The
balanced reaction would be written as:
<span>
C7H6O3 + C4H6O3--->C9H8O4 + HC2H3O2
To determine the percent yield, we need to first
determine the theoretical yield if the reaction were to proceed completely.
Then, we divide the actual yield that is given to the theoretical yield times
100 percent. The limiting reactant from the reaction would be salicylic acid.
We do as follows:
<span>Theoretical yield: 50.05 g C7H6O3 ( 1 mol /
138.21 g ) ( 1 mol C9H8O4 / 1 mol C7H6O3 ) ( 180.157 g / mol ) = 65.24 g C9H8O4 should be produced
Percent yield = 55.45 / 65.24 x 100 = 84.99%
<span>
Therefore, the percent yield for the given amount of salicylic acid is 84.99%
</span></span></span><span><span><span>
</span></span></span>
The answer is: "Twelve (12) moles of Fe (iron) would be required."
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or:
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The answer is: "12" .
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Note: The balanced chemical equation is given:
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4 Fe + 3 O₂ → 2 Fe₂O₃
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The product is: 2 moles of Fe₂O₃ ; that is, "2 moles of iron (III) oxide" .
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→ If SIX (6) moles of iron oxide were produced, that would be "3 (three) times the number of moles of iron oxide produced (3 TIMES 2) ;
→ since: "6 ÷ 2 = 3" ; and since the equation is balanced.
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→ So we want to find the number of moles of "iron (Fe)" needed in such a situation. In the balanced chemical, we have "4 Fe" (that is, "FOUR (4) moles of iron") ; so we multiply that number by "3", proportionally:
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→ 4 (moles Fe) * (3) = 12 (moles Fe) .
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It pushes the positive ions together, the positive ions repel each other, causing the crystal to shatter