Question

Combustion of 1.000 g of an organic compound known to contain only carbon, hydrogen, and oxygen produces 2.360 g of carbon dioxide and 0.640 g of water. What is the empirical formula of the compound?

Answer 1

Answer:

The empirical formula is C3H4O

Explanation:

Step 1: Data given

Mass of the compound = 1.000 grams

The compound contains:

- Carbon

- hydrogen

- oxygen

The combustion of this compound gives:

2.360 grams of CO2

0.640 grams of H2O

Step 2: Calculate moles CO2

Moles CO2 = mass CO2 / molar mass CO2

Moles CO2 = 2.360 grams / 44.01 g/mol

Moles CO2 = 0.05362 moles

In CO2 we have 1 mol

This means for 1 mol CO2 we have 1 mol C

For 0.05362 moles CO2 we have 0.05362 moles C

We have 0.05362 moles of C in the compound  

Step 3: Calculate mass of C

Mass C = moles C * molar mass C

Mass C = 0.05362 moles * 12.0 g/mol

Mass C = 0.643 grams  

Step 4: Calculate moles of H2O  

Moles H2O = 0.640 grams / 18.02 g/mol

Moles H2O =  0.0355 moles H2O

For 1 mol H2O we have 2 moles of H

For 0.0355 moles H2O we have 2*0.0355 =  0.071 moles H  

Step 5: Calculate mass of H

Mass H = moles H * molar mass H

Mass H = 0.071 moles * 1.01 g/mol

Mass H = 0.072 grams

Step 6: Calculate mass of O

Mass of O = Mass of compound - mass of C - mass of H

Mass of O = 1.000 g - 0.643 - 0.072 = 0.285 grams

Step 7: Calculate moles of O

Moles O = 0.285 grams / 16.0 g/mol

Moles O = 0.0178 moles

Step 8: Calculate mol ratio

We divide by the smallest amount of moles

C:  0.05362 / 0.0178 = 3

H: 0.071 / 0.0178 = 4

O: 0.0178/0.0178 = 1

The empirical formula is C3H4O

Answer 2

The study of chemicals and bonds is called chemistry.

The correct answer is C3H4O

What is the empirical formula?

• The empirical formula of a chemical compound is the simplest whole-number ratio of atoms present in a compound.

All the data is given in the question, these data is as follows:-

• Mass of the compound = 1.000 grams

The compound contains:

• Carbon
• Hydrogen
• Oxygen

The combustion of this compound gives:

• 2.360 grams of CO2
• 0.640 grams of H2O

The formula to calculate the moles is as follows:-

$Moles CO2 = \frac{mass}{molar mass}$

$Moles \ CO2 = \frac{2.360} {44.01} Moles\ CO2 = 0.05362 moles$

In CO2 we have 1 mole, Which means for 1 mole CO2 we have 1 mole Carbon. For 0.05362 moles CO2, we have 0.05362 moles Carbon, We have 0.05362 moles of C in the compound  

lets calculate the mass of C

Mass C = moles C * molar mass C

Mass C = $0.05362 moles * 12.0 g/mol$

Mass C = 0.643 grams  

The moles of H2O is as follows

Moles H2O = $\frac{0.640}{18.02}$

Moles H2O = 0.0355 moles H2O

For 1 mole H2O, we have 2 moles of H. For 0.0355 moles H2O we have 2*0.0355 =  0.071 moles H  

let's Calculate the mass of H

Mass H = moles H * molar mass H

Mass H = 0.071 moles * 1.01 g/mol

Mass H = 0.072 grams

let's Calculate mass of O

Mass of O = Mass of compound - mass of C - mass of H

Mass of O = 1.000 g - 0.643 - 0.072 = 0.285 grams

let's Calculate moles of O

Moles O = 0.285 grams / 16.0 g/mol

Moles O = 0.0178 moles

The mole ratio is as follows:-

We divide by the smallest amount of moles

C:  0.05362 / 0.0178 = 3

H: 0.071 / 0.0178 = 4

O: 0.0178/0.0178 = 1

Hence, The empirical formula is C3H4O

For more information about the empirical formula, refer to the link:-

https://brainly.com/question/11588623