Chloride ions are added to the AglAg* half-cell of the cellAg|Ag*l|Cu²*|Cu to precipitate AgCI (s). The cell voltage is thenmeasured to be +0.072 V at 298 K. If [Cu2+] = 1.0 M in the Cu2+|Cu halfcell, what is [Ag*] in the Ag|Ag* half-cell? (First step: You will need touse the data in Table 17-1 to calculate E°cell.) Give your answer totwo significant figures.Ecell = E°cell - (0.0257 V/n) In(Q)E'cell = E°ox + E°red cidic Solution, [H+] = 1MCIO-(aq) + H2O + 2e-Lit(aq) + e-K+(aq) + e-Ba2+(aq) + 2e-Ca2+(aq) + 2e-Na+(aq) + e-Mg2+(aq) + 2e-Al3+(aq) + 3e-Mn2+(aq) + 2eZn2+(aq) + 2e-Cr3+(aq) + 3e-Fe2+(aq) + 2e-Cr3+(aq) + e-Cd2+(aq) + 2e-PBSO4(s) + 2e-TI+(aq) + e-Co2+(aq) + 2e-Ni2+(aq) + 2e-Agl(s) + e-Sn2+(aq) + 2e-Pb2+(aq) + 2e-2H+(aq) + 2e-AgBr(s) + e-S(s) + 2H+(aq) + 2e-Sn4+(aq) + 2e-SO.2-(aq) + 4H*(aq) + 2e-Efed (V)Li(s)→K(s)Ba(s)→Ca(s)Na(s)→Mg(s)Al(s)→Mn(s)→Zn(s)Cr(s)Fe(s)Cr2+(aq)Cd(s)-3.040Lithium is the strongest reducin-2.936-2.906-2.869-2.714-2.357-1.68-1.182-0.762-0.744-0.409-0.408-0.402Pb(s) + SO,2-(aq)TI(s)Co(s)Ni(s)Ag(s) + 1-(aq)Sn(s)Pb(s)-0.356-0.336->-0.282-0.236-0.152-0.141-0.127H2(g)Ag(s) + Br(aq)H2S(aq)Sn2+(aq)→SO2(g) + 2H2OCu*(aq)Cu(s)Cu(s)21-(aq)Fe2+(aq)2Hg(1)>Ag(s)Hg2+(aq)NO(g) + 2H20→Au(s) + 4CI-(aq)2Br(aq)RO = strongest oxidiz0.000R = strongest reduc0.0730.1440.154Cu2+(aq) + e-Cu2+(aq) +.2e-Cut(aq) + e-.2(s) + 2e-Fe3+ (aq).+ e-Hg2 2+(aq) + 2e-Ag+(aq) + e-2H92+(aq) + 2e-NO3-(aq) + 4H+(aq) + 3e-AuCla-(aq) + 3e-Br2(1) + 2e-O2(g) + 4H+(aq) + 4e-MnO2(s) + 4H+(aq) + 2e-Cr20,2-(aq) + 14H+(aq) + 6e-Cl2(g) + 2e-CIO3-(aq) + 6H*(aq) + 5e¬Au3+(ag) + Зе-MnO4 (aq) + 8H+(aq) + 5e-PbO2(s) + SO,2-(aq) + 4H*(aq) + 2e-H2O2(aq) + 2H+(aq) + 2e-Co3+ (aq) + e-F2(g) + 2e-0.155->0.1610.3390.5180.5340.7690.7960.7990.9080.9641.0011.0772H201.2291.229→MN2+(aq) + 2H20→2Cr3+(aq) + 7H20→2CI-(aq)Cb(g) + 3H20Au(s)Mn2+(aq) + 4H2OPbSO4(s) + 2H2O→2H20Co2+(aq)2F-(aq)1.331.3601.458ban1.4981.5121.6871.7631.9532.889Fluorine is the strongest cBasic Solution, [OH-] = 1MEfed (V)-0.891→Fe(s) + 20H-(aq)→H2(g) + 20H-(aq)Fe(OH)2(s) + OH-(aq)-0.828Fe(OH)2(s) + 2e-2H20 + 2e-Fe(OH)3(s) + e-S(s) + 2e-NO3-(ag) + 2H2O + 3e-NO3 (ag) + H2O + 2e-ClO4 (ag) + H2O + 2eO>(g) + 2H20 + 4e-CIo3 (ag) + 3H20+6e-0.547-0.445Lithium and fluorine ardous materials to work-0.140NO(g) + 40H-(aq)NO2 (aq) + 20H-(aq)ClO, (aq) + 20H-(aq)→4OH-(aq)CI-(aq) + 60H-(aq)CI-(aq) + 20H-(aq)0.0040.3980.4010.6140.890STANDARD17.2Increasing strength of oxidizing agentsIncreasing strength of reducing agents

Nernst Equation for Single Electrode Potential Ecell = E0 – [RT/nF] ln Q Where, Ecell = cell…

Chloride ions are added to the Ag|Ag* half-cell of the cell Ag|Ag*||Cu2|Cu to precipitate AgCl (s). The cell voltage is then measured to be +0.072 V at 298 K. If [Cu²*] = 1.0 M in the Cu2+|Cu half cell, what is [Ag*] in the Ag|Ag* half-cell? (First step: You will need to use the data in Table 17-1 to calculate E'cell.) Give your answer to two significant figures. Ecell = E°cell - (0.0257 V/n) In(Q) E'cell = E'ox + E°red

Chloride ions are added to the Ag|Ag* half-cell of the cell Ag|Ag||Cu2|Cu to precipitate AgCl (s). The cell voltage is then measured to be +0.072 V at 298 K. If [Cu²] = 1.0 M in the Cu2+|Cu half cell, what is [Ag] in the Ag|Ag half-cell? (First step: You will need to use the data in Table 17-1 to calculate E'cell.) Give your answer to two significant figures. Ecell = E°cell - (0.0257 V/n) In(Q) E'cell = E'ox + E°red

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 153CP: Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment...

See similar textbooks

Similar questions

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)
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?
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)
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.
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)
Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
What is the cell potential (Ecell) of a spontaneous cell that is run at 25C and contains [Cr3+] = 0.10 M and [Ag+] = 1.0 104 M?
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?
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 standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?