Write equations for the half-reactions that occur in the electrolysis of molten potassium bromide.

The electrolysis of molten potassium bromide produces K metal at the cathode and Br gas at the anode

Electrolysis utilizes electrical energy to carry out non-spontaneous redox reactions. The ions in the solution flowed by an electric current will move toward the electrode opposite the charge.

The electrolyzed substance is an electrolyte which can be in the form of a melt or a solution.

In the electrolytic cell the positive pole - the anode is the site of oxidation, whereas the negative pole - the cathode is the site of the reduction.

The results of the reaction at the anode are based on substances around the anode which are easily oxidized while the reaction at the cathode is based on substances that are easily subjected to reduction.

Electrons (electricity) enter the electrolysis cell through the negative pole (cathode)

The negative ions from the solution will move towards the positive electrode, and release electrons around the positive electrode (oxidation occurs) and electrons flow to the negative pole

While around the negative electrode electron binding occurs and a reduction reaction occurs

In principle the reaction at the cathode:

For reactions in anode:

a. OH⁻ from the base will be oxidized

b. The halogen metal will oxidize

In the electrolysis of molten KBr with an inert electrode, the cation will be reduced at the cathode and the anion will be oxidized at the anode

Cathode (-): K⁺ (l) + e⁻ ⇒ K (l) (x 2)

Anode (+): 2Br⁻ (l) ⇒Br₂ (g) + 2e⁻

                  2K⁺ (l) + 2Br⁻9l) ⇒ 2K (l) + Br₂ (g)

metal K is produced at the cathode and Br gas at the anode

an electrolytic cell

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During electrolysis

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the substance is produced at the cathode during the electrolysis

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Keywords: the half-reactions, electrolysis, KBr

um i think it might be a car?

c. 4.54 x 10–12 j happens to be correct