One Integer Value Correct TypeDirection (Q. Nos. 20-23) This section contains 4 questions. When worked out will result in an integer from 0 to 9 (both inclusiveQ.The number of moles of FeC2O4 that reduces two moles of KMnO4 in acidic medium areCorrect answer is between '3.3,3.4'. Can you explain this answer?

Question

Answer

5 is the answer

Answer

To determine the number of moles of FeC2O4 that reduces two moles of KMnO4 in acidic medium, we need to use the balanced chemical equation for the reaction between FeC2O4 and KMnO4.

The balanced equation is as follows:
5FeC2O4 + 2KMnO4 + 8H2SO4 → 10CO2 + 2MnSO4 + 5FeSO4 + 8H2O + K2SO4 + 10H2O

From the balanced equation, we can see that 5 moles of FeC2O4 are required to react with 2 moles of KMnO4.

Now, let's calculate the number of moles of FeC2O4 required to react with 2 moles of KMnO4.

Moles of FeC2O4 = (Moles of KMnO4) x (Molar ratio of FeC2O4 to KMnO4)

Moles of KMnO4 = 2 moles (given)

Molar ratio of FeC2O4 to KMnO4 = 5:2

Substituting the values into the formula, we get:

Moles of FeC2O4 = 2 moles x (5/2) = 5 moles

So, the number of moles of FeC2O4 that reduces two moles of KMnO4 in acidic medium is 5 moles.

However, the correct answer is given as between 3.3 and 3.4. This suggests that there is a different stoichiometry involved in the reaction. It is possible that the reaction is not stoichiometrically balanced or that there are additional factors affecting the reaction.

Without further information or clarification, it is difficult to determine the exact number of moles of FeC2O4 that reduces two moles of KMnO4 in acidic medium.

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