Question

balance the redox reaction by oxidation number method​

Answer 1

Step 1: Assign oxidation numbers to each of the atoms in the equation and write the numbers above the atom.

Step 2: Identify the atoms that are oxidized and those that are reduced. In the above equation, the carbon atom is being oxidized since its oxidation increases from +2 to +4. The iron atom is being reduced since its oxidation number decreases from +3 to 0.

Step 3: Use a line to connect the atoms that are undergoing a change in oxidation number. On the line, write the oxidation-number change.

Step 4: Use coefficients to make the total increase in oxidation number equal to the total decrease in oxidation number. In this case, the least common multiple of 2 and 3 is 6. So the oxidation-number increase should be multiplied by 3, while the oxidation-number decrease should be multiplied by 2. The coefficient is also applied to the formulas in the equation. So a 3 is placed in front of the CO and in front of the CO2. A 2 is placed in front of the Fe on the right side of the equation. The Fe2O3 does not require a coefficient because the subscript of 2 after the Fe indicates that there are already two iron atoms.

process. In the current example, the equation is now balanced.

Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

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