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To solve the problem, we need to use the balanced chemical equation for the reaction between hydrogen gas and nitrogen gas to form ammonia:

\[
3H_2 + N_2 \rightarrow 2NH_3
\]

This tells us that 3 volumes of hydrogen gas react with 1 volume of nitrogen gas to produce 2 volumes of ammonia gas.

### Given:
- **Volume of hydrogen (\(H_2\)) consumed**: \(1.7 \, \text{cm}^3\)

### Find:
- **Volume of ammonia (\(NH_3\)) produced**

### Solution:
1. **Determine the mole ratio** from the balanced equation:
   \[
   \frac{2 \text{ mol NH}_3}{3 \text{ mol H}_2}
   \]
   This means that for every 3 parts (volumes) of \(H_2\) gas, 2 parts (volumes) of \(NH_3\) gas are produced.

2. **Calculate the volume of \(NH_3\) produced** using the given volume of \(H_2\):
   \[
   \text{Volume of } NH_3 = \text{Volume of } H_2 \times \frac{2}{3}
   \]
   Substituting the given values:
   \[
   \text{Volume of } NH_3 = 1.7 \, \text{cm}^3 \times \frac{2}{3}
   \]

3. **Perform the calculation**:
   \[
   \text{Volume of } NH_3 = 1.13 \, \text{cm}^3
   \]

### Answer:
The volume of ammonia produced is approximately \(1.1 \, \text{cm}^3\) (rounded to 2 significant digits).

Would you like further details or have any additional questions?

**Related Questions:**
1. What is the mass of \(NH_3\) produced if the volume is \(1.1 \, \text{cm}^3\) and the density is \(0.73 \, \text{g/cm}^3\)?
2. How many moles of \(H_2\) were consumed in the reaction if the volume is \(1.7 \, \text{cm}^3\) at STP?
3. What volume of \(N_2\) gas is required to react completely with \(1.7 \, \text{cm}^3\) of \(H_2\)?
4. How does the reaction change if the pressure or temperature is altered?
5. What is the significance of using a balanced chemical equation in determining product volumes?

**Tip:** Always ensure the chemical equation is balanced before performing any stoichiometric calculations.

Hydrogen gas and nitrogen gas react to form ammonia gas. What volume of ammonia would be produced by this reaction if 1.7 cm^3 of hydrogen were consumed?

Learn how to calculate the volume of ammonia produced when 1.7 cm^3 of hydrogen gas is consumed in a reaction with nitrogen gas. This problem involves stoichiometry and gas volume ratios, ideal for high school chemistry students.

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