Consider a galvanic cell constructed from the following half cells, linked by an external circuit and by a KCI salt bridge.an Al(s) electrode in 1.0 M Al(NO3)3 solutiona Pb(s) electrode in 1.0 M Pb(NO3)2 solutionStandard Reduction Potentialsat Standard States and 25°CHalf-reaction|E°(V).Pb (ag) + 2e → Pbo-0.13A1(e9) + 3e→ Alo-1.66(a) Write a half-reaction which occurs at the anode.(b) Write the half-reaction which occurs at the cathode(c) Write a balanced net ionic equation for the galvanic cell.(d) Calculate the value of E°cell(e) Write a cell diagram for the reaction occurring in this galvanic cell.

Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

Consider a galvanic cell constructed from the following half cells, linked by an external circuit and by a KCI salt bridge. an Al(s) electrode in 1.0 M Al(NO3)3 solution a Pb(s) electrode in 1.0 M Pb(NO3)2 solution Standard Reduction Potentials at Standard States and 25°C Half-reaction E(V) Pb (ag) + 2e →Pba Ala0) + 3e → Alo -0.13 -1.66 (a) Write a half-reaction which occurs at the anode. (b) Write the half-reaction which occurs at the cathode (c) Write a balanced net ionic equation for the galvanic cell.

Consider a galvanic cell constructed from the following half cells, linked by an external circuit and by a KCI salt bridge. an Al(s) electrode in 1.0 M Al(NO3)3 solution a Pb(s) electrode in 1.0 M Pb(NO3)2 solution Standard Reduction Potentials at Standard States and 25°C Half-reaction E(V) Pb (ag) + 2e →Pba Ala0) + 3e → Alo -0.13 -1.66 (a) Write a half-reaction which occurs at the anode. (b) Write the half-reaction which occurs at the cathode (c) Write a balanced net ionic equation for the galvanic cell.

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 76AP

See similar textbooks

Similar questions

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.
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)
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 reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 10-4M),Fe2+ (0.090 M)|Pt (c) AgBr(sat’d),Br- (0.037 M)|Ag
The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the tabulated standard potential of the silver half-reaction to find the standard reduction potential for the europium half-reaction.
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).