Question

Hiw many grams of sulfur must be burned to give 0.567 moles of SO2?

Answer 1

18.1g

Explanation:

Given parameters:

Number of moles of SO₂ = 0.567moles

Unknown parameters:

Mass of Sulfur = ?

Solution:

The reaction equation is given below:

    S + O₂   ⇒    SO₂

To solve this problem, we work from the known to the unknown. This suggests that we use the number of moles of the product to work the mass of the sulfur.

  From the reaction equation,

         1 mole of SO₂ is produced by reacting 1 moles of S

    0.567moles of SO₂ will be produced by 0.567moles of S

Since we know the number of moles of the reactant, we can find the mass of sulfur now:

  Mass of sulfur = number of moles of sulfur x molar mass of sulfur

  Molar mass of S = 32g/mol

   Mass of sulfur = 0.567 x 32 = 18.1g

learn more:

Number of moles brainly.com/question/1841136

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