Considering the reaction stoichiometry, the mass of H₂O that is produced when 11.9 moles of HNO₃ react is 107.1 grams.
Reaction stoichiometry
The balanced reaction is:
3 Cu + 8 HNO₃ → 3 Cu(NO₃)₂ + 2 NO + 4 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:
- Cu: 3 moles
- HNO₃: 8 moles
- Cu(NO₃)₂: 3 moles
- NO: 2 moles
- H₂O: 4 moles
The molar mass of the compounds present in the reaction is:
- Cu: 63.54 g/mole
- HNO₃: 63 g/mole
- Cu(NO₃)₂: 187.54 g/mole
- NO: 30 g/mole
- H₂O: 18 g/mole
Then, by reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of mass of each compound participate in the reaction:
Cu: 3 moles ×63.54 g/mole= 190.62 grams
HNO₃: 8 moles ×63 g/mole= 504 grams
Cu(NO₃)₂: 3 moles ×187.54 g/mole= 562.62 grams
NO: 2 moles ×30 g/mole= 60 grams
H₂O: 4 moles ×18 g/mole= 72 grams
Mass of H₂O produced
It is possible to determine the the amount of mass of H₂O produced by a rule of three: if by stoichiometry 8 moles of HNO₃ produce 72 grams of H₂O, if 11.9 moles of HNO₃ react how much mass of H₂O will be formed?
[tex]mass of H_{2}O=\frac{11.9 moles of HNO_{3} x72 grams of H_{2}O}{8 moles of HNO_{3}}[/tex]
mass of H₂O= 107.1 grams
In summary, the mass of H₂O that is produced when 11.9 moles of HNO₃ react is 107.1 grams.
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