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In the following equation:

[tex]\[ \text{iron oxide} + \text{carbon} \rightarrow \text{iron} + \text{carbon monoxide} \][/tex]

Which element is being oxidized, and which is being reduced?

A. iron, oxygen
B. carbon, iron
C. iron, carbon
D. carbon, oxygen

Sagot :

GinnyAnsweridn
To understand which substances are being oxidized and reduced in the given chemical reaction, iron oxide + carbon -> iron + carbon monoxide, we need to analyze the changes in oxidation states of the elements involved.

1. Identify the reactants and products:
- Reactants: Iron oxide (Fe₂O₃) and carbon (C)
- Products: Iron (Fe) and carbon monoxide (CO)

2. Determine the oxidation states:
- For iron oxide (Fe₂O₃), each iron (Fe) has an oxidation state of +3, and each oxygen (O) has an oxidation state of -2.
- For elemental carbon (C), the oxidation state is 0.
- In the product iron (Fe), the oxidation state of iron is 0.
- In carbon monoxide (CO), the oxidation state of carbon (C) is +2 and oxygen is -2.

3. Identify the changes in oxidation states:
- Iron (Fe) changes from +3 in Fe₂O₃ to 0 in Fe.
- Carbon (C) changes from 0 in elemental carbon to +2 in CO.

4. Determine what is being oxidized and reduced:
- Oxidation involves an increase in oxidation state. Carbon's oxidation state increases from 0 to +2, meaning carbon is being oxidized.
- Reduction involves a decrease in oxidation state. Iron's oxidation state decreases from +3 to 0, meaning iron is being reduced.

Based on this analysis, the correct answer is:

B. carbon, iron
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