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postnew [5]
3 years ago
7

Consider the Fischer ester synthesis of methyl benzoate from benzoic acid and methanol in the presence of sulfuric acid as a cat

alyst. A reaction was performed in which 3.8 g of benzoic acid was reacted with excess methanol to make 2.0 g of methyl benzoate. Calculate the theoretical yield and percent yield for this reaction.
Chemistry
1 answer:
zlopas [31]3 years ago
4 0

Answer:

48.8%

Explanation:

The reaction has a 1:1 mole ratio so;

Number of moles of benzoic acid reacted = mass/molar mass = 3.8 g/122.12 g/mol = 0.03 moles

So;

0.03 moles of methyl benzoate is formed in the reaction

Mass of methyl benzoate formed = 0.03 moles * 136.15 g/mol = 4.1 g

percent yield = actual yield/theoretical yield * 100/1

percent yield = 2.0 g/4.1 g * 100 = 48.8%

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what is the molecular formula of a compound that contains 38% c, 45% n and 16% h if 0.157 g of the compound occupies 125 ml with
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The molecular formula of the given compound is CH₅N.

<h3>What is the ideal gas equation?</h3>

The ideal gas law has defined the product of the volume and pressure as equal to the product of the gas constant (R) and absolute temperature of the gas.

The mathematical equation of the ideal gas law is as follows:

PV = nRT

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The simplest ratio of C: N: H is 1 : 1 : 5

The empirical formula of the given compound is CH₅N.

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