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Please show all steps to solve :) Thanks
The standard reduction potentials in V for Ag+ to Ag and Fe3+ to fe2+ are +0.80 and 0.77, respectively. Calculate (in kj) for the following reaction. (F= 96,500 j/v mol)
Please show all steps to solve :) Thanks
The standard reduction potentials in V for Ag+ to Ag and Fe3+ to fe2+ are +0.80 and 0.77, respectively. Calculate (in kj) for the following reaction. (F= 96,500 j/v mol)
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Trinidad TremblayLv2
4 May 2019
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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.