SIMULATION Voltaic Cells Under Standard ConditionsOxidizingAgentReducingAgentElectrodePotential (V)CathodeAnodeBr₂(l) + 2 eHg2+(aq) + 2eHg22+(aq) + 2 eCu2+(aq) + 2eSn 4+ (aq) + 2e2 H30+(aq) + 2eSn2+(aq) + 2e->2 Br (aq)+1.08Hg()+0.855->2 Hg()+0.789->Cu(s)+0.337GibbsFreeEnergySn2+(aq)+0.15←H2(g) + 2 H2O(l)0.00Sn(s)-0.14Ni 2+(aq) + 2eCd2+(aq) + 2eMg2+(aq) + 2e->Ni(s)-0.25->Cd(s)-0.40Mg(s)-2.37Select Hg2+ as the oxidizing agent.What is the value of E° cathode?V

Remember that reduction always occur at the cathode.E°cathode = E°reductionFrom the table above, the…

Answered: SIMULATION Voltaic Cells Under Standard…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.18QAP

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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 voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
Calculate the electrode potentials for the following systems: (a) Cr2O72-(5.00 10-3 M),Cr3+(2.50 10-2 M),H+ (0.100 M)|Pt (b) UO22+(0.100 M),U4+ (0.200 M),H+ (0.600 M)|Pt
Which of the changes below will increase the voltage of the following cell? Co|Co2+(0.010M)H+(0.010M)|H2(0.500atm)|Pt (a) Increase the volume of COCl2 solution from 100 mL to 300 mL. (b) Increase [H+] from 0.010 M to 0.500 M. (c) Increase the pressure of H2 from 0.500 atm to 1 atm. (d) Increase the mass of the Co electrode from 15 g to 25 g. (e) Increase [CO2+] from 0.010 M to 0.500 M.
Find the potentials of the following electrochemical cell: Cd|Cd2+,M=0.10Ni2+,M=0.50|Ni
A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
The table below lists the cell potentials for the 10 possible galvanic cells assembled from the metals A. B. C. D. and E. and their respective 1.00 M 2+ ions in solution. Using the data in the table, establish a standard reduction potential table similar to Table 17-1 in the text. Assign a reduction potential of 0.00 V to the half-reaction that falls in the middle of the series. You should get two different tables. Explain why, and discuss what you could do to determine which table is correct. A(s)in A2+(aq) B(s)in B2+(aq) C(s)in V2+(aq) D(s)in D2+(aq) E(s)in E2+(aq) 0.28V 0.81V 0.13V 1.00V D(s)in D2+(aq) 0.72V 0.19V 1.13V C(s)in V2+(aq) 0.41V 0.94V B(s)in B2+(aq) 0.53V
Calculate the theoretical potential of each of the following cells. Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Pt|Cr3+(2.00 10-4M),Cr2+(1.50 10-3 M)||Pb2+ (5.60 0215 10-2M)|Pb (b) Hg|Hg22+(2.00 10-2 M)||H+(1.50 10-2 M),V3+ (2.00 10-2M),VO2+(3.00 10-3M)|Pt (e) Pt|Fe3+(3.00 10-2 M), Fe2+ (4.00 10-5M)||Sn2+ (3.50 10-2M), Sn4+ (5.50 10-4 M)|Pt

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