In the reaction, `2SO_(2) +O_(2) to 2SO_(3)` when 1 mole of `SO_(2)` and 1 mole of `O_(2)` are made to react to completion

Options

A. All the oxygen will be consumed
B. 1.0 role of `SO_(3)` will be produced
C. 0.5 mole of `SO_(2)` is remained
D. All of these

Answer

To solve the problem, we need to analyze the reaction and determine how much of each reactant is consumed and how much product is formed when 1 mole of SO₂ and 1 mole of O₂ react to completion.

### Step-by-Step Solution:

1. **Write the Balanced Chemical Equation:**
The balanced equation for the reaction is:
\[ 2 \text{SO}_2 + \text{O}_2 \rightarrow 2 \text{SO}_3 \]

2. **Identify the Initial Moles of Reactants:**
We start with:
- 1 mole of SO₂
- 1 mole of O₂

3. **Determine the Stoichiometric Ratios:**
According to the balanced equation:
- 2 moles of SO₂ react with 1 mole of O₂.
This means that for every 2 moles of SO₂, 1 mole of O₂ is required.

4. **Calculate the Limiting Reagent:**
To find the limiting reagent, we compare the available moles of each reactant to their stoichiometric coefficients:
- For SO₂: The stoichiometric ratio is 2 (from the equation), so:
\[ \text{Available moles of SO}_2 = 1 \quad \text{(stoichiometric ratio = 2)} \]
\[ \text{Moles required for 1 mole of O}_2 = 2 \times 1 = 2 \]
- For O₂: The stoichiometric ratio is 1, so:
\[ \text{Available moles of O}_2 = 1 \quad \text{(stoichiometric ratio = 1)} \]
\[ \text{Moles required for 1 mole of SO}_2 = 1 \times 1 = 1 \]

Since we only have 1 mole of SO₂ (which requires 0.5 moles of O₂ to react completely), SO₂ is the limiting reagent.

5. **Calculate the Amount of Each Reactant Consumed:**
- Since SO₂ is the limiting reagent, it will be completely consumed:
\[ \text{Moles of SO}_2 consumed = 1 \text{ mole} \]
- The amount of O₂ consumed can be calculated based on the stoichiometry:
\[ \text{Moles of O}_2 consumed = \frac{1 \text{ mole of SO}_2}{2} = 0.5 \text{ moles} \]

6. **Determine Remaining Reactants:**
- Remaining O₂:
\[ \text{Initial moles of O}_2 - \text{Moles of O}_2 consumed = 1 - 0.5 = 0.5 \text{ moles} \]

7. **Calculate the Amount of Product Formed:**
- According to the stoichiometry of the balanced equation, for every 2 moles of SO₂ consumed, 2 moles of SO₃ are produced. Therefore:
\[ \text{Moles of SO}_3 produced = 1 \text{ mole of SO}_2 \times \frac{2 \text{ moles of SO}_3}{2 \text{ moles of SO}_2} = 1 \text{ mole of SO}_3 \]

### Final Results:
- Moles of SO₃ produced: 1 mole
- Moles of O₂ remaining: 0.5 moles
- Moles of SO₂ remaining: 0 moles

### Conclusion:
The correct option based on the analysis is that 1 mole of SO₃ will be produced, and half a mole of O₂ will remain unreacted.