1) For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 1.50

Question

1) For the following electrochemical cell        Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 1.50 M)|Ag(s) write the net cell equation.

Calculate the following values using standard potentials as needed. Eo cell and dGo for each reaction.............................................................2)A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M iron(II) ion solution and another electrode composed of copper in a 1.0 M copper(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25

Explanation / Answer

1. Oxidation half : Cu(s) - 2e- -------> Cu2+

Reduction half : 2Ag+ + 2e- --------> 2Ag(s)

Net reaction : Cu(s) + 2Ag+ ---------> Cu2+ + 2Ag(s)

2. [Fe2+] =1M , [Cu2+] =1M

Net cell reaction : Fe(s) + Cu2+(aq) -----> Cu(s) + Fe2+(aq)

Now, E0cell =E0cathode - E0 anode = 0.34-(-0.44) =0.78 V

delta G0 =-nFE0cell = -2*96500*0.78 =

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