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Calculate the voltage of each of the following cells. a) Fe(s)/Fe2+ (1.55 x 10-2 M)//Cu2+ (6.55 x 10-3 M)/Cu(s) b) Pt, H2 (0.255 bar)/HCl (4.55 x 10-4 M), AgCl (sat'd)/Ag Fe2+ +2e- = Fe   E0= -0.44 V Cu2+ + 2e- = Cu  E0= 0.337 V Ag+ + e- = Ag   E0= 0.799 V AgCl(s) + e- = Ag(s) + Cl-  E0= 0.222 V 2H+ + 2e- = H2   E0= 0.000 V

Calculate the voltage of each of the following cells. a) Fe(s)/Fe2+ (1.55 x 10-2 M)//Cu2+ (6.55 x 10-3 M)/Cu(s) b) Pt, H2 (0.255 bar)/HCl (4.55 x 10-4 M), AgCl (sat'd)/Ag Fe2+ +2e- = Fe   E0= -0.44 V Cu2+ + 2e- = Cu  E0= 0.337 V Ag+ + e- = Ag   E0= 0.799 V AgCl(s) + e- = Ag(s) + Cl-  E0= 0.222 V 2H+ + 2e- = H2   E0= 0.000 V

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 50QRT
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Calculate the voltage of each of the following cells.

a) Fe(s)/Fe2+ (1.55 x 10-2 M)//Cu2+ (6.55 x 10-3 M)/Cu(s)

b) Pt, H2 (0.255 bar)/HCl (4.55 x 10-4 M), AgCl (sat'd)/Ag

Fe2+ +2e- = Fe   E0= -0.44 V

Cu2+ + 2e- = Cu  E0= 0.337 V

Ag+ + e- = Ag   E0= 0.799 V

AgCl(s) + e- = Ag(s) + Cl-  E0= 0.222 V

2H+ + 2e- = H2   E0= 0.000 V

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