A cvg.cengagenow.comndTap - Cengage Learni.CoursesTransfer Course Equivalen.HomepageOWLV2 | Online teaching a..[Review Topics)[References]Use the References to access important values if needed for this question.Use standard reduction potentials to calculate the equilibrium constant for the reaction:Co2*(aq) + Hg(1)– Co(s) + Hg²*(aq)Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.Equilibrium constant:AG° for this reaction would bethan zero.Submit AnswerRetry Entire Group9 more group attempts remainingPreviEmail InstrCengage Learning | Cengage Technical Support

Solution Co2+(aq) + Hg(l) → Co (g) + Hg2+(aq)EoCo2+/Co=-0.28 VEoHg/Hg2+= -0.85 vEocell=Eored-…

cvg.cengagenow.com engage Learni. Courses Transfer Course Equivalen. OWLV2 | Online teaching Homepage [Review Topics] [References) Use the References to access important values if needed for this question. e standard reduction potentials to calculate the equilibrium constant for the reaction: 2+ Co2*(aq) + Hg(1)→ Co(s) + Hg²*(aq) nt: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.

cvg.cengagenow.com engage Learni. Courses Transfer Course Equivalen. OWLV2 | Online teaching Homepage [Review Topics] [References) Use the References to access important values if needed for this question. e standard reduction potentials to calculate the equilibrium constant for the reaction: 2+ Co2(aq) + Hg(1)→ Co(s) + Hg²(aq) nt: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 160MP

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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)?
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
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In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
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Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)