When iron rusts, solid iron reacts with gaseous oxygen to form solid iron(III) oxide. Write the balanced chemical equation for this reaction.

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Identify the reactants and products: The reactants are solid iron (Fe) and gaseous oxygen (O_2), and the product is solid iron(III) oxide (Fe_2O_3).

Write the unbalanced chemical equation: Fe (s) + O_2 (g) \rightarrow Fe_2O_3 (s).

Balance the iron atoms: Since there are 2 iron atoms in Fe_2O_3, place a coefficient of 2 in front of Fe: 2Fe (s) + O_2 (g) \rightarrow Fe_2O_3 (s).

Balance the oxygen atoms: There are 3 oxygen atoms in Fe_2O_3, so place a coefficient of 3/2 in front of O_2 to balance the oxygen atoms: 2Fe (s) + \frac{3}{2}O_2 (g) \rightarrow Fe_2O_3 (s).

Convert to whole numbers: Multiply the entire equation by 2 to eliminate the fraction: 4Fe (s) + 3O_2 (g) \rightarrow 2Fe_2O_3 (s).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Chemical Reactions

A chemical reaction involves the transformation of reactants into products through the breaking and forming of chemical bonds. In the case of rusting, iron (Fe) reacts with oxygen (O2) to produce iron(III) oxide (Fe2O3), illustrating how elements combine to form new compounds.

Balancing Chemical Equations

Balancing a chemical equation ensures that the number of atoms for each element is the same on both sides of the equation, adhering to the law of conservation of mass. This process involves adjusting coefficients in front of the chemical formulas to achieve balance, which is crucial for accurately representing the reaction.

Oxidation-Reduction Reactions

Rusting is an example of an oxidation-reduction (redox) reaction, where iron is oxidized (loses electrons) and oxygen is reduced (gains electrons). Understanding the transfer of electrons in these reactions helps explain the chemical changes occurring during rust formation and the role of oxygen in the process.

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Oxidation and Reduction Reactions

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