What is the coefficient on Sn²⁺ when the following reaction is balanced in acidic solution?
(a) 2 (b) 4 (c) 5 (d) 7

검증된 단계별 안내

insert step 1> Identify the oxidation and reduction half-reactions in the given unbalanced reaction.

insert step 2> Balance the atoms other than O and H in each half-reaction.

insert step 3> Balance the oxygen atoms by adding H2O molecules to the side that needs oxygen.

insert step 4> Balance the hydrogen atoms by adding H+ ions to the side that needs hydrogen.

insert step 5> Balance the charge by adding electrons to one side of each half-reaction, then combine the half-reactions ensuring the electrons cancel out.

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주요 개념

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Balancing Redox Reactions

Balancing redox reactions involves ensuring that both mass and charge are conserved. In acidic solutions, this typically requires the use of half-reactions, where oxidation and reduction processes are balanced separately before combining them. The coefficients in front of each species indicate the number of moles involved in the reaction, which must be adjusted to achieve balance.

Oxidation States

Oxidation states are a way to keep track of electrons in chemical reactions. Each element in a compound is assigned a specific oxidation state based on its electron configuration and bonding. Understanding the changes in oxidation states during the reaction is crucial for identifying which species are oxidized and reduced, which directly influences the coefficients used in balancing the equation.

Acidic Solution Conditions

In an acidic solution, the presence of hydrogen ions (H⁺) affects the balancing of redox reactions. When balancing in acidic conditions, additional H⁺ ions and water molecules may be added to the half-reactions to ensure that both mass and charge are balanced. This is particularly important when determining the coefficients for species like Sn²⁺ in the overall balanced equation.

What is the coefficient on Sn2+ when the following reaction is balanced in acidic solution?(a) 2 (b) 4 (c) 5 (d) 7