How many moles of K2Cr2O7 is required to oxidise?

How many moles of K2Cr2O7 are required to oxidise?

That is, each mole of K2Cr2O7 oxidises 2 moles of ferrous sulphate. Hence, to oxidize 2 moles of FeSO4, only 1 mole of K2Cr2O7 is required.

How many moles of K2Cr2O7 are required to oxidize 1mole of ferric oxalate?

Explanation: The following equations are essential in the answering of the question. In Acidic medium. We therefore need 0.5moles to oxidize one mole of ferrous oxalate.

How many moles of K2Cr2O7 can be reduced by 1 mole of Sn+?

It is clear form this equation that 3 moles of Sn2+ reduce one mole of Cr2O2-7, hence 1 mol.

How many no of moles of KMnO4 are required to oxidise?

KMnO4 is at its maximum oxidation state and cannot be further oxidized. If you mean how many moles are needed to react with KMnO4 when it is used as on oxidizing agent, then it depends on the reaction. 8 moles of HCl are needed to react with 1 mole of KMnO4.

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How many moles are in potassium chlorate?

The answer is 122.5495. We assume you are converting between grams Potassium Chlorate and mole. You can view more details on each measurement unit: molecular weight of Potassium Chlorate or mol The molecular formula for Potassium Chlorate is KClO3. The SI base unit for amount of substance is the mole.

How many moles of KMnO4 are required in acidic medium?

6 mol of MnO4− in acidic medium.

How many moles of ferrous ion are needed for its complete oxidation by one mole of kmno4 in acidic medium?

Thus it can be inferred that 0.6 moles of is required to oxidize one mole of in acidic medium.

How many moles of mno4 ions are required?

Number of moles of MnO4 required to oxidies one mole of ferrous oxalate completely in acidic medium will be. 0.6 mole.

What is the formula of ferric oxalate?

6 mol of MnO4−​ in acidic medium.

How many moles of KMnO4 are required to oxidise ferric?

Thus, 6 moles of KMnO₄ are required in acidic medium to oxidise 10 moles of ferric oxalate.

How many moles of KMnO4 are needed to oxidise a mixture of 1 mole of each FeSO4 & FeC2O4 in acidic medium?

Therefore, 2 moles of permanganate will be needed to oxidize one mole of $Fe{{C}_{2}}{{O}_{4}}$ , $F{{e}_{2}}{{({{C}_{2}}{{O}_{4}})}_{3}}$, $FeS{{O}_{4}}$ and $F{{e}_{2}}{{(S{{O}_{4}})}_{3}}$ in acidic medium.