An electrochemical cell is based on these two half-reactions and their given standard reduction potential values:
Ox: Sn(s)→Sn2+(aq,1.60molL−1)+2e−E∘anode=−0.14(V)
Red: ClO2(g,0.220bar)+e−→ClO−2(aq,1.60molL−1)E∘cathode=0.95(V)

Compute the cell potential at 25 ∘C .

An electrochemical cell is a cell that produces chemical energy from a spontaneous chemical process. Let us recall that cell potential can be obtained from; Ecell = 0.0592/n log K

The cell equation is;

Sn(s) + ClO2(g) ----> Sn^2+(aq) + ClO^2-(aq)

Hence;

K = (1.60) (1.60)/(0.220)

K = 11.6

Therefore;

Ecell = 0.0592/2 log (11.6)

= 0.03 V

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An electrochemical cell is based on these two half-reactions and their given standard reduction potential values: Ox: Sn(s)→Sn2+(aq,1.60molL−1)+2e−E∘anode=−0.14(V) Red: ClO2(g,0.220bar)+e−→ClO−2(aq,1.60molL−1)E∘cathode=0.95(V) Compute the cell potential at 25 ∘C .

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An electrochemical cell is based on these two half-reactions and their given standard reduction potential values:
Ox: Sn(s)→Sn2+(aq,1.60molL−1)+2e−E∘anode=−0.14(V)
Red: ClO2(g,0.220bar)+e−→ClO−2(aq,1.60molL−1)E∘cathode=0.95(V)

Compute the cell potential at 25 ∘C .