In a particular redox reaction, MnO₂ is oxidized to MnO₄⁻ and Ag⁺ is reduced to Ag. Complete and balance the equation for this reaction in acidic solution. Phases are optional.**Balanced redox reaction:**MnO₂ + Ag⁺ → MnO₄⁻ + Ag---This reaction demonstrates a redox process where manganese dioxide (MnO₂) is oxidized, indicating a loss of electrons, and silver ions (Ag⁺) are reduced, showing a gain of electrons. The balancing of charges and atoms is key in ensuring the conservation of mass and charge in the reaction.

Answered: Image /qna-images/answer/d78675f5-79b8-47fc-880e-48b55ce5726f.jpg

In a particular redox reaction, MnO., is oxidized to MnO, and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in acidic solution. Phases are optional. balanced redox reaction: MnO, + Ag* 2.

In a particular redox reaction, MnO., is oxidized to MnO, and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in acidic solution. Phases are optional. balanced redox reaction: MnO, + Ag* 2.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

3. Write the half-reactions (labelled as oxidation or reduction) for the following equation: Znjs) + 2 AGNO3(aq) → Zn (NO3)2(ag) +2 Ag(s)
You are tasked with creating a pourboix diagram of sulfur speciation. The relevent species are SO42-, HSO42-, S, H2S, and HS-. The total copper is 10^-6 mol. Set and balence the redox reactions needed for this question and explain how you landed on those reactions.
You are tasked with creating a pourboix diagram of copper speciation. The relevent species are Cu 1+, Cu 2+, Cu2O, and CuO. The total copper is 10^-3 mol. Set and balence the redox reactions needed for this question and explain how you landed on those reactions.
Balance the following reaction in acidic solution. Cr2O, (ag) + HNO,(aq) → Cr* (aq) + NO, (aq) 3 Fill in the coefficients for the balanced overall equation. HNO, + -- v H* + -v Cr.O,* → -- ♥ NO, +- Cr3+ + Cr,O, - H.O --V
Nn.112. Subject:- Chemistry
41. Balance each of the following equations according to the half-reaction method: (a) MnO4 (aq) + NO2 (aq) →→MnO2 (s) + NO3(aq) (in base) (b) MnO2 (aq)MnO4 (aq) + MnO2(s) (in base) (c) Br2(l) + SO2(g) → Br¯(aq) + SO4² (aq) (in acid)
4. Balance the following (redox) chemical equations using the half-reaction method, assuming acidic conditions: a. Br(aq) + NO2(aq) → Br2(aq) + NO(g) b. H2O2(aq) + S²(aq) → H2O(1) + S(s) c. Cu(s) + NO3(aq) → Cu²*(aq) + NO2(g)
Please do #9.
A. Balance the following redox reactions using the half-reaction method. B. Identify the oxidizing agent and the reducing agent. 1. Zn(s) + Fe²+ (aq) → Zn²+ (aq) + Fe (s) 2+ Zn(s) → Zn² +2e- oxidiation haut reaction (aq) 2+ 20+ Fe (an) → Fe (5) Reducation haut reaction (94) - Bris) Reducing agent (S) Fe 2+ oxidizing agent 2. (Balance this reaction In Acidic Solution):
Balance the following using the half-reaction method. Identify oxidation, reduction, reducing agent, oxidizing agent. i. Be(NO3)2 (aq) + Ce(s)--> Ce(NO3)3(aq) + Be(s) ii. A container contains H2SO3, H2SO4, Pb2+, Pb4+ and NO3- in distilled water. Create a balanced chemical reaction (Net Ionic Equation, including states of matter) for the spontaneous reaction in the container
c. For the unbalanced redox reaction Cu + 10 ➜→ Cu²+ + 1₂ Which is oxidizing agent (oxidant)? Write the balanced redox net ionic equation when the reaction is conducted in an acidic solution.