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

검증된 단계별 안내

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).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

도움이 되었나요?

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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.