Question

Write a balanced half-reaction describing the reduction of gaseous dibromine to aqueous bromide anions.

Answer 1

Answer: The balanced half reaction is written below.

Explanation:

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

$X^{n+}+ne^-\rightarrow X$

When bromine gas is reduced to bromide ions, the number of electron transferred are 2

The chemical equation for the reduction of bromine gas to bromide ions follows:

$Br_2+2e^-\rightarrow 2Br^{-}$

Hence, the balanced half reaction is written above.

Answer 2

The reduction of gaseous dibromine to bromide ions occurs according to the reaction$Br2(g) + 2e -----> 2Br^-(aq)$.

In a redox reaction a specie looses electrons while another specie gains electrons. The specie that looses electrons is the reducing agent while the specie that gains electrons is the oxidizing agent.

In the reduction of dibromine to aqueous bromide anions; the reduction half equation occurs as follows;

$Br2(g) + 2e -----> 2Br^-(aq)$

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