Taking into account the reaction stoichiometry, 8.8488 grams of (NH₄)₃PO₄ is produced by the reaction of 5.82g of phosphoric acid.
<h3>Reaction stoichiometry</h3>In first place, the balanced reaction is:
H₃PO₄ + 3 NH₃ → (NH₄)₃PO₄
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:
- H₃PO₄: 1 mole
- NH₃: 3 moles
- (NH₄)₃PO₄: 1 mole
The molar mass of the compounds is:
- H₃PO₄: 98 g/mole
- NH₃: 17 g/mole
- (NH₄)₃PO₄: 149 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- H₃PO₄: 1 mole ×98 g/mole= 98 grams
- NH₃: 3 moles ×17 g/mole= 51 grams
- (NH₄)₃PO₄: 1 mole ×149 g/mole= 149 grams
The following rule of three can be applied: if by reaction stoichiometry 98 grams of H₃PO₄ form 149 grams of (NH₄)₃PO₄, 5.82 grams of H₃PO₄ form how much mass of (NH₄)₃PO₄?
mass of (NH₄)₃PO₄=
<u><em>mass of (NH₄)₃PO₄= 8.8488 grams</em></u>
Finally, 8.8488 grams of (NH₄)₃PO₄ is produced by the reaction of 5.82g of phosphoric acid.
Learn more about the reaction stoichiometry:
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