molar mass 186.03 g/mol]can be prepared by reacting 3.0 g of FeCl2(s) [molar mass =126.75 g/mol] with 5.7 g of cyclopentadiene [C5H6(l);molar mass 66.01 g/mol]and an excess of KOH

Ferrocene, [Fe(C10H10)(s) ;molar mass 186.03 g/mol]can be prepared by reacting 3.0 g of FeCl2(s) [molar mass =126.75 g/mol] with 5.7 g of cyclopentadiene [C5H6(l);molar mass 66.01 g/mol]and an excess of KOH, as shown in the following reaction  FeCl2 + 2C5H6 + 2KOH → FeC10H10 + 2H2O  A student who carried out this reaction obtained 2.7 g of ferrocene. Of the following choices which has three correct answers?  is limiting; 4.40 g of ferrocene could be theoretically formed; obtained 61.36 % yield
Ferrocene, [Fe(C10H10)(s) ;molar mass 186.03 g/mol]can be prepared by reacting 3.0 g of FeCl2(s) [molar mass =126.75 g/mol] with 5.7 g of cyclopentadiene [C5H6(l);molar mass 66.01 g/mol]and an excess of KOH, as shown in the following reaction

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FeCl2 + 2C5H6 + 2KOH → FeC10H10 + 2H2O

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A student who carried out this reaction obtained 2.7 g of ferrocene. Of the following choices which has three correct answers?

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is limiting; 4.40 g of ferrocene could be theoretically formed; obtained 61.36 % yield

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is limiting; 2.82 g of ferrocene could be theoretically formed; obtained 95.7 % yield

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is limiting; 4.2 g of ferrocene could be theoretically formed; obtained 54.6 % yield

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is limiting; 0.0151 g of ferrocene could be theoretically formed; obtained 74.8 % yield

The Correct Answer and Explanation is :

The correct answer is:

• FeCl2 is limiting.
• 4.40 g of ferrocene could be theoretically formed.
• Obtained 61.36% yield.

Explanation:

1. Limiting Reactant:
   In the given reaction, FeCl2 and cyclopentadiene (C5H6) react in a 1:2 ratio. The moles of FeCl2 are less than half the moles of C5H6, which means FeCl2 is the limiting reagent.
2. Theoretical Yield:
   The limiting reagent (FeCl2) dictates the maximum amount of product that can be formed. From the moles of FeCl2 (3.0 g / 126.75 g/mol = 0.0237 mol), the theoretical yield of ferrocene can be calculated using the stoichiometric ratio (1 mole of FeCl2 forms 1 mole of ferrocene).
   The theoretical yield is therefore approximately 4.40 g of ferrocene.
3. Percent Yield:
   The percent yield is calculated by dividing the actual yield (2.7 g) by the theoretical yield (4.40 g) and multiplying by 100. This results in approximately 61.36%, which matches the given answer.

Now, let’s generate an image to illustrate the reaction.

Here is the chemical reaction diagram for the preparation of ferrocene, showing the reactants, products, and the balanced equation. Let me know if you need any further explanations!