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guapka [62]
3 years ago
11

Given 7.45 g of butanoic acid and excess ethanol, how many grams of ethyl butyrate would be synthesized, assuming a complete 100

% yield? express your answer in grams to three significant figures.
Chemistry
1 answer:
KengaRu [80]3 years ago
3 0

The equation for the reaction is:

C₄H₈O₂ + C₂H₅OH = C₆H₁₂O₂ + H₂O

Now you see that the number of the moles of butanoic acid and etyl butyrate is equal in

the reaction. That means;

number of moles of C₄H₈O₂ = number of moles of C₆H₁₂O₂

mass of C₄H₈O₂/ Molar mass of C₄H₈O₂ = mass of C₆H₁₂O₂/ molar mass of C₆H₁₂O₂

mass of C₆H₁₂O₂ = molar mass of C₆H₁₂O₂ x mass of C₄H₈O₂/ Molar mass of C₄H₈O₂

Now, assuming <span>100% yield, the mass of ethyl butyrate produced is: </span>

<span>= 7.45/88.11 x 116.16</span>

<span>=9.82g</span>

<span>Thus, the theoretical yield of ethyl butyrate is 9.82g.</span>

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5 0
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Read 2 more answers
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The answers include:

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Calculate the mass of ethyl alcohol required to prepare 540 grams of C4H6, if the reaction follows the scheme:
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Answer:

Explanation:

2C₂H₅OH    =   C₄H₆  +  2H₂O  +  H₂

2 mole               1 mole

molecular weight of ethyl alcohol

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= 920 gm

ethyl alcohol required = 920 gm .

3 0
3 years ago
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