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Electrochemistry: Battery

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Wize High School Grade 12 Chemistry Textbook > Electrochemistry

Galvanic Cells

7 Activities

Given the following half cells, what is the maximum voltage of a battery that could be constructed?


Li(aq)++eβˆ’β†’Li(s)Eo=βˆ’3.04 VCe(aq)4++eβˆ’β†’Ce(s)3+Eo=1.44 VCo(aq)3++eβˆ’β†’Co(aq)2+Eo=1.82 V\begin{array}{llll}&Li^+_{(aq)}&+&e^{-}&\rightarrow&Li_{(s)}&&E^o=-3.04\ V\\ \\&Ce^{4+}_{(aq)}&+&e^{-}&\rightarrow&Ce^{3+}_{(s)}&&E^o=1.44 \ V \\ \\&Co^{3+}_{(aq)}&+&e^{-}&\rightarrow&Co^{2+}_{(aq)}&&E^o=1.82 \ V \end{array}


More Galvanic Cells Questions:
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.
Na(aq)++eβˆ’β†’Na(s)Eo=βˆ’2.71VNa^+_{(aq)} +e^- \to Na_{(s)} \hspace{40pt} E^o=-2.71V
Practice: Galvanic Cells
Construct a galvanic cell with the highest voltage given the following half reactions. Determine the voltage produced and express it in standard cell notation.
Na(aq)++eβˆ’β†’Na(s)Eo=βˆ’2.71VNa^+_{(aq)} +e^- \to Na_{(s)} \hspace{40pt} E^o=-2.71V
S2O8(aq)2βˆ’+2eβˆ’β†’2SO4(aq)2βˆ’Eo=2.01VS_2O_{8(aq)}^{2-} +2e^- \to 2SO_{4(aq)}^{2-} \hspace{20pt} E^o=2.01V
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.
Na(aq)++eβˆ’β†’Na(s)Eo=βˆ’2.71VNa^+_{(aq)} +e^- \to Na_{(s)} \hspace{40pt} E^o=-2.71V
Electrochemistry: Galvanic Cells
In a galvanic cell, oxidation occurs at the:
Electrochemistry: Galvanic Cell
In a zinc-lead cell the reaction is:
Pb2+(aq)+Zn(s)β†’Pb(s)+Zn2+(aq)       EΒ°=0.637VPb^{2+}\left(aq\right)+Zn\left(s\right)\to Pb\left(s\right)+Zn^{2+}\left(aq\right)\ \ \ \ \ \ \ E\degree=0.637V
Which of the following statements about this cell is FALSE?
Electrochemistry: Galvanic Cells
Construct a galvanic cell with the highest voltage given the following half reactions. Determine the voltage produced and express it in standard cell notation.
Na(aq)++eβˆ’β†’Na(s)Eo=βˆ’2.71VNa^+_{(aq)} +e^- \to Na_{(s)} \hspace{40pt} E^o=-2.71V
S2O8(aq)2βˆ’+2eβˆ’β†’2SO4(aq)2βˆ’Eo=2.01VS_2O_{8(aq)}^{2-} +2e^- \to 2SO_{4(aq)}^{2-} \hspace{20pt} E^o=2.01V
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: 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 halfβˆ’reactionEΒ°(V)πΆπ‘Ž2+(π‘Žπ‘ž)+2π‘’βˆ’β‡ŒπΆπ‘Ž(𝑠)βˆ’2.87π‘π‘Ž+(π‘Žπ‘ž)+π‘’βˆ’β‡Œπ‘π‘Ž(𝑠)βˆ’2.71𝐴𝑙3+(π‘Žπ‘ž)+3π‘’βˆ’β‡Œπ΄π‘™(𝑠)βˆ’1.66𝑀𝑛2+(π‘Žπ‘ž)+2π‘’βˆ’β‡Œπ‘€π‘›(𝑠)βˆ’1.18𝐢𝑒2+(π‘Žπ‘ž)+2π‘’βˆ’β‡ŒπΆπ‘’(𝑠)+0.15𝐴𝑔+(π‘Žπ‘ž)+π‘’βˆ’β‡Œπ΄π‘”(𝑠)+0.80\begin{array}{c:c}\rm Reduction\ half-reaction& EΒ° (V)\\ \hline πΆπ‘Ž^{2+} (π‘Žπ‘ž)+2 𝑒^βˆ’β‡ŒπΆπ‘Ž (𝑠)& -2.87\\ \hline π‘π‘Ž^+ (π‘Žπ‘ž)+𝑒^βˆ’β‡Œπ‘π‘Ž (𝑠)&-2.71\\ \hline 𝐴𝑙^{3+} (π‘Žπ‘ž)+3 𝑒^βˆ’β‡Œπ΄π‘™(𝑠) &-1.66\\ \hline 𝑀𝑛^{2+} (π‘Žπ‘ž)+2 𝑒^βˆ’β‡Œπ‘€π‘› (𝑠)&-1.18\\ \hline 𝐢𝑒^{2+} (π‘Žπ‘ž)+2 𝑒^βˆ’ β‡ŒπΆπ‘’ (𝑠) &+0.15\\ \hline 𝐴𝑔^+ (π‘Žπ‘ž)+𝑒^βˆ’ β‡Œπ΄π‘” (𝑠)&+0.80\end{array}
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)+3eβˆ’β‡ŒCr(s)Cr^{3+}(aq)+3e^-β‡ŒCr(s) EΒ°red=βˆ’0.74VEΒ°_{red}=-0.74V
Cu2+(aq)+2eβˆ’β‡ŒCu(s)Cu^{2+}(aq)+2e^-β‡ŒCu(s) EΒ°red=+0.34VEΒ°_{red}=+0.34V
A voltaic cell is constructed with an Sn/Sn2+ half-cell and a Zn/Zn2+ half-cell. The zinc electrode is negative.
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

Electrochemistry: Ksp calculations
Use the following reduction potentials to calculate the Ksp of La(OH)3(s)
La(OH)3(s)+3eβˆ’β†’La(s)+3 OH(aq)βˆ’Eo=βˆ’2.90VLa(aq)3++3eβˆ’β†’La(s)Eo=βˆ’2.379 V\begin{array}{llllll}&La(OH)_{3(s)}&+&3e-&\rightarrow& La_{(s)}&+&3\ OH^-_{(aq)}& &&E^o=-2.90 V \\ &La^{3+}_{(aq)}&+&3e^-&\rightarrow& La_{(s)}&&&&& E^o=-2.379\ V \end{array}