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x moles of potassium dichromate oxidizes...

x moles of potassium dichromate oxidizes 1 mole of ferrous oxalate in acidic medium. Here x is :

A

3

B

1.5

C

0.5

D

1

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The correct Answer is:
To determine how many moles of potassium dichromate (KMnO4) are required to oxidize 1 mole of ferrous oxalate (FeC2O4) in acidic medium, we can follow these steps: ### Step 1: Write the balanced chemical equation The balanced chemical equation for the reaction between potassium dichromate and ferrous oxalate in acidic medium is: \[ 3 \text{KMnO}_4 + 5 \text{FeC}_2\text{O}_4 \rightarrow 3 \text{K}^+ + 3 \text{Mn}^{2+} + 5 \text{Fe}^{3+} + 10 \text{CO}_2 + 12 \text{H}_2\text{O} \] ### Step 2: Identify the mole ratio From the balanced equation, we can see that: - 3 moles of KMnO4 react with 5 moles of FeC2O4. ### Step 3: Calculate the moles of KMnO4 required for 1 mole of FeC2O4 To find out how many moles of KMnO4 are needed for 1 mole of FeC2O4, we can set up a proportion based on the mole ratio: \[ \frac{3 \text{ moles KMnO}_4}{5 \text{ moles FeC}_2\text{O}_4} = \frac{x \text{ moles KMnO}_4}{1 \text{ mole FeC}_2\text{O}_4} \] ### Step 4: Solve for x Cross-multiply to solve for x: \[ x = \frac{3}{5} \text{ moles of KMnO}_4 \] Calculating this gives: \[ x = 0.6 \text{ moles of KMnO}_4 \] ### Conclusion Thus, the value of x, which represents the moles of potassium dichromate required to oxidize 1 mole of ferrous oxalate, is: \[ \boxed{0.6} \] ---
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