Use the half-reactions below to produce a voltaic ...

Question

Use the half-reactions below to produce a voltaic cell with the given standard cell potential.

Jules Bruno · Accepted Answer

In a voltaic/galvanic cell: Anode is in the negative side (left side of the diagram)▪ Anode → oxidation▪ oxidation half-reaction happens in the anode solution▪ losing electrons → becoming more positive → anode dissolves away Cathode is in the positive side (right side of the diagram)▪ Cathode → reduction▪ reduction half-reaction happens in the anode solution▪ gaining electrons → becoming more negative → solids is deposited in the surface[readmore]Loss Electrons → Oxidation → Reducing AgentGain Electrons → Reduction → Oxidizing AgentThe cell potential (E˚cell) is given by:E°cell=E°cathode-E°anodeWe need to produce a cell potential of +0.67 V.• ↓ E° → oxidation → anode• ↑ E° → reduction → cathodeFrom the given half-cell reaction and potentials, the two reactions that can produce 0.67 V are:Ag+(aq) + e- → Ag(s)                        E°cell = 0.80 VSn4+(aq) + 2 e- → Sn2+(s)                 E°cell = 0.13 VStep 4. Calculate E°cell.Ag+(aq) + e- → Ag(s)                        E°cell = 0.80 V                    anodeSn4+(aq) + 2 e- → Sn2+(s)                 E°cell = 0.13 V                    cathodeE°cell=E°cathode-E°anodeE°cell=0.80 V -0.13 V    E°cell = 0.67 VTherefore, half-reactions that will produce a voltaic cell with the given standard cell potential are:Ag+(aq) + e- → Ag(s)                        E°cell = 0.80 VSn4+(aq) + 2 e- → Sn2+(s)                 E°cell = 0.13 V

Problem: Use the half-reactions below to produce a voltaic cell with the given standard cell potential.

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Problem Details

Problem: Use the half-reactions below to produce a voltaic cell with the given standard cell potential.

FREE Expert Solution

Problem Details

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