Which batteries have reversible reactions

A cell made from magnesium and copper has a higher voltage than either of the other two combinations. Suggest the voltage of a cell made using magnesium and silver. Any value greater than 2. This is because the difference between the reactivity of magnesium and silver is greater than the difference between magnesium and copper.

In fact, the cell would have a voltage of approximately 3. When a battery is discharged, an electrochemical oxidation reaction proceeds at the negative electrode, and an electrochemical reduction reaction occurs at the positive electrode.

When one attempts to recharge a battery by reversing the direction of electric current flow, the opposite takes place: a reduction reaction proceeds at the negative electrode, and an oxidation reaction takes place at the positive electrode.

For example, when the battery is recharged, the overall electrochemical reduction reaction at the negative electrode is identical to the electrochemical oxidation reaction that proceeded at the negative electrode when the battery was discharged, only written in reverse. When the battery is charged, the overall reduction reaction that proceeds at the negative electrode may not be the true reverse of the oxidation reaction that proceeded when the battery was discharged.

For example, metal oxidation might be the sole oxidation reaction during battery discharge, whereas the formation of hydrogen a highly inflammable and therefore dangerous gas might be a significant reduction reaction during battery recharging.

For example, rough or filamentary structures may form in the battery after repeated charge- discharge cycles. These structures can result in unwanted growth of the electrode and subsequent electronic contact between the battery electrodes- -a short circuit. In the case of the nickel-cadmium battery, the cadmium electrode has two important features.

First, the rate of hydrogen formation on cadmium is very slow compared with that on pure zinc or pure iron, for example. Second, the solubility of cadmium in basic aqueous electrolyte solutions is sufficiently low that the cadmium does not tend to dissolve in the electrolyte and migrate to the positive electrode or elsewhere within the battery.

At the same time, however, the cadmium is sufficiently soluble that its reduction can proceed easily, and it can form compact cadmium structures during battery recharge; the solubilities of most other metals are either too high or too low.

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