Half-Reaction, Addic SolutionPotential, E (volts)-3.045L"(aq) + eLi()K'(ag) + e K(s)Rb (aq) + eRb()Ba (aq) +2e- Ba(s)Sr (ag) + 2 e Sr(s)Ca (aq) +2 e Ca(s)Na (aq) + e Na()Mg "(aq) +2 e → Mg)H(+2e 2H (1)AP"(aq) +3 e Al(s)-2.925-2.925-2.90-2.89-2.87-2.7143D2.37-2.251.66Z (aq) + 4 e Zr)-1.53ZAS6) + 2 e Zn(x) + S (a4)-1.44-1.21CASG) + 2 e >Cd() + $ (a)V (aq) +2e V©)L.I8Mn (aq) + 2e Mn(s)1.181.01FeSts)C"(aq) + 2e >Cr(«).Zn (aq)+ 2 e →Zn(x)Cr"2e Fe(s) S (aq)0.91-0.7630.74(aq)+ 3e Cris)HgS() + 2 H (a4) +2 H0 USg)Ga (aq) + eGas)0.720.530.492 CO.()+211 aq) +2e (COOLD em)FeCr" (aq) + Cr (aq)CF (aq) + 2 e Cde)Sefe)+2 11 (aq 2e HSe2eFet)一040.410.4040.400356TI aq+TIG):0.340.28Co (aq) 2 e Cos)N og) +2x Ni)(SaF (ag) teSafs) F Go)Agl) e0.150140.1260,0%0,0000.10 [References]Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells3+(a) Cr(s) | Cr (aq) || Pd (aq) | Pd(s)2+2124(b) Zn(s) | Zn (ag) || Co (ag) | Co(s)24(© Ca(s), Cds(s) | S (aq) || Sn (ag) | Su[s)

Answered: Image /qna-images/answer/71983d7e-2934-433f-85d7-27458a04dea2.jpg

Answered: [References] Using values from the…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 84AP

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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)
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
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.

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[References] Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells 3+ 2+ (a) Cr(s) | Cr (aq) || Pd (aq) | Pd(s) 21 (b) Zn(s) | Zn (ag) || Co (aq) | Co(s) 24 (0 ca(s), Cds()|S (aq) || Sn (aq) | Su(s)