This invention uses different chemistry to gain the most energy from the aluminum anode. Even though galvanic cells using an aluminum anode and a hydrogen peroxide cathode reaction are known, the substitution of an alkali metal peroxide represents a different chemistry. The correlation of cell functions to the relative anode and cathode areas permits a higher efficiency of energy output over losses from parasitic reactions. The use of solid alkali metal peroxide in the cathode reaction affords additional control of the cathode to form hydroxide ion. Decomposition of hydrogen peroxide into oxygen and water occurs as a side reaction to the reduction to hydroxide ion formation at the cathode. Prior art for aluminum anode galvanic cells do not take the relative area of the anode and cathode into account for the cell performance. In prior art the excess anode area leads to additional consumption of the aluminum anode by parasitic reactions, thus reducing anode efficiency. Advantages
- Invention uses different peroxide chemistry to gain the most control over the hydroxide ion production at the cathode.
- Optimum bulk surface area relationship between the anode and cathode improves power delivery from the cell.
- This invention substitutes sodium peroxide for hydrogen peroxide which involves different reaction steps, resulting in a different overall cathode reaction and serves to overcome the problems encountered with hydrogen peroxide as the cathode oxygen source.
- Cell performance to the relative anode and cathode stoichiometry in terms of electrode bulk surface areas permits a higher energy output relative to losses from parasitic reactions.
- The use of solid sodium peroxide in the cathode reaction affords additional control of the cathode reaction.
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