Consider a voltaic cell represented by the following line notation: Mn (s) | Mn^2+ (aq) || ClO_2 (g) | ClO^-_2 (aq) | Pt (s) (a) Write the overall balanced chemical equation for the reaction. (b) Calculate E degree cell.
1) Calculate the standard emf (electromotive force) for a voltaic cell whose cell reaction is represented by the balanced equation.
2H2O(l) â H2(g) + H2O2(aq)
2) Calculate the standard cell potential for a galvanic cell whose cell reaction is represented by the balanced equation.
2Fe(s) + 3I2(s) â 2Fe3+(aq) + 6I-(aq)
St. Red. Pot. (V)
Fe3+/Fe
-0.04
I2/I-
0.54
3) For the voltaic cell shown, calculate the standard cell potential.
Pt(s) l H2O(l), H2O2(aq), H+(aq) ll H+(aq) l H2(g), Pt(s)
St. Red. Pot. (V)
H2O2/H2O
1.78
H+/H2
0
4)For the voltaic cell shown, calculate the standard cell potential.
Mn(s) l Mn2+(aq) ll F2(g) l F-(aq) l Pt(s)
St. Red. Pot. (V)
Mn2+/Mn
-1.18
F2/F-
2.87
5)For the galvanic cell shown, calculate the Eo.
Fe(s) l Fe2+(aq) ll Cd2+(aq) l Cd(s)
St. Red. Pot. (V)
Fe2+/Fe
-0.44
Cd2+/Cd
-0.40
6) The value for the standard emf of a voltaic cell described by the cell notation is 1.88 V. Determine the value (V) of the standard half cell potential for the F2/F- couple.
Au(s) l AuCl4-(aq), Cl-(aq) ll F2(g) l F-(aq) l Pt(s)