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14.3 moles of methane (CH4) burns completely, find the grams of H20 would be produced CH4 + 202 CO2 + 2H20 w​

User Nick Turner
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Answer:

514.8 grams of H₂O would be produced.

Step-by-step explanation:

The balanced reaction is:

CH₄ + 2 O₂ → CO₂ + 2 H₂O

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

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

Being the molar mass of each compound:

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

By stoichiometry, the following amounts of mass 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

You can apply the following rule of three: if 1 mole of methane produces 36 grams of water, 14.3 moles of methane produces how much mass of water?


image

mass of water= 514.8 grams

514.8 grams of H₂O would be produced.

User Awalias
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