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CH4​+2O2​→CO2​+2H2O How many grams of \text{CO}_2CO 2 ​ start text, C, O, end text, start subscript, 2, end subscript will be produced from 12.0 \text{ g}12.0 g12, point, 0, start text, space, g, end text of \text{CH}_4CH 4 ​ start text, C, H, end text, start subscript, 4, end subscript and 133 \text{ g}133 g133, start text, space, g, end text of \text{O}_2O 2 ​ start text, O, end text, start subscript, 2, end subscript?

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Answer:

  • 33.0 g

Explanation:

Rewrite the question for better understanding:

  • CH₄ + 2O₂ → CO₂ + 2H₂O. How many grams of CO₂ will be produced from 12.0g of CH₄ and 133g of O₂?

Solution

1. Write the mole ratio

  • 1mol CH₄ : 2mol H₂O

2. Convert the masses of CH₄ and O₂ to number of moles

  • number of moles = mass in grams / molar mass

  • molar mass of CH₄ ≈ 16.0g/mol

  • number of moles of CH₄ = 12.0g / (16.0g/mol) = 0.750 mol

  • molar mass of O₂ ≈ 16.0g/mol

  • number of moles of O₂ = 133g/(16.0g/mol) = 8.3125 mol

Since 1 mole of CH₄ react with 2 moles of O₂, 0.750 mole of CH₄ need 1.50 moles of O₂, which means that there is O₂ in excess and the limiting reactant is CH₄.

Since every mole of CH₄ produced one mole of CO₂, 0.750 moles of CH₄ will produce 0.75 moles of CO₂.

To convert moles to grams, multiply by the molar mass.

  • mass = number of moles × molar mass
  • molar mass of CO₂ ≈ 44.0g/mol
  • mass = 0.750 mol × 44.0g/mol = 33.0g ← answer

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