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N-factor for the following reaction is ...

N-factor for the following reaction is
`FeS_(2)toFe_(2)O_(3)+SO_(2)`

A

8

B

9

C

10

D

11

Text Solution

AI Generated Solution

The correct Answer is:
To find the n-factor for the reaction \( \text{FeS}_2 \rightarrow \text{Fe}_2\text{O}_3 + \text{SO}_2 \), we need to determine the change in oxidation states of the elements involved in the reaction. Here’s a step-by-step solution: ### Step 1: Identify the oxidation states of the reactants and products. - In \( \text{FeS}_2 \): - Iron (Fe) has an oxidation state of \( +2 \) (since it is bonded to two sulfurs). - Sulfur (S) has an oxidation state of \( -1 \). - In \( \text{Fe}_2\text{O}_3 \): - Iron (Fe) has an oxidation state of \( +3 \). - Oxygen (O) has an oxidation state of \( -2 \). - In \( \text{SO}_2 \): - Sulfur (S) has an oxidation state of \( +4 \). - Oxygen (O) has an oxidation state of \( -2 \). ### Step 2: Calculate the change in oxidation states for Iron. - For Iron: - Change from \( +2 \) (in \( \text{FeS}_2 \)) to \( +3 \) (in \( \text{Fe}_2\text{O}_3 \)). - The change in oxidation state is \( +3 - (+2) = +1 \). ### Step 3: Calculate the change in oxidation states for Sulfur. - For Sulfur: - Change from \( -1 \) (in \( \text{FeS}_2 \)) to \( +4 \) (in \( \text{SO}_2 \)). - The change in oxidation state is \( +4 - (-1) = +5 \). ### Step 4: Consider the number of atoms involved. - In the reaction, we have: - 2 Iron atoms in \( \text{Fe}_2\text{O}_3 \) contributing to the total change. - 2 Sulfur atoms in \( \text{FeS}_2 \) contributing to the total change. ### Step 5: Calculate the total n-factor. - For Iron: - Since there are 2 Iron atoms, the total change for Iron is \( 2 \times 1 = 2 \). - For Sulfur: - Since there are 2 Sulfur atoms, the total change for Sulfur is \( 2 \times 5 = 10 \). ### Step 6: Add the contributions to find the overall n-factor. - Total n-factor = Change from Iron + Change from Sulfur - Total n-factor = \( 2 + 10 = 12 \). ### Conclusion The n-factor for the reaction \( \text{FeS}_2 \rightarrow \text{Fe}_2\text{O}_3 + \text{SO}_2 \) is **12**. ---

To find the n-factor for the reaction \( \text{FeS}_2 \rightarrow \text{Fe}_2\text{O}_3 + \text{SO}_2 \), we need to determine the change in oxidation states of the elements involved in the reaction. Here’s a step-by-step solution: ### Step 1: Identify the oxidation states of the reactants and products. - In \( \text{FeS}_2 \): - Iron (Fe) has an oxidation state of \( +2 \) (since it is bonded to two sulfurs). - Sulfur (S) has an oxidation state of \( -1 \). ...
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