Complete and balance the following equations, and identify the oxidizing and reducing agents:

a. MnO4−(𝑎𝑞)+CH3OH(𝑎𝑞)⟶Mn2+(𝑎𝑞)+HCOOH(𝑎𝑞)(acidic solution)
b. As2O3(𝑠)+NO3−(𝑎𝑞)⟶H3AsO4(𝑎𝑞)+N2O3(𝑎𝑞)(acidic solution)
c. Pb(OH)42−(𝑎𝑞)+ClO−(𝑎𝑞)⟶PbO2(𝑠)+Cl−(𝑎𝑞)(basic solution)

Verified step by step guidance

Step 1: Identify the oxidation states of each element in the reactants and products for each equation to determine which elements are oxidized and reduced.

Step 2: Write the half-reactions for the oxidation and reduction processes separately for each equation.

Step 3: Balance each half-reaction for mass and charge. In acidic solutions, add H₂O to balance oxygen and H⁺ to balance hydrogen. In basic solutions, add OH^- to balance both hydrogen and oxygen.

Step 4: Multiply each half-reaction by appropriate coefficients so that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.

Step 5: Add the balanced half-reactions together, canceling out electrons and any other species that appear on both sides, to obtain the balanced overall equation. Identify the oxidizing agent (species that is reduced) and the reducing agent (species that is oxidized).

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Key Concepts

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

Redox Reactions

Redox reactions, or reduction-oxidation 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 electron transfer is crucial for identifying the oxidizing and reducing agents in a reaction.

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 and may require separate balancing of oxidation and reduction half-reactions in redox processes.

Oxidizing and Reducing Agents

The oxidizing agent is the species that gets reduced by gaining electrons, while the reducing agent is the species that gets oxidized by losing electrons. Identifying these agents is essential in redox reactions, as they play a key role in determining the direction of electron flow and the overall reaction mechanism.

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01:01

Oxidizing and Reducing Agents

Related Practice

Textbook Question

Complete and balance the following half-reactions in acidic solution. In each case indicate whether the half-reaction is an oxidation or a reduction. b. H2SO3(𝑎𝑞)⟶SO42−(𝑎𝑞)

Textbook Question

Complete and balance the following equations, and identify the oxidizing and reducing agents: (a) Cr₂O₇^2-(aq) + I^-(aq) → Cr³⁺(aq) + IO₃^-(aq) (acidic solution) (b) MnO₄^-(aq) + CH₃O(1aq) → Mn²⁺(aq) + HCOOH(aq) (acidic solution) (c) I₂(s) + OCl^-(aq) → IO₃^-(aq) + Cl^-(aq) (acidic solution)

Textbook Question

Complete and balance the following equations, and identify the oxidizing and reducing agents: MnO₄^-(aq) + Br^-(aq) → MnO₂(s) + BrO₃^-(aq) (basic solution)

Textbook Question

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

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Textbook Question

Complete and balance the following equations, and identify the oxidizing and reducing agents. (Recall that the O atoms in hydrogen peroxide, H₂O₂, have an atypical oxidation state.) (a) NO₂^-(aq) + Cr₂O₇^2-(aq) → Cr³⁺(aq) + NO₃^-(aq) (acidic solution) (b) S(s) + HNO₃(aq) → H₂SO₃(aq) + N₂O(g) (acidic solution) (c) Cr₂O₇^2- (aq) + CH₃OH(aq) → HCOOH(aq) + Cr³⁺(aq) (acidic solution) (d) BrO₃^-(aq) + N₂H₄(g) → Br^-(aq) + N₂(g) (acidic solution)

Textbook Question

Complete and balance the following equations, and identify the oxidizing and reducing agents. (Recall that the O atoms in hydrogen peroxide, H2O2, have an atypical oxidation state.)

a. S(s) + HNO3(aq) → H2SO3(aq) + N2O(g) (acidic solution)

b. BrO3-(aq) + N2H4(g) → Br-(aq) + N2(g) (acidic solution)

c. H2O2(aq) + ClO2(aq) → ClO20(aq) _ O2(g) (basic solution)