Question

Identify the oxidizing agent and the reducing agent for the following reaction:

2Rb(s)+Br²(g)→2RbBr(s)
Express your answers as chemical formulas separated by a comma.

Answer 1

The reducing agent in the reaction is Rb and the oxidizing agent is Br².The species that undergoes oxidation is Rb(s) because its oxidation state increases from 0 to +1 in RbBr(s). The species that undergoes reduction is Br2(g) because its oxidation state decreases from 0 to -1 in RbBr(s).

Step-by-step explanation:

In the reaction

2Rb(s) + Br²(g) → 2RbBr(s),

the reducing agent is Rb and the oxidizing agent is Br². The species that undergoes oxidation is Rb(s) because its oxidation state increases from 0 to +1 in RbBr(s). The species that undergoes reduction is Br2(g) because its oxidation state decreases from 0 to -1 in RbBr(s). So, the oxidizing agent is Br². (bromine) and the reducing agent is Rb (rubidium).

The species that undergoes oxidation is Rb(s) because its oxidation state increases from 0 to +1 in RbBr(s). The species that undergoes reduction is Br2(g) because its oxidation state decreases from 0 to -1 in RbBr(s). The reducing agent in the reaction is Rb and the oxidizing agent is Br².