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GIven that : HalfReactions Ered(V)

Cu2+(aq) + 2e- ------>Cu(s) +0.337

Pb2+(aq) + 2e- ------>Pb(s) -0.125

a) Calculate E cell for the reaction: Cu2+ (aq) + Pb (s)<----------> Cu (s) + Pb2+ (aq)

b) Calculate Delta G for the reaction (F = 9.65 x10^4 J/Vmol)

c) Determine the Keq value for the reaction

d)Using the Nernst equation, calculate the Ecell when [Pb2+] = 1.0 x10^-2 M and [Cu2+] =1.0 M

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Reid WolffLv2
6 Jun 2019
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Consider a Galvanic cell constructed from the following half cells, linked by a KCl salt bridge.

. an Al(s) electrode in 0.5 M Al2(SO4)3 solution

. a Pb(s) electrode in 1.0 M Pb(NO3)2 solution

Which electrode is the cathode?

Al

Pb

Al3+

Pb2+

1)Calculate forthe electrochemical cell below,

Pb(s) |PbSO4(s) | Pb2+(aq) Ag+(aq) | Ag(s)

given the following standard reduction potentials.

Ag+(aq) + e- ->Ag(s) E° = +0.799 V

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a) -1.954 V

b) -1.155 V

c) +0.443V

d) +1.155 V

2) Consider the following half- reactions:

Cu2+ (aq) + 2e- --> Cu(s)E = +0.34 V

Sn2+(aq) + 2e- --> Sn(s) E = -0.14 V

Fe2+(aq) +2e- --> Fe(s)E = -0.44 V

Al3+(aq) +3e- --> Al(s) E = -1.66 V

Mg2+(aq) + 2e---> Mg(s) E = -2.37 V

Which of the abovemetals or metal ions will reduce Fe2+ ?

a) Cu(s) andSn(s)

b) Cu2+(aq) andSn2+(aq)

c) Al3+(aq) andMg2+ (aq)

d) Al(s) andMg(s)

e) Sn(s) and Al3+(aq)

3) The following reaction occurs spontaneously

2H+ (aq) +Ca(s) --> Ca2+(aq) + H2(g)

Write a balanced recuction half-reaction-

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b) 2H+ (aq) --> H2(g) + 2e-

c) H2(g) --> 2H+(aq) + 2e-

d) Ca(s) + 2e- --> Ca2+(aq)

e) Ca(s) --> Ca2+(aq) + 2e-

A cell is set up with copper and lead electrodes in contact withCuSO4 (aq,1.0 M) and Pb (NO3)2 (aq, 1.0 M), respectively, at 25°C.The standard cell potential is 0.47 V for the reaction: Cu2+ + Pb--> Cu + Pb2+

If solid sodium sulfate is added to the Pb (NO3)2 solution, aprecipitate of PbSO4 will form. Using the Nerst equation to predicthow the cell potential will change.

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