A) Write out the full balanced reaction for the redox reaction involving sulfuric acid, potassium permanganate, and sodium oxalate to form manganese sulfate, carbon dioxide, potassium sulfate, sodium sulfate, and water. B) Write out the full ionic and net ionic equation for the reaction described in part b, provide the oxidation numbers for each atom, and indicate what the oxidizing and reducing agents are.

Q: Determine if a precipitation reaction would occur when an aluminum bromide solution is mixed with a…

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Q: Write the balanced molecular chemical equation for the reaction in aqueous solution for mercury(I)…

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Q: Balance the equation for the reaction of aluminum metal with solid iodine to form solid aluminum…

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Q: Describe examples of redox processes.

A: An Examples of redox reaction has to be given,

Q: In a hard water analysis, sodium oxalate solution reacts with calcium hydrogen carbonate (in the…

A: To write the net ionic equation for the reaction between sodium oxalate solution and calcium…

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Q: What is the net ionic equation for a reaction between Potassium Nitrate and Water?

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Q: Determine the oxidation state for each of the elements below. The oxidation state of manganese in…

A: Answer:Formal charge on an atom present in a specie is called its oxidation number in that specie.

Q: Does a reaction occur when aqueous solutions of chromium(II) nitrate and potassium carbonate are…

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A:

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A: The precipitation reaction refers to formation of insoluble salt , commonly called as precipitate ,…

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A:

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A:

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A: (a)

Q: Determine the oxidation state for each of the elements below. The oxidation state of carbon dioxide…

A: The oxidation state of the given compounds can be calculated as follows:

Redox Reactions

Redox reactions are considered to be the chemical reactions involving both oxidation and reduction processes. They are actually oxidation-reduction reactions. The term redox is made from two words where “red” comes from reduction and “ox” comes from oxidation. During a redox reaction electron transfer takes place in such a way that one chemical compound gets reduced and the other one gets oxidized.