The oxidation of 25 mL of a solution containing Fe²+ requires 3.0 × 10¹ mL of 0.0315 M K₂Cr₂O7 in acidic solution. Balance the following equation. Do NOT include the states of each species. Cr₂O72+ Fe²+ +H → Cr³+ + Fe³+ Calculate the molar concentration of Fe²+: M

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A:

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A: To find: The balanced equation for the given reaction

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Q: I Reactions please balance | Fe2+ MnO4!- Mn2+ Fe3+ oxidation, { el-s}: reduction, { el·'s}:

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A:

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A: Thank you.

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Q: For a particular redox reaction, BrO− is oxidized to BrO−3 and Fe3+ is reduced to Fe2+ . Complete…

A: BrO− is oxidized to BrO−3 and Fe3+ is reduced to Fe2+

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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.