What is the standard cell notation for a galvanic cell made with silver and nickel?

Ni (s) ∣∣ N i 2 + (aq) ∣∣ ∣∣ A g + (aq) ∣∣ A g (s)

Explanation:

Start by finding the standard reduction potential for the A g + and N i 2 + ion. Normally, the values are listed at the back of most chemistry textbooks.

A g + (aq) + 1 e - →A g (s) Eo = 0.80 V

N i 2 + (aq) + 2 e - →Ni (s) Eo = - 0.23 V

In the galvanic cell, the reaction is spontaneous and for a spontaneous reaction E o cell must be a positive quantity.

E o cell = E o Anode + E o cathode

Manipulate the two equations so that E o cell is positive. Note that the anode is the site of oxidation (where electrons are lost) and the cathode (where electron are gained) is the site for reduction.

A g + (aq) + 1 e - →A g (s) Eo = 0.80 V

Ni (s) →N i 2 + (aq) + 2 e - Eo = 0.23 V

2 * {A g + (aq) + 1 e - →A g (s) } Eo = 0.80 V (Cathode)

Ni (s) →N i 2 + (aq) + 2 e - Eo = 0.23 V (Anode)

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2A g + (aq) + Ni (s) →N i 2 + (aq) + 2A g (s) E o cell = 1.03 V

Start with the anode components (site of oxidation) - the cathode components are listed to the right.

Ni (s) ∣∣ N i 2 + (aq) ∣∣ ∣∣ A g + (aq) ∣∣ A g (s)

The single vertical lines indicate the boundary (phase difference) between solid Ni and N i 2 + ions in the aqueous solution of the first compartment and between solid Ag and A g + ions present in the aqueous solution of the second compartments.

The double vertical lines refer to the salt bridge - note that the salt bridge must be an inert salt to both ions present in both compartments of the galvanic cell ...