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If you answer this please include the steps because I used to know how to do these problems really well I just forgot how.

Hydrogen sulfide gas, which smells like rotten eggs, burns in air to produce sulfur
dioxide and water. How many moles of oxygen gas would be needed to completely
burn 8 moles of hydrogen sulfide?

Respuesta :

Answer:

12 moles of oxygen gas

Explanation:

  • 2H₂S + 3O₂ => 2SO₂ + 2H₂O [balanced equation]
  • For every 2 moles  of hydrogen sulfide gas, 3 moles of oxygen is required
  • Therefore, 8 moles of hydrogen sulfide requires 12 moles of oxygen gas

mickymike92

12 moles of oxygen gas would be needed to completely burn 8 moles of hydrogen sulfide.

What is mole ratio of a reaction?

The mole ratio of a reaction is a ratio showing the how moles of reactants combine to form products or the ratio of moles if products formed to the moles of reactants used up.

The balanced equation of the reaction is given below:

[tex]2H_{2}S + 3O_{2}\rightarrow 2H_{2}O + SO_{2}[/tex]

3 moles of oxygen reacts completely with 2 moles of hydrogen sulphide.

8 moles of hydrogen sulphide will require 3 × 8/2 moles of oxygen = 12 moles of oxygen.

Therefore, 12 moles of moles of oxygen gas would be needed to completely burn 8 moles of hydrogen sulfide.

Learn more about mole ratio at: https://brainly.com/question/19099163

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