Consider the Daniell battery. Determine how the voltage changes over time, E(t), if the battery is run at 50mA, using a starting concentration of [ZnSO4] and [CuSO4] of 1.00M in 1.000L. Remember that the charge (in Coulombs) for a mole of electrons is equal to Faraday's constant. (Using the table below)
Plot the function E(t) versus time.
Reaction Ag+ + e -> Ag
Ag2+ + e -> Ag*
AgBr + e -> Ag + Br
AgCl + e -> Ag + Cl
AgCN + e -> Ag + CN
AgF + e -> Ag + F
Ag4[Fe(CN)6] + 4e -> 4Ag + [Fe(CN)6]4
AgI + e -> Ag + I
AgNO + e -> Ag+ + NO
Al3+ + 3e -> Al
Au* + e -> Au
E(V)
Reaction Au3+ + 2e- -> Au*
nV _++nV
AuBr2 + e -> Au + 2Br
AuCl4 + 3e -> Au + 4Cl
Ba2+ + 2e- -> Ba
Be2+ + 2e -> Be
E(V)
0.7996
1.980
0.07133
0.22233
1.401
1.498
0.959
1.002
2.912
1.847
0.20
1.0873
0.761
3.80
2.868
0.017
0.779
0.1478
0.15224
0.564
1.662
1.692
Br2(aq) + 2e -> 2Br
BrO + H2O + 2e -> Br + 2OH
Ca* + e -> Ca
Ca2+ + 2e- -> Ca