Question

Methyl butyrate is a compound that is partially responsible for the flavor of apples. It consists...

Methyl butyrate is a compound that is partially responsible for the flavor of apples. It consists of 58.80% C, 9.87% H, and 31.33% O. What is the empirical formula of methyl butyrate? Explain.

Homework Answers

Answer #1

Assume you have 100g of the sample, in which

mass of C = 58.80g

mass of H = 9.87g

mass of O = 31.33g

Now calculate the number of moles of the above species

Number of moles = Mass given / Molecular mass

No. of moles (C) = 58.80 / 12.01 = 4.90

No. of moles (H) = 9.87 / 1.008 = 9.79

No. of moles (O) = 31.33 / 16.0 = 1.95

Now, Divide each mole value by the smallest number of moles calculated.

4.90 / 1.95 =2.5

9.79 / 1.95 = 5.0

1.95 / 1.95 = 1

Now, Round to the nearest whole number. (Multiply by 2)

moles of C = 5

Moles of H = 10

moles of O = 2

Therefore empirical formula comes out to be C5H10O2.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Putrescine is a compound that is partially responsible for the rotten smell of decaying flesh. It...
Putrescine is a compound that is partially responsible for the rotten smell of decaying flesh. It consists of 54.50% C, 13.73% H, and 31.77% N. What is the empirical formula of putrescine?
an unknown compound contains only c h and o. Combustion of 5.60g of this compound is...
an unknown compound contains only c h and o. Combustion of 5.60g of this compound is produced, 13.7 of CO2 and 5.60g of H2O. What is the empirical formula of the unknown compound ?
An unknown compound contains only C, H, and O. Combustion of 8.20 g of this compound...
An unknown compound contains only C, H, and O. Combustion of 8.20 g of this compound produced 16.4 g of CO2 and 6.71 g of H2O. What is the empirical formula of the unknown compound?
An unknown compound contains only C, H, and O. Combustion of 4.20 g of this compound...
An unknown compound contains only C, H, and O. Combustion of 4.20 g of this compound produced 10.3 g of CO2 and 4.20 g of H2O. What is the empirical formula of the unknown compound?
An unknown compound contains only C, H, and O. Combustion of 8.90 g of this compound...
An unknown compound contains only C, H, and O. Combustion of 8.90 g of this compound produced 21.7 g of CO2 and 8.89 g of H2O. What is the empirical formula of the unknown compound?
An unknown compound contains only C, H, and O. Combustion of 8.30 g of this compound...
An unknown compound contains only C, H, and O. Combustion of 8.30 g of this compound produced 19.5 g of CO2 and 5.33 g of H2O. What is the empirical formula of the unknown compound?
An unknown compound contains only C, H, and O. Combustion of 6.80 g of this compound...
An unknown compound contains only C, H, and O. Combustion of 6.80 g of this compound produced 16.6 g of CO2 and 6.80 g of H2O. what is the empirical formula of the unknown compound?
An unknown compound contains only C, H, and O. Combustion of 2.70 g of this compound...
An unknown compound contains only C, H, and O. Combustion of 2.70 g of this compound produced 6.14 g of CO2 and 2.51 g of H2O. What is the empirical formula of the unknown compound? CHO
An unknown compound contains only C, H, and O. Combustion of 6.80 g of this compound...
An unknown compound contains only C, H, and O. Combustion of 6.80 g of this compound produced 16.6 g of CO2 and 6.80 g of H2O. What is the empirical formula of the unknown compound? CHO
A compound is 54.53% C, 9.15% H, and 36.32% O by mass. What is its empirical...
A compound is 54.53% C, 9.15% H, and 36.32% O by mass. What is its empirical formula?