Question

провели электролиз раствора хлорида натрия. к полученому раствору добавили хлорид железа(III). выпавший осадок отфильтровали и прокалили. твердый осадок растворили в иодоводородной кислоте. напишите уровнения четырех описанных реакций

Answer 1

пишу без коэффициентов.

NaCl + H2O (e.t.) = NaOH + Cl2 + H2

FeCl3 + NaOH= Fe(OH)3 + NaCl

Fe(OH)3 (t) = Fe2O3 + H2O

Fe2O3 + HI = FeI2 + I2 + H2O

Answer 2

Electrolysis of Sodium Chloride Solution:

The electrolysis of a sodium chloride (NaCl) solution involves the decomposition of water and the formation of chlorine gas (Cl2) and hydrogen gas (H2) at the electrodes. The overall reaction can be represented as follows:

2 NaCl(aq) + 2 H2O(l) → 2 NaOH(aq) + Cl2(g) + H2(g).

Addition of Iron(III) Chloride to the Obtained Solution:

When iron(III) chloride (FeCl3) is added to the solution obtained from the electrolysis of sodium chloride, a precipitation reaction occurs. Iron(III) chloride reacts with sodium hydroxide (NaOH) to form iron(III) hydroxide (Fe(OH)3) as a solid precipitate and sodium chloride (NaCl) remains in solution. The balanced equation for this reaction is:

FeCl3(aq) + 3 NaOH(aq) → Fe(OH)3(s) + 3 NaCl(aq).

Filtration and Calcination of the Precipitate:

The solid precipitate of iron(III) hydroxide (Fe(OH)3) is then filtered to separate it from the solution. The precipitate is then subjected to calcination, which involves heating the solid to a high temperature to convert it into another compound. In this case, calcination of iron(III) hydroxide results in the formation of iron(III) oxide (Fe2O3). The balanced equation for this reaction is:

2 Fe(OH)3(s) → Fe2O3(s) + 3 H2O(g).

Dissolution of the Solid Precipitate in Hydroiodic Acid:

The solid iron(III) oxide (Fe2O3) obtained from the calcination step is dissolved in hydroiodic acid (HI). This reaction results in the formation of iron(III) iodide (FeI3) and water (H2O). The balanced equation for this reaction is:

Fe2O3(s) + 6 HI(aq) → 2 FeI3(aq) + 3 H2O(l).

Please note that the specific reaction conditions and concentrations of the solutions may affect the reaction outcomes.