Reactants:
* Lead(IV) oxide (PbO2)
* Sulfuric acid (H2SO4)
Products:
* Lead(II) sulfate (PbSO4)
* Water (H2O)
* Oxygen gas (O2)
Electrochemical Reaction:
The overall electrochemical reaction for this process is:
PbO2(s) + 2H2SO4(aq) → PbSO4(s) + 2H2O(l) + O2(g)
In this reaction, lead(IV) oxide is reduced to lead(II) sulfate, while sulfuric acid is oxidized to water and oxygen gas. The reduction of lead(IV) oxide occurs at the cathode, while the oxidation of sulfuric acid occurs at the anode.
Electrode Reactions:
* Cathode (Reduction): PbO2(s) + 4H+ (aq) + 2e- → PbSO4(s) + 2H2O(l)
* Anode (Oxidation): 2H2SO4(aq) → O2(g) + 2H2O(l) + 2SO42-(aq)
Electric Current:
The flow of electrons from the anode to the cathode through the external circuit generates an electric current. This current can be used to power various electrical devices.
Applications:
This electrochemical reaction is employed in lead-acid batteries, which are commonly used in automobiles and other vehicles. In these batteries, lead(IV) oxide is used as the positive electrode (cathode), while sulfuric acid is used as the electrolyte. The reaction between these components produces an electric current and generates water and oxygen gas as by-products.
