calculate the standard cell potential for the reaction below please help with qu

Question

calculate the standard cell potential for the reaction below

please help with questions 2 and 3

A. Calculate the standard cell potential (E degree cell) for the reaction below: Pb^2+ (aq) + Zn (s) rightarrow Zn^2+ (aq) + Pb (s) B. Calculate the Delta G degree for the reaction above at 25 degree C. C. Identify if this reaction is spontaneous or nonspontaneous. _____ A common shorthand way to represent a voltaic cell is: anode | anode solution || cathode solution || cathode A double vertical line represents a salt bridge or a porous barrier. A single vertical line represents a change in phase, such as from solid to solution. Write the half reactions and overall cell reaction represented by Fe | Fe^2+ || Ag^+ |Ag.

Explanation / Answer

2) a Eocell = Eocathode - Eoanode

Pb2+ + 2e- ------> Pb Eocell = -0.13 V

Zn2+ + 2e- ---> Zn Eocell = -0.76 V

Eocell = -0.13 - (-0.76 ) V = 0.63 V

Go = - nFEocell

{ n = number of electron transfer, F = faraday constant = 96500 }

Go = -2 x 96500 x 0.63 V = -121590 J/mol = 121.59 KJ/mol

Go of reaction is negetive so reaction is spontaneous

3) Fe | Fe2+ || Ag+ | Ag

Fe2+ + 2e- ----> Fe anode

2Ag+ + 2e- ----> 2Ag cathode

Fe + 2Ag+ ----> 2Ag + Fe2+ over all cell reaction

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