What is the molar mass of N2O4? What is the equality and write 2 conversion factors
The Correct Answer and Explanation is:
Molar Mass of N₂O₄ (Dinitrogen Tetroxide):
To find the molar mass of N₂O₄, we sum the molar masses of all atoms in the molecule:
- Nitrogen (N) = 14.01 g/mol × 2 = 28.02 g/mol
- Oxygen (O) = 16.00 g/mol × 4 = 64.00 g/mol
Total Molar Mass = 28.02 g/mol + 64.00 g/mol = 92.02 g/mol
Equality Statement:
1 mole of N₂O₄ = 92.02 grams of N₂O₄
Two Conversion Factors:
- 1 mol N₂O₄92.02 g N₂O₄\frac{1\ \text{mol N₂O₄}}{92.02\ \text{g N₂O₄}}
- 92.02 g N₂O₄1 mol N₂O₄\frac{92.02\ \text{g N₂O₄}}{1\ \text{mol N₂O₄}}
Explanation
Understanding the molar mass of a compound like N₂O₄ is a foundational concept in chemistry that connects the atomic scale to the macroscopic world. The molar mass tells us how much one mole of a substance weighs in grams. In the case of dinitrogen tetroxide (N₂O₄), the molecule contains two nitrogen atoms and four oxygen atoms. By consulting the periodic table, we find that nitrogen has an atomic mass of approximately 14.01 g/mol and oxygen has an atomic mass of about 16.00 g/mol. Thus, the total molar mass of N₂O₄ is 92.02 g/mol.
This means that if you have one mole (6.022 × 10²³ molecules) of N₂O₄, it would weigh 92.02 grams. This relationship is essential when converting between the mass of a substance and the number of moles, which is often required in stoichiometry, chemical reactions, and laboratory calculations.
The equality statement, 1 mol N₂O₄ = 92.02 g N₂O₄, gives rise to two useful conversion factors. These allow you to convert grams of N₂O₄ to moles and vice versa. For example, if you have 184.04 grams of N₂O₄, you can calculate the number of moles by multiplying by the conversion factor 1 mol92.02 g\frac{1\ \text{mol}}{92.02\ \text{g}}, giving you 2.00 moles.
These conversions are crucial in determining how much of a reactant is needed or how much product will be formed in a chemical reaction. Mastery of molar mass and these conversion principles enables chemists to precisely measure and predict chemical quantities in both academic and real-world applications.
