Answer :
Taking into account the reaction stoichiometry, 120.615 kg of HNO₃ are consumed to produce 112 kg Ca(H₂PO₄)₂.
Reaction stoichiometry
In first place, the balanced reaction is:
Ca₃(H₂PO₄)₂ + 4 HNO₃ → Ca(H₂PO₄)₂ + 2 Ca(NO₃)₂
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:
- Ca₃(H₂PO₄)₂: 1 mole
- HNO₃: 4 moles
- Ca(H₂PO₄)₂: 1 mole
- Ca(NO₃)₂: 2 moles
The molar mass of the compounds is:
- Ca₃(H₂PO₄)₂: 314 g/mole
- HNO₃: 63 g/mole
- Ca(H₂PO₄)₂: 234 g/mole
- Ca(NO₃)₂: 164 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction (being 1000 g= 1 kg):
- Ca₃(H₂PO₄)₂: 1 mole ×314 g/mole= 314 grams= 0.314 kg
- HNO₃: 4 moles ×63 g/mole= 252 grams= 0.252 kg
- Ca(H₂PO₄)₂: 1 mole ×234 g/mole= 234 grams= 0.234 kg
- Ca(NO₃)₂: 2 moles ×164 g/mole= 328 grams= 0.328 kg
Mass of HNO₃ required
The following rule of three can be applied: If by reaction stoichiometry 0.234 kg of Ca(H₂PO₄)₂ is produced from 0.252 kg of HNO₃, 112 kg of Ca(H₂PO₄)₂ is produced from how much mass of HNO₃?
mass of HNO₃= (112 kg of Ca(H₂PO₄)₂× 0.252 kg of HNO₃)÷ 0.234 kg of Ca(H₂PO₄)₂
mass of HNO₃= 120.615 kg
Finally, 120.615 kg of HNO₃ are consumed to produce 112 kg Ca(H₂PO₄)₂.
Learn more about the reaction stoichiometry and how to get quantity of product:
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