Complete and balance the following equations, and identify the oxidizing and reducing agents: As₂O₃(s) + NO₃^-(aq) → H₃AsO₄(aq) + N₂O₃(aq) (acidic solution)

검증된 단계별 안내

Step 1: Write the unbalanced equation: \( \text{As}_2\text{O}_3 (s) + \text{NO}_3^- (aq) \rightarrow \text{H}_3\text{AsO}_4 (aq) + \text{N}_2\text{O}_3 (aq) \).

Step 2: Separate the equation into two half-reactions, one for oxidation and one for reduction. Identify the changes in oxidation states for arsenic and nitrogen.

Step 3: Balance each half-reaction for mass and charge. For the oxidation half-reaction, balance arsenic and oxygen atoms, then add \( \text{H}^+ \) ions to balance hydrogen in acidic solution. For the reduction half-reaction, balance nitrogen and oxygen atoms, then add \( \text{H}^+ \) ions.

Step 4: Balance the charges in each half-reaction by adding electrons. Ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.

Step 5: Combine the balanced half-reactions, cancel out common species, and identify the oxidizing agent (the species that gets reduced) and the reducing agent (the species that gets oxidized).

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주요 개념

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

Redox Reactions

Redox reactions, or oxidation-reduction reactions, involve the transfer of electrons between species. In these reactions, one substance is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the changes in oxidation states of the elements involved is crucial for identifying the oxidizing and reducing agents.

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 often involves adjusting coefficients in front of compounds and may require balancing charges in redox reactions, especially in acidic or basic solutions.

Identifying Oxidizing and Reducing Agents

The oxidizing agent is the species that gets reduced (gains electrons), while the reducing agent is the species that gets oxidized (loses electrons). To identify these agents, one must analyze the changes in oxidation states of the elements in the reaction, determining which species undergoes reduction and which undergoes oxidation.

Complete and balance the following equations, and identify the oxidizing and reducing agents: As2O3(s) + NO3-(aq) → H3AsO4(aq) + N2O3(aq) (acidic solution)