Balance this equation for the reaction occurring in an acidic solution. HNO2+ MnO4 →Mn²+ + NO3 HNO₂ + MnO4 → Mn²+ + NO3 O 3HNO2 + MnO4 → Mn2+ + 3NO3 + H₂O + H+ 5HNO₂ + 2MnO4+H2Mn2+ + 5NO3 + 3H₂O HNO₂ + MnO4 +5H+ → Mn2+ + NO3 + 3H₂O

Balance this equation for the reaction occurring in an acidic solution. HNO2+ MnO4 →Mn²+ + NO3 HNO₂ + MnO4 → Mn²+ + NO3 O 3HNO2 + MnO4 → Mn2+ + 3NO3 + H₂O + H+ 5HNO₂ + 2MnO4+H2Mn2+ + 5NO3 + 3H₂O HNO₂ + MnO4 +5H+ → Mn2+ + NO3 + 3H₂O

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 9QAP: Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid...

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Balance this equation for the reaction occurring in an acidic solution.
HNO2 + MnO4 → Mn²+ + NO3
HNO₂ + MnO4 → Mn²+ + NO3
O 3HNO2 + MnO4 → Mn2+ + 3NO3 + H₂O + H+
5HNO₂ + 2MnO4+H*→ 2Mn²+ + 5NO3¯ + 3H₂O
HNO₂ + MnO4 +5H+ → Mn2+ + NO3 + 3H₂O

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