A galvanic cell is constructed with a zinc electrode in a 1.00 M solution of Zn ions…
CHEMISTRY · Multi-part · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry
Problem
A galvanic cell is constructed with a zinc electrode in a 1.00 M solution of Zn2+ ions and a silver electrode in a 1.00 M solution of Ag+ ions.
Cell notation: Zn(s)∣Zn2+(1.00M)∣∣Ag+(1.00M)∣Ag(s)
Use the information in the cell notation to write a balanced net ionic equation that conserves both mass and charge.
(a) Write the oxidation half-reaction that occurs at the zinc electrode and state the total charge on each side.
(b) Write the reduction half-reaction that occurs at the silver electrode and state the total charge on each side.
(c) Combine the two half-reactions, showing all electrons explicitly, and verify that the electrons lost equal the electrons gained.
(d) Remove the electrons and provide the final net ionic equation for the cell reaction. Demonstrate that charge is conserved in this final equation.