The Correct Molar Mass For Nitrous Oxide, N2O Is Given By: A. 44.02 G/Mole B. 30.01 G/Mole C. 60.02 G/Mole 40 D .02 G/Mole E .46.01 G/Mole
The Correct Answer and Explanation is :
The correct molar mass for Nitrous Oxide (N₂O) is A. 44.02 g/mol.
Explanation:
The molar mass of a compound is determined by adding the atomic masses of the elements that make up the compound. In the case of Nitrous Oxide (N₂O), it consists of two nitrogen (N) atoms and one oxygen (O) atom.
- Atomic Mass of Nitrogen (N): The atomic mass of nitrogen is approximately 14.01 g/mol.
- Atomic Mass of Oxygen (O): The atomic mass of oxygen is approximately 16.00 g/mol.
Now, let’s calculate the molar mass of N₂O:
- Since there are two nitrogen atoms, their combined mass is:
[
2 \times 14.01 = 28.02 \, \text{g/mol}
] - The mass of the single oxygen atom is:
[
16.00 \, \text{g/mol}
] - Adding these together gives the molar mass of Nitrous Oxide (N₂O):
[
28.02 \, \text{g/mol} + 16.00 \, \text{g/mol} = 44.02 \, \text{g/mol}
]
Thus, the molar mass of N₂O is 44.02 g/mol, which corresponds to Option A.
Why Other Options are Incorrect:
- Option B (30.01 g/mol): This value would correspond to a compound with a different atomic composition than N₂O.
- Option C (60.02 g/mol): This mass would be too high for N₂O, suggesting a compound with more atoms of nitrogen or oxygen.
- Option D (40.02 g/mol): This value is close, but slightly lower than the actual molar mass of N₂O.
- Option E (46.01 g/mol): This value is slightly higher than the actual molar mass of N₂O, indicating an incorrect atomic combination.
Final Answer:
Therefore, the correct answer is A. 44.02 g/mol.
Now, I will generate an image to visually represent this calculation.
Here is the image showing the calculation of the molar mass of Nitrous Oxide (N₂O). It includes the molecular formula, atomic masses, and a step-by-step breakdown of the calculation, leading to the correct molar mass of 44.02 g/mol.