What is the molar mass of NH4NO3?
Understand the Problem
The question is asking for the calculation of the molar mass of the compound ammonium nitrate (NH4NO3). To solve this, we will sum the atomic masses of all the atoms present in the formula.
Answer
$80.06 \, \text{g/mol}$
Answer for screen readers
The molar mass of ammonium nitrate (NH₄NO₃) is approximately $80.06 , \text{g/mol}$.
Steps to Solve
- Identify the atoms in ammonium nitrate
The formula for ammonium nitrate is $NH_4NO_3$, which consists of
- Nitrogen (N)
- Hydrogen (H)
- Oxygen (O)
- Count the number of each atom
In the formula $NH_4NO_3$, we have:
- 2 Nitrogen atoms
- 4 Hydrogen atoms
- 3 Oxygen atoms
- Find the atomic masses of each element
Using common atomic masses:
- Nitrogen (N): approximately 14.01 g/mol
- Hydrogen (H): approximately 1.01 g/mol
- Oxygen (O): approximately 16.00 g/mol
- Calculate the total mass for each element
Multiply the number of each atom by its atomic mass:
- For Nitrogen: $$ 2 \times 14.01 = 28.02 , \text{g/mol} $$
- For Hydrogen: $$ 4 \times 1.01 = 4.04 , \text{g/mol} $$
- For Oxygen: $$ 3 \times 16.00 = 48.00 , \text{g/mol} $$
- Sum the total masses
Now, add these total masses together to find the molar mass of $NH_4NO_3$: $$ 28.02 + 4.04 + 48.00 = 80.06 , \text{g/mol} $$
The molar mass of ammonium nitrate (NH₄NO₃) is approximately $80.06 , \text{g/mol}$.
More Information
Molar mass is an important concept in chemistry that helps in stoichiometric calculations. Ammonium nitrate is commonly used in fertilizers and explosives.
Tips
- Forgetting to count the correct number of atoms in the formula.
- Using incorrect atomic masses for the elements.
