based on the oxidation states of the atoms in this reaction, answer the questions.\n4fe^(0) + 3o₂^(0) →…

based on the oxidation states of the atoms in this reaction, answer the questions.\n4fe^(0) + 3o₂^(0) → 2fe₂^(3+)o₃^(2-)\nhow many electrons does the iron half - reaction lose?\nhow many electrons does the oxygen half - reaction gain?\nwhat is the total number of electrons that are moved in this oxidation - reduction reaction?

based on the oxidation states of the atoms in this reaction, answer the questions.\n4fe^(0) + 3o₂^(0) → 2fe₂^(3+)o₃^(2-)\nhow many electrons does the iron half - reaction lose?\nhow many electrons does the oxygen half - reaction gain?\nwhat is the total number of electrons that are moved in this oxidation - reduction reaction?

Answer

Explanation:

Step1: Analyze iron half - reaction

Iron goes from 0 oxidation state to + 3. One iron atom loses 3 electrons. Since there are 4 iron atoms in the reaction, the total number of electrons lost by iron is $4\times3 = 12$.

Step2: Analyze oxygen half - reaction

Oxygen goes from 0 oxidation state to - 2. One oxygen atom gains 2 electrons. In $O_2$, there are 2 oxygen atoms, so one $O_2$ molecule gains 4 electrons. Since there are 3 $O_2$ molecules, the total number of electrons gained by oxygen is $3\times4=12$.

Step3: Determine total electrons moved

In a redox reaction, the number of electrons lost in the oxidation half - reaction is equal to the number of electrons gained in the reduction half - reaction. So the total number of electrons moved is 12.

Answer:

How many electrons does the iron half - reaction lose? 12 How many electrons does the oxygen half - reaction gain? 12 What is the total number of electrons that are moved in this oxidation - reduction reaction? 12