For the reaction, `X + 2Y rarr Z`
5 moles of X and 9 moles of Y will produce:

Options

A. 5.5 moles of Z
B. 8.5 moles of Z
C. 14.5 moles of Z
D. 4.5 moles of Z

Explanation

To solve the problem, we need to determine how many moles of product \( Z \) can be produced from the given moles of reactants \( X \) and \( Y \) in the reaction:

\[ X + 2Y \rightarrow Z \]

### Step-by-Step Solution:

1. **Identify the Reaction and Given Moles**:
- The balanced chemical equation is:
\[ X + 2Y \rightarrow Z \]
- We are given:
- Moles of \( X = 5 \)
- Moles of \( Y = 9 \)

2. **Determine the Stoichiometric Ratios**:
- From the balanced equation, we can see that:
- 1 mole of \( X \) reacts with 2 moles of \( Y \) to produce 1 mole of \( Z \).

3. **Calculate the Limiting Reagent**:
- To find the limiting reagent, we need to calculate how many moles of \( Z \) can be produced from each reactant.
- From \( X \):
- Moles of \( Z \) produced from \( X = \frac{5 \text{ moles of } X}{1 \text{ mole of } X} = 5 \text{ moles of } Z \)
- From \( Y \):
- Moles of \( Z \) produced from \( Y = \frac{9 \text{ moles of } Y}{2 \text{ moles of } Y} = \frac{9}{2} = 4.5 \text{ moles of } Z \)

4. **Identify the Limiting Reagent**:
- Since \( Y \) produces fewer moles of \( Z \) (4.5 moles) compared to \( X \) (5 moles), \( Y \) is the limiting reagent.

5. **Calculate the Moles of \( Z \) Produced**:
- Since \( Y \) is the limiting reagent and it can produce 4.5 moles of \( Z \), the maximum amount of \( Z \) produced will be:
\[ \text{Moles of } Z = 4.5 \text{ moles} \]

6. **Final Answer**:
- Therefore, the number of moles of \( Z \) produced is **4.5 moles**.