Question

Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the concentrations.

Cu(s)∣∣Cu²⁺(aq,0.0155 M)∥∥Ag⁺(aq,3.50 M)∣∣Ag(s)

net cell equation:

Answer 1

The net cell equation for the electrochemical cell with copper and silver is Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s).

Step-by-step explanation:

The net cell equation for an electrochemical cell involving copper and silver can be written by identifying the anode (oxidation) and cathode (reduction) reactions, then combining them. In this case, copper undergoes oxidation (loses electrons) and silver undergoes reduction (gains electrons). The half-reactions would be as follows:

• Cu(s) → Cu²⁺(aq) + 2e⁻ (oxidation at the anode)
• Ag⁺(aq) + e⁻ → Ag(s) (reduction at the cathode)

Combining both half-reactions while canceling out the electrons, the net cell equation becomes:

Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

No concentrations are included as they are not needed for the net cell equation. In this cell diagram, the salt bridge and inert electrodes are not represented because they are not part of the net reaction; they are however crucial for the complete electrochemical cell functionality. The anode is where oxidation takes place, and the cathode is where reduction occurs.