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The Nernst equation the following electrochemical cell will be: Ni(s) | Ni2+ (aq)|| Ag+ (aq)| Ag A) Ecell = Eºcell-RT/F[In[Ni2+]/[Ag+12] B) Ecell = Eccl1-RT/2F[In[Ni2+1/[Ag+1?] C) Ecell = Eºcell-RT/2F[In[Ag+]2/[Ni2+]] D) Ece = Eccl1-RT/2F[In[Ni2+1/[Ag+l]
Calculate the emf of the cell in which the following reaction takes place: Ni(s)+2Ag^+(0.002M)→ Ni^2+(0.160 M)+2Ag(s) Given that E^∘_cell=1.05 V nbsp;
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Calculate the cell emf at 25° C for the following cell:Ni(s)
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