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qwelly [4]
3 years ago
6

A reaction was performed in which 3.7 g of benzoic acid was reacted with excess methanol to make 2.1 g of methyl benzoate. Calcu

late the theoretical yield and percent yield for this reaction.
Chemistry
1 answer:
Sav [38]3 years ago
4 0

Answer:

The theoretical yield is 4.13 grams methyl benzoate

The percent yield is 50.8 %

Explanation:

Step 1: Data given

Mass of benzoic acid = 3.7 grams

Mass of methyl benzoate = 2.1 grams

Molar mass of benzoic acid = 122.12 g/mol

Molar mass of methyl benzoate = 136.15 g/mol

Step 2: The balanced equation

C7H6O2 + CH3OH → C8H8O2 + H2O

Step 3: Calculate moles benzoic acid

Moles benzoic acid = mass benzoic acid / molar mass

Moles benzoic acid = 3.7 grams / 122.12 g/mol

Moles benzoic acid = 0.0303 moles

Step 4: Calculate moles methy benzoate

For 1 mol benzoic acid we'll have 1 mol methyl benzoate

For 0.0303 moles benzoic acid we'll have 0.0303 moles methyl benzoate

Step 5: Calculate mass methyl benzoate

Mass methyl benzoate = moles methyl benzoate * molar mass

Mass methyl benzoate = 0.0303 moles * 136.15 g/mol

Mass methyl benzoate = 4.13 grams

Step 6: Calculate % yield

% yield = (actual yield / theoretical yield ) * 100%

% yield = (2.1 grams / 4.13 grams ) *100%

% yield = 50.8 %

The theoretical yield is 4.13 grams methyl benzoate

The percent yield is 50.8 %

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Answer: 2.12\times 10^{25} atoms of hydrogen are there in

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Explanation:

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To calculate the moles, we use the equation:

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1 mole of hydrogen (H_2) = 2\times 6.023\times 10^{23}=12.05\times 10^{23} atoms

17.5 mole of hydrogen (H_2) = \frac{12.05\times 10^{23}}{1}\times 17.5=2.12\times 10^{25} atoms

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