Calculate the molar mass of NH
4
NO
3
.
Molar mass of NH
4
NO
3
= __ g/mol.
The Correct Answer and Explanation is :
To calculate the molar mass of ammonium nitrate (NH₄NO₃), we need to determine the molar masses of each element in the compound and then sum them up according to their proportions in the formula.
Step 1: Identify the elements and their quantities
In ammonium nitrate (NH₄NO₃), the elements and their quantities are as follows:
- Nitrogen (N): 2 atoms (1 from NH₄ and 1 from NO₃)
- Hydrogen (H): 4 atoms (from NH₄)
- Oxygen (O): 3 atoms (from NO₃)
Step 2: Find the molar mass of each element
Using the periodic table, we find the molar masses of the elements:
- Nitrogen (N): approximately 14.01 g/mol
- Hydrogen (H): approximately 1.01 g/mol
- Oxygen (O): approximately 16.00 g/mol
Step 3: Calculate the total molar mass
Now, we can calculate the total molar mass of NH₄NO₃ by multiplying the number of atoms by the molar mass of each element:
- For Nitrogen:
[
2 \, \text{N} \times 14.01 \, \text{g/mol} = 28.02 \, \text{g/mol}
] - For Hydrogen:
[
4 \, \text{H} \times 1.01 \, \text{g/mol} = 4.04 \, \text{g/mol}
] - For Oxygen:
[
3 \, \text{O} \times 16.00 \, \text{g/mol} = 48.00 \, \text{g/mol}
]
Step 4: Sum the contributions
Now, we sum all the contributions:
[
\text{Total Molar Mass} = 28.02 \, \text{g/mol} + 4.04 \, \text{g/mol} + 48.00 \, \text{g/mol} = 80.06 \, \text{g/mol}
]
Conclusion
Therefore, the molar mass of ammonium nitrate (NH₄NO₃) is 80.06 g/mol.
Understanding the molar mass is crucial in stoichiometry, which allows chemists to calculate the amounts of reactants and products in chemical reactions. Molar mass plays a key role in converting grams to moles and vice versa, facilitating the quantification of substances involved in chemical processes. This concept is fundamental for various applications in chemistry, including solution preparation, reaction yield predictions, and laboratory measurements.