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SOLVED:The Nernst equation applies to both cell reactions and half-reactions. For the conditions specified, calculate the potential for the following half-reactions at 25^∘ C : (a) I2(s) 2 e^- ⟶2 I(a q) ;[I]=0.020 M (b) Fe^3 (a q) e^- ⟶Fe^2 (a q) ;[Fe^3 ]=[Fe^2 ]=0.10 M (c) Sn^2 (a q) ⟶Sn^4 (a q) 2 e^- ;[Sn^2 ]=1.0 ×10^-3 M [Sn^4 ]=0.40 M (d) 2 Cr^3 (a q) 7 H2 O(l) ⟶Cr2 O7^2-(a q) 14 H^ (a q) 6 e^- ;[Cr^3 ]=[Cr2 O7^2-]=1.0 M,[H^ ]=0.010 M

SOLVED:The Nernst equation applies to both cell reactions and half-reactions. For the conditions specified, calculate the potential for the following half-reactions at 25^∘ C : (a) I2(s) 2

The Nernst equation applies to both cell reactions and half-reactions. For the conditions specified, calculate the potential for the following half-reactions at 25^∘ C : (a) I2(s) 2 e^- 2 I(a q) ;[I]=0.020 M (b) Fe^3 (a q) e^- Fe^2 (a q) ;[Fe^3 ]=[Fe^2 ]=0.10 M (c) Sn^2 (a q) Sn^4 (a q) 2 e^- ;[Sn^2 ]=1.0 ×10^-3 M [Sn^4 ]=0.40 M (d) 2 Cr^3 ...

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SOLVED: Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of the following two half-cells:Ag (0.0020 M) e- â†’ Ag(s)Cr3 (0.20 M) 3e- â†’ Cr(s)Use the standard reduction table provided in the lab to determine E.

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