Nicole0923
Answered

For the reaction So3 + H2O -> H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid

Answer :

CintiaSalazar

Answer:

320 grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid.

Explanation:

The balanced reaction is:

SO₃ + H₂O → H₂SO₄

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

  • SO₃: 1 mole
  • H₂O: 1 mole
  • H₂SO₄: 1 mole

Being the molar mass of each compound:

  • SO₃: 80 g/mole
  • H₂O: 18 g/mole
  • H₂SO₄: 98 g/mole

By reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

  • SO₃: 1 mole* 80 g/mole= 80 grams
  • H₂O: 1 mole* 18 g/mole= 18 grams
  • H₂SO₄: 1 mole* 98 g/mole= 98 grams

Then you can apply the following rule of three: if 1 mole of sulfuric acid is produced by the reaction of 80 grams of sulfur trioxide, 4 moles of sulfuric acid is produced from how much mass of sulfur trioxide?

[tex]mass of sulfur trioxide= \frac{4 moles of sulfuric acid* 80 grams of sulfur trioxide}{1 mole of sulfuric acid }[/tex]

mass of sulfur trioxide= 320 grams

320 grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid.

abidemiokin

The mass of the required compound is 320 grams

Chemical reactions

Given the chemical equation expressed as:

[tex]SO_3 + H_2O \rightarrow H_2SO_4[/tex]

According to stochiometry, 1 mole of SO3  produces 1 mole of H2SO4, hence the moles of SO3 will also be 4.00moles

Determine the mass of SO3

Mass = mole * molar mass

Mass = 4.0 * [32+3(16)]

Mass = 4.0 * 80

Mass = 320 grams

The mass of the required compound is 320 grams

Learn more on stoichiometry here:  https://brainly.com/question/16060223

Other Questions