Example 1: Identifying Oxidation and ReductionUse changes in oxidation number to determine which atoms are oxidized and which atoms are reduced in the following reaction Then, identify the oxidizing and reducing agent.SolutionUse the oxidation number rules to assign oxidation numbers to each atom in the balanced equation. Remember, coefficients do not affect oxidation numbers. The oxidized atom increases in oxidation number and the reduced atom decreases in oxidation number.Note the following:The element carbon is oxidized because its oxidation number increases from +2 to +4.The iron(III) ion within the is reduced because its oxidation number decreases from +3 to 0.The carbon monoxide (CO) is the reducing agent since it contains the element that is oxidized.The Fe 3+ ion is the oxidizing agent since it is reduced in the reaction.Text AnswerTEXT ANSWERIn Example 1, describe how the reduction of ferric oxide fits the definitions of oxidation and reduction.
Question
Example 1: Identifying Oxidation and ReductionUse changes in oxidation number to determine which atoms are oxidized and which atoms are reduced in the following reaction Then, identify the oxidizing and reducing agent.SolutionUse the oxidation number rules to assign oxidation numbers to each atom in the balanced equation. Remember, coefficients do not affect oxidation numbers. The oxidized atom increases in oxidation number and the reduced atom decreases in oxidation number.Note the following:The element carbon is oxidized because its oxidation number increases from +2 to +4.The iron(III) ion within the is reduced because its oxidation number decreases from +3 to 0.The carbon monoxide (CO) is the reducing agent since it contains the element that is oxidized.The Fe 3+ ion is the oxidizing agent since it is reduced in the reaction.Text AnswerTEXT ANSWERIn Example 1, describe how the reduction of ferric oxide fits the definitions of oxidation and reduction.
Solution
In the given example, the reduction of ferric oxide fits the definitions of oxidation and reduction as follows:
Oxidation is defined as the process where an atom, ion, or molecule loses electrons, thereby increasing its oxidation state. In this reaction, carbon in carbon monoxide (CO) is oxidized because its oxidation number increases from +2 to +4. This means it loses electrons.
On the other hand, reduction is defined as the process where an atom, ion, or molecule gains electrons, thereby decreasing its oxidation state. In this reaction, the iron(III) ion within the ferric oxide is reduced because its oxidation number decreases from +3 to 0. This means it gains electrons.
Therefore, the reduction of ferric oxide in this reaction fits the definitions of oxidation (for carbon) and reduction (for iron).
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