10 moles of `SO_(2)` and 4 moles of `O_(2)` are mixed in a closed vessel of volume 2 litres. The mixture is heated in the presence of Pt catalyst. Following reaction takes place:
`2SO_(2)(g)+O_(2)(g)to2SO_(3)(g)`
Number of moles of `SO_(3)` formed in the reaction will be

Options

A. 10
B. 4
C. 8
D. 14

Answer

To solve the problem, we need to determine how many moles of `SO3` are formed when `10 moles` of `SO2` and `4 moles` of `O2` react according to the equation:

\[ 2SO2(g) + O2(g) \rightarrow 2SO3(g) \]

### Step-by-Step Solution:

1. **Identify the Reaction Stoichiometry**:
The balanced chemical equation shows that:
- 2 moles of `SO2` react with 1 mole of `O2` to produce 2 moles of `SO3`.

2. **Calculate the Required Moles of Reactants**:
From the stoichiometry of the reaction:
- For every 2 moles of `SO2`, 1 mole of `O2` is required.
- Therefore, for `10 moles` of `SO2`, the moles of `O2` required can be calculated as:
\[ \text{Required } O2 = \frac{10 \text{ moles } SO2}{2} = 5 \text{ moles } O2 \]

3. **Determine the Limiting Reagent**:
We have `4 moles` of `O2` available, but we need `5 moles` to completely react with `10 moles` of `SO2`. Therefore, `O2` is the limiting reagent.

4. **Calculate the Moles of `SO3` Formed**:
According to the reaction, `1 mole` of `O2` produces `2 moles` of `SO3`. Since we have `4 moles` of `O2`, we can calculate the moles of `SO3` formed as follows:
\[ \text{Moles of } SO3 = 2 \times \text{Moles of } O2 = 2 \times 4 = 8 \text{ moles } SO3 \]

5. **Conclusion**:
The number of moles of `SO3` formed in the reaction is `8 moles`.

### Final Answer:
The number of moles of `SO3` formed in the reaction will be **8 moles**.

---