An electrochemical cell consists of a silver electrode dipping into 1.0M AgNO3 a

Chemistry
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An electrochemical cell consists of a silver electrode dipping into 1.0M AgNO3 and a nickel electrode dipping into 1.0M M Ni(NO3)2. A) Describe the cell using cell notation. B) Write the net reaction that occurs as this cell generates electric current, and show the reaction that occurs at each electrode.

 C) Calculate the EMF, free energy and equilibrium constant for the net cell reaction.  Assume the cell is operating under standard conditions

May 13th, 2015

a) Ni/Ni2+ / NO3-/ Ag+/Ag

b) Ni(s) → Ni2+(aq) + 2e- Ox - Anode

  2Ag+ (aq) + 2e- → 2Ag(s) Red – Cathode

 E = Eo - 0.059/2 *log [Ni2+]/ [Ag+]

 E = E0  -0 

E =Eo  

Eo = EAg+/Ag - ENi2+/Ni

       =0.80-(-0.26) = 0.80+0.26=  1.06

E cell = 1.06 V

Regarding any doubt plz let me know.

I will explain. 


May 13th, 2015

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