Using information from the table above, write a net-ionic equation for the reaction between the Sn electrode and the Cu(NO3)2 solution that would be thermodynamically favorable. Justify that the reaction is thermodynamically favorable. 2. Calculate the value of ∆G° for the reaction. Include units with your answer.

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1. Using information from the table above, write a net-ionic equation for the reaction between the Sn electrode and the Cu(NO3)2 solution that would be thermodynamically favorable. Justify that the reaction is thermodynamically favorable.

2. Calculate the value of ∆G° for the reaction. Include units with your answer.

In another experiment, the student places a new Sn electrode into a fresh solution of 1.0 M Cu(NO3),.
Half-Reaction
E° (V)
Cu* + e → Cu(s)
0.52
Cu²+ + 2 e –→ Cu(s)
0.34
Sn+ + 2 e → Sn²+
0.15
Sn2+ + 2 e –→ Sn(s)
-0.14
Transcribed Image Text:In another experiment, the student places a new Sn electrode into a fresh solution of 1.0 M Cu(NO3),. Half-Reaction E° (V) Cu* + e → Cu(s) 0.52 Cu²+ + 2 e –→ Cu(s) 0.34 Sn+ + 2 e → Sn²+ 0.15 Sn2+ + 2 e –→ Sn(s) -0.14
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