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pstnonsonjoku

The mass of CO2 produced is 275 g.

What is combustion?

The term combustion refers to the situation in which a substance is burnt in oxygen. We have to first write down the equation of the reaction as follows;

[tex]CH_{4} + 2O_{2} ---- > CO_{2} + 2H_2}O[/tex]

Number of moles of methane = 100.0 g / 16 g/mol = 6.25 moles

Now;

1 mole of methane produces 1 mole CO2

6.25 moles of methane produces 6.25 moles of CO2

Mass of CO2 = 6.25 moles * 44 g/mol

= 275 g

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CintiaSalazar

Taking into account the reaction stoichiometry, 275 grams of CO₂ are formed in the complete combustion of 100.0 g of methane.

Reaction stoichiometry

In first place, the balanced reaction is:

CH₄ + 2 O₂ → CO₂ + 2 H₂O

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:

  • CH₄: 1 mole
  • O₂: 2 moles
  • CO₂: 1 mole
  • H₂O: 2 moles

The molar mass of the compounds is:

  • CH₄: 16 g/mole
  • O₂: 32 g/mole
  • CO₂: 44 g/mole
  • H₂O: 18 g/mole

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

  • CH₄: 1 mole ×16 g/mole= 16 grams
  • O₂: 2 moles ×32 g/mole= 64 grams
  • CO₂: 1 mole ×44 g/mole= 44 grams
  • H₂O: 2 moles ×18 g/mole= 36 grams

Mass of CO₂ formed

The following rule of three can be applied: if by reaction stoichiometry 16 grams of CH₄ form 44 grams of CO₂, 100 grams of CH₄ form how much mass of CO₂?

mass of CO₂= (100 grams of CH₄× 44 grams of CO₂)÷ 16 grams of CH₄

mass of CO₂= 275 grams

Finally, 275 grams of CO₂ are formed in the complete combustion of 100.0 g of methane.

Learn more about the reaction stoichiometry:

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brainly.com/question/24653699

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