From iron sulfide (||) hydrogen sulfide was obtained, the combustion of which consumed 306 liters

From iron sulfide (||) hydrogen sulfide was obtained, the combustion of which consumed 306 liters of oxygen. What is the mass of FeS?

Hydrogen sulfide from iron sulfide can be obtained as a result of the interaction of FeS with hydrochloric acid:

FeS + 2 HCl = FeCl2 + H2S [1]

Hydrogen sulfide burns in an excess of oxygen with the formation of water and sulfur dioxide:

2 H2S + 3 O2 = 2 H2O +2 SO2 [2]

To solve the problem, let us first calculate the volume of hydrogen sulfide using equation [2], and then, using the reaction equation [1], calculate the mass of iron sulfide.

Molar mass FeS = 88 g / mol. Gases according to Avogadro’s law have the same molar volume equal to 22.4 l / mol

We calculate the volume of hydrogen sulfide according to the equation [2]:

X l. hydrogen sulfide corresponds to 306 liters of oxygen, as

2 * 22.4 l / mol of hydrogen sulfide corresponds to 3 * 22.4 l / mol of oxygen.

X = (306 * 2 * 22.4) / (3 * 22.4) = 204 liters of H2S

According to the equation [1], we now calculate the mass of sulfur sulfide:

Y g sulfur sulfide corresponds to 204 liters. hydrogen sulfide as

88 g / mol of sulfur sulfide corresponds to 22.4 l / mol of hydrogen sulfide.

Y = (204 * 88) / 22.4 = 801.4 g. FeS

Answer: the mass of iron sulfide is 801.4 g.