In coal pyrites `(FeS_(2))` is present as a pollution-causing impurity, which is removed by combustion.
`2FeS_(2) + 5O_(2) rarr 4SO_(2) + 2FeO`.
What volume of `3.0 M KOH` would be required to react with the `SO_(2)` produced in

Options

A. `2.77 L`
B. `5.54 L`
C. `1.38 L`
D. `8.31 L`

Explanation

To solve the problem, we need to follow these steps:

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the combustion of iron pyrites (FeS₂) is given as:
\[ 2 \text{FeS}_2 + 5 \text{O}_2 \rightarrow 4 \text{SO}_2 + 2 \text{FeO} \]

### Step 2: Determine the moles of SO₂ produced
From the balanced equation, we can see that 2 moles of FeS₂ produce 4 moles of SO₂. Therefore, if we assume that 2 moles of FeS₂ are completely combusted, we will produce 4 moles of SO₂.

### Step 3: Relate moles of SO₂ to KOH
The reaction between sulfur dioxide (SO₂) and potassium hydroxide (KOH) can be represented as:
\[ \text{SO}_2 + 2 \text{KOH} \rightarrow \text{K}_2\text{SO}_3 + \text{H}_2\text{O} \]
From this reaction, we can see that 1 mole of SO₂ reacts with 2 moles of KOH.

### Step 4: Calculate the moles of KOH required
If we have 4 moles of SO₂, the moles of KOH required would be:
\[ \text{Moles of KOH} = 2 \times \text{Moles of SO}_2 = 2 \times 4 = 8 \text{ moles of KOH} \]

### Step 5: Use the molarity to find the volume of KOH solution required
The molarity (M) of KOH is given as 3.0 M. We can use the formula:
\[ \text{Moles} = \text{Molarity} \times \text{Volume (L)} \]
Rearranging this gives us:
\[ \text{Volume (L)} = \frac{\text{Moles}}{\text{Molarity}} \]
Substituting in the values we have:
\[ \text{Volume (L)} = \frac{8 \text{ moles}}{3.0 \text{ M}} = \frac{8}{3} \approx 2.67 \text{ L} \]

### Step 6: Conclusion
The volume of 3.0 M KOH required to react with the SO₂ produced is approximately 2.67 liters.

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