Find the E_cell⁰ from the given data

• a. Zn|Zn²⁺||Cu²⁺|Cu: E_cell⁰ = 1.10 V
• b. Cu|Cu²⁺||Ag⁺|Ag: E_cell⁰ = 0.46 V
• c. Zn|Zn²⁺||Ag⁺|Ag: E_cell⁰ = ?

(Given E_Cu²⁺|Cu⁰ = 0.34 V)

• (1) - 0.04 V
• (2) + 0.04 V
• (3) + 0.30 V
• (4) 1.56 V

To find the standard cell potential (E_cell⁰) for the reaction Zn|Zn²⁺ || Ag⁺|Ag, we can use the given standard reduction potentials.

Given Data

• ECu2+|Cu0 = 0.34 V
• EZn|Zn2+0 = -0.76 V (standard value)

Calculating E_cell⁰

The standard cell potential can be calculated using the formula:

E_cell⁰ = E_cathode⁰ - E_anode⁰

Identifying Anode and Cathode

In this case:

• Anode: Zn (oxidation)
• Cathode: Ag⁺ (reduction)

Substituting Values

Now, we can substitute the values:

Ecell0 = EAg+|Ag0 - EZn|Zn2+0

Since E_Ag⁺|Ag⁰ is not given directly, we can calculate it using:

E_Ag⁺|Ag⁰ = E_Cu²⁺|Cu⁰ - 0.46 V

Thus, E_Ag⁺|Ag⁰ = 0.34 V + 0.46 V = 0.80 V.

Final Calculation

Now substituting back:

E_cell⁰ = 0.80 V - (-0.76 V)

E_cell⁰ = 0.80 V + 0.76 V = 1.56 V

Answer

The standard cell potential E_cell⁰ for the reaction Zn|Zn²⁺ || Ag⁺|Ag is 1.56 V.