Taking into account definition of percent yield, the theoretical yield is:
In first place, the balanced reaction is:
2 Fe + 3 H₂SO₄ → Fe₂(SO₄)₃ + 3 H₂
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:
The molar mass of the compounds is:
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
Fe: 2 moles ×55.85 g/mole= 111.7 grams
H₂SO₄: 3 moles ×98 g/mole= 294 grams
Fe₂(SO₄)₃: 1 mole ×399.7 g/mole= 399.7 grams
H₂: 3 moles ×2 g/mole= 6 grams
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction.
To determine the limiting reagent, it is possible to use a simple rule of three as follows: if by stoichiometry 111.7 grams of Fe reacts with 294 grams of H₂SO₄, 1.4 grams of Fe reacts with how much mass of H₂SO₄?
[tex]mass of H_{2} SO_{4} =\frac{1.4 grams of Fex 294 grams of H_{2} SO_{4}}{111.4 grams of Fe}[/tex]
mass of H₂SO₄= 3.6849 grams
But 3.6849 grams of H₂SO₄ are not available, 3.4 grams are available. Since you have less mass than you need to react with 1.4 grams of Fe, H₂SO₄ will be the limiting reagent.
The theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.
Considering the limiting reagent, the following rule of three can be applied:
[tex]mass of Fe_{2} (SO_{4} )_{3} =\frac{3.4 grams of H_{2} SO_{4} x399.7 grams of Fe_{2} (SO_{4} )_{3} }{294 grams of H_{2} SO_{4} }[/tex]
mass of Fe₂(SO₄)₃= 4.6224 grams
[tex]mass of H_{2} =\frac{3.4 grams of H_{2} SO_{4} x6 grams of H_{2} }{294 grams of H_{2} SO_{4} }[/tex]
mass of H₂= 0.0694 grams
Finally, the theoretical yield is:
Learn more about
the reaction stoichiometry:
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theoretical yield:
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