Introduction:
The given question is asking for the number of moles of KMnO4 required to completely oxidize 1 mole of ferrous oxalate in an acidic medium. In order to determine the answer, we need to understand the balanced chemical equation for the reaction between KMnO4 and ferrous oxalate.

Chemical Equation:
The balanced chemical equation for the reaction between KMnO4 and ferrous oxalate in acidic medium can be represented as follows:

5FeC2O4 + KMnO4 + 8H2SO4 → 5FeSO4 + K2SO4 + MnSO4 + 8CO2 + 8H2O

Explanation:
- The balanced equation shows that for every 1 mole of ferrous oxalate (FeC2O4), we need 1 mole of KMnO4 to completely oxidize it.
- However, it is important to note that the question asks for the number of moles of KMnO4 required to completely oxidize 1 mole of ferrous oxalate. Therefore, we need to consider the molar ratio between KMnO4 and ferrous oxalate.
- According to the balanced equation, the molar ratio between KMnO4 and ferrous oxalate is 1:1.
- This means that 1 mole of KMnO4 is required to oxidize 1 mole of ferrous oxalate.
- Since the question specifically asks for the number of moles of KMnO4 required to oxidize 1 mole of ferrous oxalate, the answer is 1 mole of KMnO4.
- However, the answer provided in the question is between '0.5,0.7'. This suggests that there may be additional information or conditions given in the question that could affect the stoichiometry of the reaction or the molar ratio between KMnO4 and ferrous oxalate.
- Without any additional information or conditions, the correct answer would be 1 mole of KMnO4. However, if there are specific conditions or limitations given in the question, they need to be taken into account to determine the correct answer.