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3 years ago

How many liters of oxygen are needed to react completely with 25.0 L of H2S at STP?

Chemistry

1 answer:

HACTEHA [7]3 years ago

3 0

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

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