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Chemistry
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13 Dec 2019

The oxidation-reduction reaction given below has a standard cell potential E?cell = ?0.65 V.

Sn4+(aq) + 2 Ag(s) ? 2 Ag+(aq) + Sn2+(aq)

What is the spontaneity of this reaction under standard conditions? spontaneous OR nonspontaneous

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Collen Von
Collen VonLv2
17 Dec 2019

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Related questions

The standard reduction potential for the reduction of AgBr (s) is +0.095 V. The standard reduction potential for the reduction of Ag+ (aq) is +0.799 V.(a) Calculate the standard potential for the cell: Ag (s) | AgBr (s) | Br- (aq) || Ag+ (aq) | Ag (s)(b) Determine the Ksp for AgBr.(c) A silver electrode coated with AgBr (s) is immersed in a sample solution with an unknown concentration of Br- (aq). When this half-cell is connected to a standard Ag+ /Ag electrode, the measured potential is +0.50 V, with the Ag+ /Ag electrode acting as the cathode. What is the concentration Brin the sample?


Calculate the standard cell potential for each of the following electrochemical cells.

Standard Electrode Potentials at 25 ∘C
Reduction half-reaction E∘(V)
Ag+(aq)+e− →Ag(s) 0.80
Sn2+(aq)+2e− →Sn(s) -0.14
ClO2(g)+e− →ClO2−(aq) 0.95
I2(s)+2e− →2I−(aq) 0.54
Ni2+(s)+2e− →Ni(s) -0.23
O2(g)+4H+(aq)+2e− →2H2O(l)

1.23

1. 2Ag+(aq)+Sn(s)→2Ag(s)+Sn2+(aq)

2. 2ClO2(g)+2I−(aq)→2ClO−2(aq)+I2(s)

3. O2(g)+4H+(aq)+2Ni(s)→2H2O(l)+2Ni2+(aq)

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