Iron powder was dissolved in dilute sulfuric acid. Concentrated hydrogen peroxide was added to the solution

| June 2, 2021 | education

Iron powder was dissolved in dilute sulfuric acid. Concentrated hydrogen peroxide was added to the solution; as a result, the solution acquired a yellowish color. A solution of potassium sulfide was added to the resulting solution, resulting in a precipitate. The resulting precipitate was acted upon with a dilute solution of hydrochloric acid, and part of the precipitate was dissolved. The insoluble part of the precipitate had a yellow color. Make the equations for the four reactions described.

We compose the equations:
1. Fe + H2SO4 (P – P) = FeSO4 + H2 – substitution reaction.
2. FeSO4 + H2O2 + H2SO4 = Fe2 (SO4) 3 + 2H2O – redox reaction.
3. Fe2 (SO4) 3 + 3K2S = FeS + 3K2SO4 – the ion exchange reaction leads to the formation of a yellow precipitate of iron sulfide.
4. FeS + 2HCL = H2S + FeCL2 – ion exchange reaction.
Iron sulfide dissolves in dilute hydrochloric acid and is used to produce hydrogen sulfide in the laboratory. In the course of the reactions carried out, iron salts were obtained: FeSO4; Fe2 (SO4) 3, FeS, FeCL2.



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