Question

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

Sn(s)|Sn²⁺+(aq, 0.0155 M) || Ag⁺ (aq, 1.50 M) Ag(s)

Answer 1

The net cell equation for the electrochemical cell composed of Sn and Ag is Sn(s) + 2Ag⁺(aq) → Sn²⁺(aq) + 2Ag(s), representing the oxidation of tin and the reduction of silver ions.

Step-by-step explanation:

The question involves writing the net cell equation for an electrochemical cell composed of tin (Sn) and silver (Ag). In electrochemical cells, half-reactions at the anode and cathode can be combined to give the overall net cell reaction. The anode is the electrode where oxidation (loss of electrons) occurs, and the cathode is where reduction (gain of electrons) happens. In the given cell, tin will lose electrons (oxidation) and silver ions will gain electrons (reduction).

The half-reactions for the cell are:

• Anode (oxidation): Sn(s) → Sn²⁺(aq) + 2e⁻
• Cathode (reduction): 2Ag⁺(aq) + 2e⁻ → 2Ag(s)

By balancing the electrons, we combine these half-reactions to get the net cell equation:

Sn(s) + 2Ag⁺(aq) → Sn²⁺(aq) + 2Ag(s)

This equation represents the overall cell reaction, showing that tin is being oxidized to tin ions while silver ions are being reduced to solid silver. No platinum electrode or salt bridge are involved in the reaction, and the phases have been omitted as requested.