Answer:
514.8 grams of H₂O would be produced.
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?
[tex]mass of water=\frac{14.3 moles of methane*36 grams of water}{1 mole of methane}[/tex]
mass of water= 514.8 grams
514.8 grams of H₂O would be produced.
