Question

Определите массовые доли (в%) сульфата железа (II) и сульфида железа (II) в смеси, если при обработке 32 г этой смеси соляной кислотой выделился газ, который полностью прореагировал с 640 г 5% ного раствора сульфата меди(II)

Answer 1

Надеюсь, все правильно)

Answer 2

Calculation of Mass Fractions of Iron(II) Sulfate and Iron(II) Sulfide

To determine the mass fractions of iron(II) sulfate (FeSO4) and iron(II) sulfide (FeS) in the mixture, we need to use the given information about the reaction between the mixture and hydrochloric acid (HCl), as well as the reaction between the released gas and copper(II) sulfate (CuSO4).

Let's break down the problem step by step:

1. Reaction between the Mixture and Hydrochloric Acid: - The mixture, weighing 32 g, reacts with hydrochloric acid (HCl). - The reaction produces a gas, which is assumed to be hydrogen sulfide (H2S). - The gas completely reacts with 640 g of a 5% solution of copper(II) sulfate (CuSO4).

2. Reaction between Hydrogen Sulfide and Copper(II) Sulfate: - Hydrogen sulfide (H2S) reacts with copper(II) sulfate (CuSO4) to form copper(II) sulfide (CuS) and sulfuric acid (H2SO4). - The reaction is assumed to be complete.

To calculate the mass fractions of FeSO4 and FeS, we need to determine the amount of hydrogen sulfide (H2S) produced in the reaction between the mixture and hydrochloric acid. Then, we can use stoichiometry to find the corresponding amounts of FeSO4 and FeS.

Calculation Steps:

1. Calculate the amount of hydrogen sulfide (H2S) produced: - The molar mass of H2S is 34.08 g/mol. - Using the ideal gas law, we can calculate the number of moles of H2S produced: - n(H2S) = (PV) / (RT) - P = pressure of the gas (not given) - V = volume of the gas (not given) - R = ideal gas constant (