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Na(aq)++e−→Na(s)Eo=−2.71VNa^+_{(aq)} +e^- \to Na_{(s)} \hspace{40pt} E^o=-2.71VNa(aq)++e−→Na(s)Eo=−2.71V
S2O8(aq)2−+2e−→2SO4(aq)2−Eo=2.01VS_2O_{8(aq)}^{2-} +2e^- \to 2SO_{4(aq)}^{2-} \hspace{20pt} E^o=2.01VS2O8(aq)2−+2e−→2SO4(aq)2−Eo=2.01V
I2(s)+2e−→2I(aq)−Eo=0.54VI_{2(s)}+2e^- \to 2I^-_{(aq)} \hspace{43pt} E^o=0.54VI2(s)+2e−→2I(aq)−Eo=0.54V
Ni(aq)2++2e−→Ni(s)Eo=−0.23VNi_{(aq)}^{2+} +2e^- \to Ni_{(s)} \hspace{35pt} E^o=-0.23VNi(aq)2++2e−→Ni(s)Eo=−0.23V
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Electrochemistry: Reduction potentials in a Galvanic Cell
Use the standard reduction potentials below to answer the following question: which metal could be used to create a sacrificial anode for an aluminum pipe?
Reduction half−reactionE°(V)𝐶𝑎2+(𝑎𝑞)+2𝑒−⇌𝐶𝑎(𝑠)−2.87𝑁𝑎+(𝑎𝑞)+𝑒−⇌𝑁𝑎(𝑠)−2.71𝐴𝑙3+(𝑎𝑞)+3𝑒−⇌𝐴𝑙(𝑠)−1.66𝑀𝑛2+(𝑎𝑞)+2𝑒−⇌𝑀𝑛(𝑠)−1.18𝐶𝑢2+(𝑎𝑞)+2𝑒−⇌𝐶𝑢(𝑠)+0.15𝐴𝑔+(𝑎𝑞)+𝑒−⇌𝐴𝑔(𝑠)+0.80\begin{array}{c:c}\rm Reduction\ half-reaction& E° (V)\\ \hline 𝐶𝑎^{2+} (𝑎𝑞)+2 𝑒^−⇌𝐶𝑎 (𝑠)& -2.87\\ \hline 𝑁𝑎^+ (𝑎𝑞)+𝑒^−⇌𝑁𝑎 (𝑠)&-2.71\\ \hline 𝐴𝑙^{3+} (𝑎𝑞)+3 𝑒^−⇌𝐴𝑙(𝑠) &-1.66\\ \hline 𝑀𝑛^{2+} (𝑎𝑞)+2 𝑒^−⇌𝑀𝑛 (𝑠)&-1.18\\ \hline 𝐶𝑢^{2+} (𝑎𝑞)+2 𝑒^− ⇌𝐶𝑢 (𝑠) &+0.15\\ \hline 𝐴𝑔^+ (𝑎𝑞)+𝑒^− ⇌𝐴𝑔 (𝑠)&+0.80\end{array}Reduction half−reactionCa2+(aq)+2e−⇌Ca(s)Na+(aq)+e−⇌Na(s)Al3+(aq)+3e−⇌Al(s)Mn2+(aq)+2e−⇌Mn(s)Cu2+(aq)+2e−⇌Cu(s)Ag+(aq)+e−⇌Ag(s)E°(V)−2.87−2.71−1.66−1.18+0.15+0.80
A voltaic cell is constructed with an Sn/Sn2+ half-cell and a Zn/Zn2+ half-cell. The zinc electrode is negative.
Write a balanced overall reaction for this cell
Draw a diagram of this cell, labeling electrodes with their charges and showing the direction of electron flow in the wire and anion/cation flow in the salt bridge
Choose the INCORRECT statement
Electrochemistry: Galvanic Cell
In a zinc-lead cell the reaction is:
Pb2+(aq)+Zn(s)→Pb(s)+Zn2+(aq) E°=0.637VPb^{2+}\left(aq\right)+Zn\left(s\right)\to Pb\left(s\right)+Zn^{2+}\left(aq\right)\ \ \ \ \ \ \ E\degree=0.637VPb2+(aq)+Zn(s)→Pb(s)+Zn2+(aq) E°=0.637V
Which of the following statements about this cell is FALSE?
Electrochemistry: Galvanic Cells
In a galvanic cell, oxidation occurs at the:
Electrochemistry: Ksp calculations
Use the following reduction potentials to calculate the Ksp of La(OH)3(s)
Electrochemistry: Battery
Given the following half cells, what is the maximum voltage of a battery that could be constructed?
Electrochemistry: Standard Reduction Potentials
A galvanic cell is constructed from chromium and copper electrodes immersed in aqueous solutions of Cr3+and Cu2+ respectively (half-reactions shown below).
Cr3+(aq)+3e−⇌Cr(s)Cr^{3+}(aq)+3e^-⇌Cr(s)Cr3+(aq)+3e−⇌Cr(s) E°red=−0.74VE°_{red}=-0.74VE°red=−0.74V
Cu2+(aq)+2e−⇌Cu(s)Cu^{2+}(aq)+2e^-⇌Cu(s)Cu2+(aq)+2e−⇌Cu(s) E°red=+0.34VE°_{red}=+0.34VE°red=+0.34V
Practice: Galvanic Cells
Galvanic Cell Practice
Construct a galvanic cell with the highest voltage given the following half reactions. Determine the voltage produced and express it in standard cell notation.
Write the cell notation for the voltaic (or galvanic) cell that incorporates the following redox reaction:
Al(s)+Cr(aq)3+→Al(aq)3++Cr(s)Al_{(s)}+Cr^{3+}_{(aq)} \to Al^{3+}_{(aq)}+Cr_{(s)}Al(s)+Cr(aq)3+→Al(aq)3++Cr(s)
Al3+ +3e -> Al(s) Eored=-1.66V
Write the cell notation for the voltaic cell that incorporates each of the following redox reactions:
Cu(aq)2++SO2(g)+2H2O(l)→Cu(s)+SO4(aq)2−+4H(aq)+Cu^{2+}_{(aq)}+SO_{2(g)}+2H_2O_{(l)} \to Cu_{(s)}+SO^{2-}_{4(aq)}+4H^+_{(aq)}Cu(aq)2++SO2(g)+2H2O(l)→Cu(s)+SO4(aq)2−+4H(aq)+