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To solve the problem, we will need to:

1. Write the balanced chemical equation for the reaction of ammonia (\( \text{NH}_3 \)) with oxygen (\( \text{O}_2 \)).
2. Use stoichiometry to relate the mass of oxygen gas to the mass of ammonia consumed.
3. Calculate the mass of ammonia.

### Step 1: Balanced Chemical Equation
The reaction between ammonia and oxygen to produce nitric oxide (\( \text{NO} \)) and water (\( \text{H}_2\text{O} \)) is:

\[
4 \text{NH}_3 + 5 \text{O}_2 \rightarrow 4 \text{NO} + 6 \text{H}_2\text{O}
\]

### Step 2: Stoichiometric Relationship
From the balanced equation, we can see that:
- 4 moles of ammonia (\( \text{NH}_3 \)) react with 5 moles of oxygen (\( \text{O}_2 \)).

### Step 3: Given Data
- Mass of oxygen gas = 9.80 g
- Molar mass of oxygen (\( \text{O}_2 \)) = \( 32.00 \, \text{g/mol} \)
- Molar mass of ammonia (\( \text{NH}_3 \)) = \( 17.03 \, \text{g/mol} \)

### Step 4: Calculation

#### 1. Calculate the number of moles of oxygen gas:

\[
\text{Moles of } O_2 = \frac{9.80 \, \text{g}}{32.00 \, \text{g/mol}}
\]

#### 2. Using the stoichiometric ratio, calculate the moles of ammonia required:

\[
\text{Moles of } \text{NH}_3 = \left( \frac{4}{5} \right) \times \text{Moles of } O_2
\]

#### 3. Convert the moles of ammonia to mass:

\[
\text{Mass of } \text{NH}_3 = \text{Moles of } \text{NH}_3 \times 17.03 \, \text{g/mol}
\]

Let's compute these values.The mass of ammonia (\( \text{NH}_3 \)) consumed by the reaction of 9.80 g of oxygen gas is approximately **4.17 g**, rounded to three significant digits.

Would you like further details on the calculation, or do you have any questions?

Here are some related questions to expand your understanding:

1. What is the significance of balancing a chemical equation in stoichiometry?
2. How does the molar mass of a compound affect its role in chemical reactions?
3. What are some practical applications of the reaction between ammonia and oxygen in industry?
4. How would the mass of ammonia change if more oxygen gas were used in the reaction?
5. How can you use stoichiometry to predict the amounts of all products in a chemical reaction?

**Tip:** Always ensure your chemical equation is balanced before performing stoichiometric calculations to maintain the correct proportion of reactants and products.

What mass of ammonia is consumed by the reaction of 9.80 g of oxygen gas?

Learn how to calculate the mass of ammonia consumed when 9.80 g of oxygen reacts. This problem uses stoichiometry and mass-mole conversions based on the balanced chemical equation for the reaction of NH3 and O2. Suitable for high school students in Grades 10-12.

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