Taking into account the reaction stoichiometry, 47.655 grams of Cu is required to react with 2 moles of HNO₃.
Reaction stoichiometry
In first place, 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 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, the following mass quantities 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 Cu required
The following rule of three can be applied: If by reaction stoichiometry 8 moles of HNO₃ react with 190.62 grams of Cu, 2 moles of HNO₃ react with how much mass of Cu?
[tex]mass of Cu=\frac{2 moles of HNO_{3} x190.62 grams of Cu}{8 moles of HNO_{3} }[/tex]
mass of Cu= 47.655 grams
Finally, 47.655 grams of Cu is required to react with 2 moles of HNO₃.
Learn more about the reaction stoichiometry:
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