the chemical formula for acetic acid is: calculate the molar mass of acetic acid. round your answer to decimal places.
The Correct Answer and Explanation is :
The chemical formula for acetic acid is ( \text{C}_2\text{H}_4\text{O}_2 ). To calculate the molar mass of acetic acid, we need to sum the molar masses of all the atoms present in the formula.
- Identify the elements and their molar masses:
- Carbon (C): The molar mass of carbon is approximately 12.01 g/mol.
- Hydrogen (H): The molar mass of hydrogen is approximately 1.01 g/mol.
- Oxygen (O): The molar mass of oxygen is approximately 16.00 g/mol.
- Count the number of each type of atom in acetic acid:
- There are 2 carbon atoms.
- There are 4 hydrogen atoms.
- There are 2 oxygen atoms.
- Calculate the total mass for each element:
- Carbon: ( 2 \, \text{C} \times 12.01 \, \text{g/mol} = 24.02 \, \text{g/mol} )
- Hydrogen: ( 4 \, \text{H} \times 1.01 \, \text{g/mol} = 4.04 \, \text{g/mol} )
- Oxygen: ( 2 \, \text{O} \times 16.00 \, \text{g/mol} = 32.00 \, \text{g/mol} )
- Add the total masses together:
[
\text{Total molar mass of acetic acid} = 24.02 \, \text{g/mol} + 4.04 \, \text{g/mol} + 32.00 \, \text{g/mol} = 60.06 \, \text{g/mol}
]
Final Answer:
The molar mass of acetic acid (( \text{C}_2\text{H}_4\text{O}_2 )) is approximately 60.06 g/mol.
Explanation:
The molar mass is a critical property in chemistry that indicates the mass of one mole of a substance. Acetic acid, a simple carboxylic acid, is commonly found in vinegar and has applications in food, chemical synthesis, and biochemistry. Understanding the molar mass helps in stoichiometric calculations, such as determining how much of a reactant is needed for a chemical reaction or the concentration of solutions.
In acetic acid’s case, the ratio of its constituent elements reflects its functional groups: the carboxyl group (–COOH) gives it acidic properties. The calculation process involves using the atomic weights from the periodic table, which is fundamental for various applications in chemistry, including balancing equations and calculating yields in reactions. By rounding to two decimal places, we maintain precision while providing a clear, manageable number for practical use.