Question

Calculate the standard cell potential, ∘cell , for the reaction shown. Use these standard reduction potentials. Cu(s) + Ag⁺(aq)⟶Cu⁺(aq) + Ag(s)

Answer 1

The standard cell potential for the reaction Cu(s) + Ag⁺(aq) → Cu⁺(aq) + Ag(s) is calculated by subtracting the standard electrode potential of the anode from the cathode. This gives a cell potential of +0.95 V, indicating that the reaction is spontaneous under standard state conditions.

Step-by-step explanation:

To calculate the standard cell potential, E°cell, for the reaction Cu(s) + Ag⁺(aq) → Cu⁺(aq) + Ag(s), we need to look at the standard reduction potentials for the reduction of Ag⁺ and the oxidation of Cu to Cu⁺. The standard reduction potential for the reduction of Ag⁺ to Ag is +0.80 V and for the oxidation of Cu to Cu⁺ is +0.15 V. However, since Cu is being oxidized, we need to reverse the sign of its standard reduction potential.Thus, the E°cell is calculated as:

E°cell = E°cathode (Ag/Ag⁺) - E°anode (Cu/Cu⁺)

E°cell = +0.80 V - (-0.15 V)

E°cell = +0.95 V

Since the standard cell potential is positive, the reaction is spontaneous under standard state conditions.