Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel (b) dilute sulfuric acid with iron

검증된 단계별 안내

Identify the reactants: Dilute sulfuric acid (H2SO4) and iron (Fe).

Write the unbalanced molecular equation: H2SO4(aq) + Fe(s) → FeSO4(aq) + H2(g).

Balance the molecular equation: H2SO4(aq) + Fe(s) → FeSO4(aq) + H2(g). Since there is one sulfate ion (SO4^2-) and one iron atom on both sides, and two hydrogen atoms on both sides, the equation is balanced as written.

Write the total ionic equation by breaking all soluble strong electrolytes into their ions: H2SO4(aq) + Fe(s) → Fe^2+(aq) + SO4^2-(aq) + H2(g).

Identify and remove the spectator ions (ions that appear on both sides of the equation in the same form) to write the net ionic equation. In this case, the sulfate ion is a spectator ion: Fe(s) + 2H+(aq) → Fe^2+(aq) + H2(g).

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주요 개념

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

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, sulfuric acid (H2SO4) acts as an acid, donating protons to iron (Fe), which can accept them. Understanding this concept is crucial for predicting the products of the reaction and writing balanced equations.

Balancing Chemical Equations

Balancing chemical equations 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 compounds to achieve balance, which is essential for accurately representing the stoichiometry of the reaction.

Net Ionic Equations

Net ionic equations focus on the species that actually participate in a chemical reaction, omitting spectator ions that do not change during the reaction. This concept is important for simplifying reactions in aqueous solutions, allowing for a clearer understanding of the underlying chemical processes.