What is the volume of 17 g of `NH_(3)` gas at STP?

Answer

To find the volume of 17 g of ammonia (NH₃) gas at standard temperature and pressure (STP), we can follow these steps:

### Step 1: Determine the molar mass of ammonia (NH₃).
- The molar mass of ammonia is calculated as follows:
- Nitrogen (N) has an atomic mass of 14 g/mol.
- Hydrogen (H) has an atomic mass of 1 g/mol, and since there are three hydrogen atoms in ammonia, we multiply by 3.

\[ \text{Molar mass of NH}_3 = 14 \, \text{g/mol} + (3 \times 1 \, \text{g/mol}) = 14 \, \text{g/mol} + 3 \, \text{g/mol} = 17 \, \text{g/mol} \]

### Step 2: Calculate the number of moles of ammonia in 17 g.
- To find the number of moles, we use the formula:

\[ \text{Number of moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \]

Substituting the values:

\[ \text{Number of moles} = \frac{17 \, \text{g}}{17 \, \text{g/mol}} = 1 \, \text{mol} \]

### Step 3: Use the volume of 1 mole of gas at STP.
- At STP, 1 mole of any ideal gas occupies 22.4 liters.

### Step 4: Calculate the volume occupied by 17 g of NH₃.
- Since we have 1 mole of NH₃, the volume occupied is:

\[ \text{Volume} = 1 \, \text{mol} \times 22.4 \, \text{L/mol} = 22.4 \, \text{L} \]

### Final Answer:
The volume of 17 g of NH₃ gas at STP is **22.4 liters**.

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