Question

ПОЖАЛУЙСТА!! ПОМОГИТЕ!! Сколько моль пирита надо сжечь , чтобы получить 980 г сернoй кислоты? Мr( H2SO4)=98

Answer 1

 дано
m(H2SO4)=980 g
-----------------------
n(FeS2)-?

FeS2+O2-->Fe2O3+SO2

SO2+O2-->SO3

SO3+H2O-->H2SO4
M(H2SO4)=98 g/mol
n(H2SO4)=m/M=980 / 98 = 10 mol
 из УХР видно n(FeS2) = n(H2SO4)=10 mol
n(FeS2)=10 mol
ответ 10 моль

Answer 2

Calculating the Amount of Pyrite Needed to Produce Sulfuric Acid

To calculate the amount of pyrite needed to produce 980g of sulfuric acid (H2SO4), we can use the stoichiometry of the reaction between pyrite (FeS2) and sulfuric acid. The balanced chemical equation for the reaction is:

FeS2 + 7O2 + 2H2O → Fe2(SO4)3 + 2H2SO4

From the balanced equation, we can see that 1 mole of pyrite (FeS2) reacts with 7 moles of oxygen (O2) and produces 2 moles of sulfuric acid (H2SO4).

Calculation Steps

1. Calculate the molar mass of sulfuric acid (H2SO4): - Molar mass of H2SO4 = (2 * atomic mass of H) + (1 * atomic mass of S) + (4 * atomic mass of O) - Molar mass of H2SO4 = (2 * 1.008) + 32.07 + (4 * 16.00) = 98.09 g/mol

2. Determine the number of moles of sulfuric acid produced: - Moles of H2SO4 = Mass of H2SO4 / Molar mass of H2SO4 - Moles of H2SO4 = 980g / 98.09 g/mol = 10 moles

3. Use the stoichiometry of the reaction to find the moles of pyrite needed: - According to the balanced equation, 1 mole of pyrite produces 2 moles of sulfuric acid. - Moles of pyrite needed = Moles of H2SO4 / 2 - Moles of pyrite needed = 10 moles / 2 = 5 moles

Therefore, 5 moles of pyrite need to be burned to produce 980g of sulfuric acid.