Balance the following redox reaction:
Fe\(_2\)O\(_3\) + CO → Fe + CO\(_2\)
- Fe\(_2\)O\(_3\) + CO → 2Fe + 2CO\(_2\)
- 2Fe\(_2\)O\(_3\) + 3CO → 4Fe + 3CO\(_2\)
- Fe\(_2\)O\(_3\) + 2CO → 2Fe + 2CO\(_2\)
-
Fe\(_2\)O\(_3\) + 3CO → 2Fe + 3CO\(_2\)
The correct answer is: D
Explanation
To balance the redox reaction, we need to ensure that the number of atoms of each element and the total charge are the same on both sides of the equation. In this reaction, we can see that the number of oxygen (O) atoms is not balanced. To balance them, we need to add a coefficient of 3 in front of CO\(_2\) to get 3CO\(_2\). Similarly, the number of iron (Fe) atoms is not balanced. To balance them, we need to add a coefficient of 2 in front of Fe to get 2Fe
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