Line notation is given for an elecrtochemical cell as well asthe standard reduction potentials.
Ba(s)|Ba2+(aq)||Rb+(aq)|Rb?(s)
Ba2+(aq)+2e- --> Ba(s); E%u25E6 =-2.91 V
Rb+(aq)+e- --> Rb(s); E%u25E6=-2.98
a)Calculate E%u25E6, /\G%u25E6, and K at 25%u25E6C for thereaction. Show work!
b)What will the cell potentials be if the concentrations of Rb+is 0.0500 M and the concentration of Ba2+ is 0.100 M?
Line notation is given for an elecrtochemical cell as well asthe standard reduction potentials.
Ba(s)|Ba2+(aq)||Rb+(aq)|Rb?(s)
Ba2+(aq)+2e- --> Ba(s); E%u25E6 =-2.91 V
Rb+(aq)+e- --> Rb(s); E%u25E6=-2.98
a)Calculate E%u25E6, /\G%u25E6, and K at 25%u25E6C for thereaction. Show work!
b)What will the cell potentials be if the concentrations of Rb+is 0.0500 M and the concentration of Ba2+ is 0.100 M?
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Related questions
Standard reduction potentials
| Reduction half-reaction | E∘ (V) |
| Ag+(aq)+e−→Ag(s) | 0.80 |
| Cu2+(aq)+2e−→Cu(s) | 0.34 |
| Sn4+(aq)+4e−→Sn(s) | 0.15 |
| 2H+(aq)+2e−→H2(g) | 0 |
| Ni2+(aq)+2e−→Ni(s) | −0.26 |
| Fe2+(aq)+2e−→Fe(s) | −0.45 |
| Zn2+(aq)+2e−→Zn(s) | −0.76 |
| Al3+(aq)+3e−→Al(s) | −1.66 |
| Mg2+(aq)+2e−→Mg(s) | −2.37 |
Part A
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction:
Express your answer numerically.
Part B
Calculate the standard cell potential (E∘) for the reaction
if K = 3.04×10−3.
Express your answer to three significant figures and include the appropriate units.
