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Write a proposed reaction for the oxidation-reduction of copper (II) iodide. Justify the choice of the substance that reduces the copper, based on the fact that a precipitate forms when copper nitrate and potassium iodide react, even though solubility rules would contradict this fact. Also, justify the choice using the atomic structure of potassium ion and iodide ion.

Sagot :

2Cu2^+ + 2I^- ----> 2Cu^+ + I2

The reaction performed in the experiment is;

2 Cu(NO3)2 + 4 KI → 2 CuI (s) + 4 KNO3 + I2

What is redox reaction?

A reaction that happens when an oxidizing substance and a reducing substance come into contact. In the reaction, the reducing substance obtains electrons while the oxidizing substance loses electrons.

The precipitate results from the reduction of Cu2+ by iodide ions to Cu+, which is insoluble in water. Iodine is a good oxidizing agent, and since its outermost shell must be filled with one electron, this is why. On the other hand, because it may quickly lose its one electron, potassium makes a good reducing agent.

The oxidation - reduction equation is as follows;

2Cu2^+ + 2e ----> 2Cu^+ reduction half equation

2I^- ----> I2 + 2e. Oxidation half equation

Balanced redox reaction equation;

2Cu2^+ + 2I^- ----> 2Cu^+ + I2

For more information regarding redox reaction equation, visit:

https://brainly.com/question/10203480

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