Electrochemical Cells
- Page ID
- 283128
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)1.) Consider this overall redox process: Cu2+(aq)+Ba(s)→Cu(s)+Ba2+(aq)
a.) Split the reaction into half reactions and determine their standard reduction potentials. Indicate which would be the anode and cathode.
b.) Construct a cell diagram.
c.) Give the line notation for this cell.
d.) Calculate E°cell, the standard cell potential, which is given by E°red - E°ox.
2.) Consider this overall redox process: Al(s)+Sn2+(aq)→Al3+(aq)+Sn(s)
a.) Split the reaction into half reactions and determine their standard reduction potentials. Indicate which would be the anode and cathode.
b.) Construct a cell diagram.
c.) Give the line notation for this cell.
d.) Calculate E°cell.
3.) Consider a galvanic cell with Zn(s) and 0.25 M Zn(NO3)2(aq) in one compartment and Cu(s) and 0.25 M Cu(NO3)2(aq) in the other compartment.
a.) Give the half-reactions and their standard reduction potentials.
b.) Give the net, overall cell reaction and the standard cell potential:
c.) Now calculate the overall cell potential at the specific concentrations given. You’ll need to use the Nernst equation: Ecell = Eocell – (0.0592/n)log Q
d.) What would be the cell potential if the concentration of Zn(NO3)2 was increased to 2.5 M?
4.) Consider a voltaic cell with Cr(s) and Cr3+(aq) in one compartment and Zn(s) and Zn2+(aq) in the other compartment.
a.) Draw and label a diagram of this cell.
b.) Calculate the standard cell potential for the overall reaction.
c.) If zinc is the anode and [Cr3+] = 0.010 M, what must the [Zn2+] be in order to achieve 0.050V?
5.) A Zn/Zn2+ half-cell was coupled to a hydrogen electrode in which PH2 = 1 bar. The [Zn2+] in the anode compartment was 0.10 M and the cell potential was 0.542 V. Calculate the pH in the cathode compartment.
Contributors and Attributions
- Molly McGuire, Bucknell University (mmcguire@bucknell.edu)
- Sourced from the Analytical Sciences Digital Library