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To determine the limiting reactant, we need to analyze the reaction and the mole ratio between \( \text{H}_2 \) and \( \text{O}_2 \).

### Reaction:
The chemical reaction between hydrogen gas (\( \text{H}_2 \)) and oxygen gas (\( \text{O}_2 \)) to form water (\( \text{H}_2\text{O} \)) is:
\[
2 \text{H}_2 + \text{O}_2 \rightarrow 2 \text{H}_2\text{O}
\]

### Step-by-Step Solution:
1. **Mole Ratio**: According to the balanced equation, 2 moles of \( \text{H}_2 \) react with 1 mole of \( \text{O}_2 \).
  
2. **Given Quantities**:
   - \( \text{H}_2 \): 3.0 moles
   - \( \text{O}_2 \): 7.0 moles

3. **Determine Limiting Reactant**:
   - For 3.0 moles of \( \text{H}_2 \):
     \[
     \text{Required } \text{O}_2 = \frac{3.0 \, \text{moles } \text{H}_2}{2} = 1.5 \, \text{moles } \text{O}_2
     \]
   - Since we have 7.0 moles of \( \text{O}_2 \), which is more than enough to react with the 3.0 moles of \( \text{H}_2 \), \( \text{H}_2 \) is the **limiting reactant**.

### Answer:
The limiting reactant is \( \text{H}_2 \).

Would you like a more detailed explanation of any part? 

Here are some related questions to consider:
1. What is the excess reactant in this reaction, and how much is left over?
2. How many moles of \( \text{H}_2\text{O} \) would be produced in this reaction?
3. If you started with 5 moles of \( \text{H}_2 \) and 7 moles of \( \text{O}_2 \), what would be the limiting reactant?
4. How does the concept of a limiting reactant apply in industrial chemical processes?
5. How would the reaction differ if it was taking place under non-ideal conditions, such as in a closed container with limited space?

**Tip**: Always compare the mole ratio of reactants based on the balanced equation to find the limiting reactant accurately.

Hydrogen (H2) gas and oxygen (O2) gas react to form water (H2O) vapor. Suppose you have 3.0 mol of H2 and 7.0 mol of O2 in a reactor. What would be the limiting reactant? Enter its chemical formula below.

Learn how to determine the limiting reactant in a reaction between hydrogen (H2) and oxygen (O2) to form water vapor (H2O). This solution covers stoichiometry, mole ratios, and limiting reactants, suitable for high school chemistry students.

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