Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (a) Mo 3+ (aq) → Mo(s) (acidic solution) (b) H 2 SO 3 (aq) → SO 4 2- (aq) (acidic solution) (c) NO 3 - (aq) → NO(g) (acidic solution) (d) O 2 (g) → H 2 O(l) (acidic solution)

every once you were asked about the balance half reactions under acidic conditions and identify whether it is an oxidation reduction reaction. We need to first write this reaction out with B R minus eight years. And this yields 7 2. Like when we need to first balance the non hydrogen and non oxygen elements first, it's gonna be brimming. We have one brought me on the wrapped inside but to on the product side they can put a two in front of B R 03 minus. And just to balance it so now we can balance the oxygen by adding H 20 liquid to the side. That needs oxygen. We have six oxygen on the wrapping side but none on the product side drink it as six H 20 liquid to the product side. Now we can bounce our hydrogen by adding H plus to the side that needs hydrogen. We have no hydrogen on the reactive side. We have 12 on the product side. Look at 12 h plus the react inside. Now we can balance the charges by adding electrons to the more positive side. Also get our charges plus 12 here -2 Here, right here, right here Have a plus 10 over here and over here overall. So this means we need to add 10 electrons on the reactant side. For the balance reaction, I'm gonna get to the R 03 minus grants Plus 12 h plus eight plus electrons. It's gonna be our two. Like when Plus six H 20. And for our oxidation reaction, this means we're losing electrons electrons gonna be on the product side for the reduction reaction, this means we're gaining electrons so the electrons going to be on the reactive side. On this case, this is a reduction reaction because we have electrons on the left side, we're gaining electrons. Thanks for watching my video. And I hope it was helpful.

Ch.20 - Electrochemistry

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Brown 14th Edition

Ch.20 - Electrochemistry

Problem 24a,b,c,d

Chapter 20, Problem 24a,b,c,d

Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (a) Mo³⁺(aq) → Mo(s) (acidic solution) (b) H₂SO₃(aq) → SO₄^2-(aq) (acidic solution) (c) NO₃^-(aq) → NO(g) (acidic solution) (d) O₂(g) → H₂O(l) (acidic solution)

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Identify the oxidation states of sulfur in H_2SO_3 and SO_4^{2-}.

Determine the change in oxidation state to identify if it is oxidation or reduction.

Balance the sulfur atoms on both sides of the equation.

Balance the oxygen atoms by adding H_2O molecules to the side that needs more oxygen.

Balance the hydrogen atoms by adding H^+ ions to the side that needs more hydrogen.

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Key Concepts

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

Half-Reactions

Half-reactions are the individual oxidation or reduction processes that occur in a redox reaction. They represent the transfer of electrons, with oxidation involving the loss of electrons and reduction involving the gain of electrons. Balancing half-reactions is essential for understanding the overall redox process and ensuring that the number of electrons lost equals the number gained.

Oxidation and Reduction

Oxidation is defined as the process where a substance loses electrons, resulting in an increase in oxidation state, while reduction is the gain of electrons, leading to a decrease in oxidation state. In redox reactions, one species is oxidized and another is reduced, and identifying these processes is crucial for balancing chemical equations and understanding reaction mechanisms.

Balancing Redox Reactions in Acidic Solution

When balancing redox reactions in acidic solutions, it is important to account for hydrogen ions (H+) and water (H2O) to ensure mass and charge balance. The steps typically involve separating the half-reactions, balancing the atoms other than O and H, then balancing O with H2O and H with H+. Finally, the charges are balanced by adding electrons, which helps in determining the overall balanced equation.

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Balancing Acidic Redox Reactions

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Textbook Question

Hydrazine (N₂H₄) and dinitrogen tetroxide (N₂O₄) form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N₂ and H₂O. (c) Which substance serves as the reducing agent and which as the oxidizing agent?

Textbook Question

Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (a) Sn²⁺(aq) → Sn⁴⁺(aq) (acidic solution) (b) TiO₂(s) → Ti²⁺(aq) (acidic solution) (c) ClO₃^-(aq) → Cl^-(aq) (acidic solution) (d) N₂(g) → NH₄⁺(aq) (acidic solution)

Textbook Question

Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (f) SO32-1aq2 ¡ SO42-1aq2 (basic solution)

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Textbook Question

Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (g) Cr(OH)₃(s) → CrO₄^2-(aq) (basic solution)

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: As₂O₃(s) + NO₃^-(aq) → H₃AsO₄(aq) + N₂O₃(aq) (acidic solution)

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Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (a) Mo3+(aq) → Mo(s) (acidic solution) (b) H2SO3(aq) → SO42-(aq) (acidic solution) (c) NO3-(aq) → NO(g) (acidic solution) (d) O2(g) → H2O(l) (acidic solution)

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Key Concepts

Half-Reactions

Oxidation and Reduction

Balancing Redox Reactions in Acidic Solution