Answer:
37.5 L
Explanation:
Data Given
volume of H₂S = 25.0 L
volume of O₂ = ?
Solution:
Reaction of Oxygen and H₂S is as below
2H₂S + 3O₂ ----------> 2SO₂ + 2H₂O
2 mole 3 mole
we come to know that 2 mole of H₂S combine with 3 mole of O₂ and produce SO₂ and water
So,
Now we will calculate that how many liters of O₂ is Required to react with H₂S
So for this first we find moles of 25.0 L H₂S
no. of moles = Volume in dm³ / molar volume at STP (22.4 dm³/mol)
So, we know
1 dm³ = 1 L
Put values in the above formula:
no. of moles = 25 L / 22.4 L /mol
no. of moles = 1.11 mol
So now apply Unity formula
if 2 mole of H₂S react with 3 mole of O₂ then how many mole will react with 1.11 mol of H₂S
2 mole of H₂S ≅ 3 mole of O₂
1.11 mole of H₂S ≅ ? mole of O₂
by doing cross multiplication
mole of O₂ = 3 mole x 1.11 mole / 2 mole
mole of O₂ = 1.67 mol
Now,
Convert mole to volume by using below formula
no. of moles = Volume in dm³ / 22.4 dm³/mol
Rearrange the above equation
Volume in dm³ = no. of moles x 22.4 dm³/mol
Put values in above equation
Volume in dm³ = 1.67 mol x 22.4 dm³/mol
Volume in dm³ = 37.5 dm³ or L
So 37.5 L of volume is required to react with 25 L of H₂S
