Write the equations describing the electrode reactions and the net cell reaction for this electrochemical cell containing tin and silver:
Sn(s)|Sn2 (aq)||Ag (aq)|Ag(s)
what is the equation for cathode, anode, and net cell reaction
To determine the equations for the cathode, anode, and the net cell reaction for this electrochemical cell, we need to understand the half-reactions occurring at each electrode.
1. Cathode (Reduction half-reaction):
Looking at the given cell, the cathode is the silver electrode (Ag(s)). The reduction half-reaction occurring at the cathode is the gain of electrons by Ag+ ions from the solution to form solid Ag.
Ag+(aq) + e- → Ag(s)
2. Anode (Oxidation half-reaction):
The anode in the cell is the tin electrode (Sn(s)). The oxidation half-reaction occurring at the anode involves the loss of electrons by solid tin to form Sn2+ ions in solution.
Sn(s) → Sn2+(aq) + 2e-
3. Net Cell Reaction:
To determine the net cell reaction, we need to balance the two half-reactions so that they have an equal number of electrons. Since two electrons are involved in the reduction half-reaction and one electron in the oxidation half-reaction, we multiply the oxidation half-reaction by 2 to balance the electrons.
2Sn(s) → 2Sn2+(aq) + 4e-
Now we add the balanced oxidation and reduction half-reactions to obtain the net cell reaction. Since two electrons are canceled out in the overall reaction, we don't need to multiply by any coefficients.
Net cell reaction:
2Sn(s) + Ag+(aq) → 2Sn2+(aq) + Ag(s)
Therefore, the equations for the cathode, anode, and net cell reaction are:
Cathode (Reduction): Ag+(aq) + e- → Ag(s)
Anode (Oxidation): Sn(s) → Sn2+(aq) + 2e-
Net Cell Reaction: 2Sn(s) + Ag+(aq) → 2Sn2+(aq) + Ag(s)