For the following voltaic cell (the concentrations of all metal ions are 1M) and the corresponding half reactions,Rh(ag) + 3e Rh(s)Cu*(aq)+e Cu(s)E = 0.80 VE' = 0.52 Vsalt bridge-CuRh* (49)Cu (ag)नवंIn what direction do the electrons flow in the external circuit?O from the Rh anode to the Cu cathodefrom the Rh cathode to the Cu anodefrom the Cu anode to the Rh cathodefrom the Cu cathode to the Rh anode* PreviousASUS

Answered: Image /qna-images/answer/e493d87a-d461-42c0-b617-e2a7a68641c2.jpg

Answered: For the following voltaic cell (the…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.19QAP

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Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
What is the voltage of a concentration cell of Cl ions where the concentrations are 1.045 and 0.085 M? What the spontaneous reaction?
Consider the standard galvanic cell based on the following half-reactions: Cu2++2eCuAg++eAg The electrodes in this cell are Ag(s) and Cu(s). Does the cell potential increase. decrease. or remain the same when the following changes occur to the standard cell? a. CuSO4(s) is added to the copper half-cell compartment (assume no volume change). b. NH3(aq) is added to the copper half-cell compartment (Hint: Cu2+ reacts with NH3, to form Cu(NH3)42+(aq).] c. NaCl(s) is added to the silver half .cell compartment (Hint: Ag+ reacts with Cl to form AgCl(s).] d. Water is added to both half-cell compartments until the volume or solution is doubled. e. The silver electrode is replaced with a platinum electrode
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
Calculate the theoretical potential of each of the following cells.Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Bi|BiO+ (0.0300 M),H+ (0.100 M)||I- (0.100 M), AgI(sat’d)|Ag (b) Zn|Zn2+(5.75 10-4M)||Fe(CN)64-(530 10-2 M),Fe(CN)63-(6.75 10-2M)|Pt (c) Pt,H2O (0.200 atm)|HCI(8.25 10-4M), AgCI(sat’d)| Ag
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
A solution at 25C contains 1.0 M Cd2+, 1.0 M Ag+, 1.0 M Au3+, and 1.0 M NiH2+ in the cathode compartment of an electrolytic cell. Predict the order in which the metals will plate out as the voltage is gradually increased.
What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and 0.750 M? What is the spontaneous reaction?
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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