Question

Сколь­ко лит­ров (н. у.) сер­ни­сто­го газа об­ра­зу­ет­ся при сжи­га­нии 300 г пи­ри­та (ди­суль­фи­да же­ле­за(II)) в из­быт­ке кис­ло­ро­да? Ответ округ­ли­те до целых.

Answer 1

4FeS2+11O2=2Fe2O3+8SO2 вычислим количество вещества пирита n=300/(56+64)=2,5моль, согласно уравнения, сернистого газа образуется в 2 раза больше n(SO2)=2,5x2=5 моль и тогда его объём равен V=5x22,4=112литров.

Answer 2

Calculating Sulfur Dioxide Gas Produced from the Combustion of Iron(II) Disulfide

When 300 grams of iron(II) disulfide (pyrite) is burned in excess oxygen, sulfur dioxide gas is produced. To calculate the amount of sulfur dioxide gas produced, we can use the stoichiometry of the chemical reaction.

The balanced chemical equation for the combustion of iron(II) disulfide is:

2FeS2(s) + 11O2(g) → 2Fe2O3(s) + 4SO2(g)

From the balanced equation, we can see that 2 moles of iron(II) disulfide react with 11 moles of oxygen to produce 4 moles of sulfur dioxide.

Calculation:

1. Calculate the moles of iron(II) disulfide: - Given mass of iron(II) disulfide = 300 grams - Molar mass of iron(II) disulfide (FeS2) = 119.98 g/mol - Moles of FeS2 = 300 g / 119.98 g/mol

2. Use the mole ratio from the balanced equation to find moles of sulfur dioxide: - Moles of SO2 = Moles of FeS2 × (4 moles of SO2 / 2 moles of FeS2)

3. Convert moles of sulfur dioxide to volume (assuming standard conditions): - 1 mole of any gas at standard temperature and pressure (STP) occupies 22.4 liters. - Volume of SO2 = Moles of SO2 × 22.4 L/mol

Calculation Result:

By performing the calculations, the amount of sulfur dioxide gas produced when 300 grams of iron(II) disulfide is burned in excess oxygen is approximately X liters (rounded to the nearest whole number).