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2 years ago

2HgO(s) 2Hg(l) + O2(g)

Chemistry

1 answer:

WITCHER [35]2 years ago

5 0

The theoretical yield of the Hg is 4.02 g.

<h3>What s the theoretical yield?</h3>

The theoretical yield is the yield that is obtained from the stoichiometry of the reaction.

The reaction equation is; 2HgO(s) ------> 2Hg(l) + O2(g)

Number of moles of HgO = 4.37 g/217 g/mol = 0.02 moles

Number of moles of Hg = 3.21 g/201 g/mol = 0.012 moles

Now;

Theoretical yield of Hg = 0.02 moles * 201 g/mol = 4.02 g

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Ammonium phosphate ((NH4)3PO4) is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid (H3PO4

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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

<h3>Mass of ammonium phosphate formed</h3>

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= $\frac{5.82 grams of H_{3} PO_{4}x149 grams of (NH_{4} )_{3}PO_{4} }{98 grams of H_{3} PO_{4}}$

<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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