For the reaction `A + 2B to C,`5moles of A and 8moles of B will produce :-

Options

A. 5 moles of C
B. 4 moles of C
C. 8 moles of C
D. 13 moles of C

Explanation

To solve the problem of how many moles of C will be produced from the reaction \( A + 2B \rightarrow C \) with 5 moles of A and 8 moles of B, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Stoichiometry of the Reaction**:
The balanced chemical equation shows that 1 mole of A reacts with 2 moles of B to produce 1 mole of C.

2. **Determine the Required Moles of B for the Given Moles of A**:
Since we have 5 moles of A, we need to calculate how many moles of B are required:
\[ \text{Required moles of B} = 5 \text{ moles of A} \times 2 \text{ moles of B/mole of A} = 10 \text{ moles of B} \]

3. **Compare Available Moles of B with Required Moles**:
We have 8 moles of B available, but we need 10 moles to fully react with 5 moles of A. Therefore, B is the limiting reagent.

4. **Calculate the Amount of C Produced**:
According to the stoichiometry of the reaction, 2 moles of B produce 1 mole of C. We can find out how many moles of C can be produced from the available moles of B:
\[ \text{Moles of C produced} = \frac{8 \text{ moles of B}}{2 \text{ moles of B/mole of C}} = 4 \text{ moles of C} \]

5. **Conclusion**:
Therefore, when 5 moles of A and 8 moles of B react, they will produce **4 moles of C**.

### Final Answer:
**4 moles of C**

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