`FeS_(2)+O_(2) to `?
The product formed in above reaction is

Options

A. `FeO+SO_(2)`
B. `Fe_(2)O_(3)+SO_(2)`
C. `Fe_(2)O_(3)+SO_(3)`
D. `FeO+SO_(3)`

Answer

To solve the question regarding the reaction of FeS₂ with O₂, we will follow these steps:

### Step 1: Identify the Reactants
The reactants in the reaction are:
- Iron disulfide (FeS₂)
- Oxygen (O₂)

### Step 2: Write the Reaction
The unbalanced reaction can be written as:
\[ \text{FeS}_2 + \text{O}_2 \rightarrow ? \]

### Step 3: Identify the Products
When iron disulfide (FeS₂) reacts with oxygen (O₂), it typically forms:
- Ferric oxide (Fe₂O₃)
- Sulfur dioxide (SO₂)

### Step 4: Balance the Reaction
To balance the reaction, we need to ensure that the number of atoms for each element is the same on both sides. The balanced equation is:
\[ 4 \text{FeS}_2 + 11 \text{O}_2 \rightarrow 2 \text{Fe}_2\text{O}_3 + 8 \text{SO}_2 \]

### Step 5: Identify the Correct Option
From the balanced equation, we can see that the products formed are:
- 2 moles of Fe₂O₃ (ferric oxide)
- 8 moles of SO₂ (sulfur dioxide)

Looking at the options provided:
- Option A: FeO + SO₂
- Option B: Fe₂O₃ + SO₂
- Option C: Fe₂O₃ + SO₃
- Option D: FeO + SO₃

The correct answer is **Option B: Fe₂O₃ + SO₂**.

### Final Answer
The product formed in the reaction of FeS₂ with O₂ is **Fe₂O₃ + SO₂**.

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