Understanding the properties of ethylene glycol is crucial in various chemical and industrial applications. One of the fundamental properties of any chemical compound is its molar mass, which is the mass of one mole of that substance. Ethylene glycol, with the chemical formula C2H6O2, is a significant compound due to its wide range of uses, including as an antifreeze in vehicles, in the production of polyester fibers, and in the manufacturing of resins. To calculate the molar mass of ethylene glycol, we must sum the atomic masses of all the atoms in one molecule of the compound.
Key Points
- The chemical formula for ethylene glycol is C2H6O2.
- The atomic masses (rounded to the nearest whole number for simplicity) are approximately: Carbon (C) = 12 g/mol, Hydrogen (H) = 1 g/mol, and Oxygen (O) = 16 g/mol.
- The molar mass of ethylene glycol can be calculated by summing the atomic masses of all atoms in the molecule.
- Understanding the molar mass of ethylene glycol is essential for calculating the amounts of reactants and products in chemical reactions.
- Ethylene glycol's properties, including its molar mass, make it a versatile compound in various industries.
Calculation of Molar Mass
To calculate the molar mass of ethylene glycol, we follow a straightforward process. Given the chemical formula C2H6O2, we have 2 carbon atoms, 6 hydrogen atoms, and 2 oxygen atoms. The atomic masses are: Carbon © = 12.01 g/mol, Hydrogen (H) = 1.008 g/mol, and Oxygen (O) = 16.00 g/mol. Plugging these values into our calculation gives us: (2 * 12.01) + (6 * 1.008) + (2 * 16.00).
Performing the Calculation
Now, let’s perform the calculation step by step:
- For Carbon: 2 * 12.01 = 24.02 g/mol
- For Hydrogen: 6 * 1.008 = 6.048 g/mol
- For Oxygen: 2 * 16.00 = 32.00 g/mol
Summing these values: 24.02 + 6.048 + 32.00 = 62.068 g/mol. Therefore, the molar mass of ethylene glycol is approximately 62.07 g/mol when rounded to the nearest hundredth.
| Element | Atomic Mass (g/mol) | Number of Atoms | Total Mass Contribution (g/mol) |
|---|---|---|---|
| Carbon (C) | 12.01 | 2 | 24.02 |
| Hydrogen (H) | 1.008 | 6 | 6.048 |
| Oxygen (O) | 16.00 | 2 | 32.00 |
| Total | - | - | 62.068 |
Practical Applications and Considerations
The molar mass of ethylene glycol is not just a theoretical concept; it has significant practical implications. For instance, in the production of polyester fibers, knowing the exact amount of ethylene glycol required per mole of terephthalic acid (another reactant) is crucial for optimizing the reaction conditions and yields. Similarly, in the use of ethylene glycol as an antifreeze, its molar mass is relevant for calculating the concentration of solutions and ensuring the proper protection of engines against freezing temperatures.
Industry-Specific Uses
In the automotive industry, ethylene glycol’s use as an antifreeze is widespread. The molar mass of ethylene glycol helps in formulating antifreeze solutions that meet specific standards for freezing point depression and boiling point elevation. In the textile industry, the molar mass is critical for the synthesis of polyester, where the stoichiometric ratio of reactants must be precisely controlled to achieve the desired fiber properties.
In conclusion, the molar mass of ethylene glycol, calculated to be approximately 62.07 g/mol, is a foundational piece of information that underpins its various applications across different industries. Understanding this property is essential for the efficient, safe, and effective use of ethylene glycol in chemical reactions, industrial processes, and everyday products.
What is the chemical formula of ethylene glycol?
+The chemical formula for ethylene glycol is C2H6O2.
How is the molar mass of ethylene glycol calculated?
+The molar mass of ethylene glycol is calculated by summing the atomic masses of all the atoms in one molecule of the compound, which includes 2 carbon atoms, 6 hydrogen atoms, and 2 oxygen atoms.
What are some practical applications of ethylene glycol where its molar mass is relevant?
+Ethylene glycol’s molar mass is relevant in its use as an antifreeze in vehicles, in the production of polyester fibers, and in the manufacturing of resins, among other applications.
