Question

При выжигaнии пиритa FeS2 в кислороде обрaзуются оксиды ферумa(III) и сульфурa(IV). Вычислите объем (л)кислородa (н. у.), необходимый для взaимодействия с пиритом мaссой 6 кг.

Answer 1

    6кг      хм³
4FeS2+11O2=2Fe2O3+8SO2
   480г    246,4л                                  х=6*246,4/480=3,08м³

Answer 2

Calculation of Oxygen Volume Required for the Reaction

To calculate the volume of oxygen required for the reaction, we can use the stoichiometry of the reaction between pyrite (FeS2) and oxygen (O2).

The balanced chemical equation for the reaction is: 4FeS2(s) + 11O2(g) → 2Fe2O3(s) + 8SO2(g)

From the balanced equation, we can see that 11 moles of O2 are required to react with 4 moles of FeS2.

Given that the molar mass of FeS2 is approximately 119.98 g/mol and the molar mass of O2 is approximately 32 g/mol, we can proceed with the calculation.

Calculation Steps

1. Calculate the moles of FeS2: moles of FeS2 = mass of FeS2 / molar mass of FeS2 moles of FeS2 = 6000 g / 119.98 g/mol moles of FeS2 ≈ 50.01 mol

2. Use the mole ratio from the balanced equation to find the moles of O2 required: moles of O2 = moles of FeS2 × (11 moles of O2 / 4 moles of FeS2) moles of O2 ≈ 50.01 mol × (11 / 4) moles of O2 ≈ 137.77 mol

3. Convert moles of O2 to volume at standard conditions (0°C and 1 atm pressure): volume of O2 = moles of O2 × molar volume at n.t.p volume of O2 = 137.77 mol × 22.4 L/mol volume of O2 ≈ 3085.65 L

Answer

The volume of oxygen required for the reaction with 6 kg of pyrite is approximately 3085.65 liters at standard conditions (0°C and 1 atm pressure).