Taking into account the reaction stoichiometry, 5.2634 grams of Cu(NO₃)₂ are formed when 4.69 grams of HNO₃, assuming an excess of solid copper is present.
<h3>Reaction stoichiometry</h3>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 mole
- NO: 2 moles
- H₂O: 4 moles
The molar mass of the compounds is:
- Cu: 63.55 g/mole
- HNO₃: 63 g/mole
- Cu(NO₃)₂: 187.55 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 ×63.55 g/mole= 190.65 grams
- HNO₃: 8 moles ×63 g/mole= 504 grams
- Cu(NO₃)₂: 3 moles ×187.55 g/mole= 562.65 grams
- NO: 2 moles ×30 g/mole= 60 grams
- H₂O: 4 moles ×18 g/mole= 72 grams
The following rule of three can be applied: if by reaction stoichiometry 504 grams of HNO₃ form 562.65 grams of Cu(NO₃)₂, 4.69 grams of HNO₃ form how much mass of Cu(NO₃)₂?
<u><em>mass of Cu(NO₃)₂= 5.2634 grams</em></u>
Then, 5.2634 grams of Cu(NO₃)₂ are formed when 4.69 grams of HNO₃, assuming an excess of solid copper is present.
Learn more about the reaction stoichiometry:
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