How many moles of KMnO4 are needed to oxidise a mixture of 1 mole each of FeSO4 FeC2O4 and fe2 c2o4 completely in each 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. Hence, the correct option is the B option.

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

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

How many moles of oxalic acid are oxidised by 1 mole of KMnO4?

Thus, 0.4 moles of acidified KMnO4 is required to oxidize 1 mole of oxalic acid.

How many moles of KMnO4 are required to oxidizes 5 moles?

Acidified KMnO4 reacts with SO32– ion as follows. 2 moles of KMnO4 produces= 5 (O).

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 mol of each FeSO4 and sec24 in acidic medium?

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

How many moles of K2Cr2O7 is 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 KMnO4 are required?

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.

How many moles are in KMnO4?

So 1 mole. KMnO4 produce= 2.5 (O). Therefore 1 mole of sulphite ion (SO32-) in acid medium requires 2/5 =0.4 mole of KMnO4. Or 1 mole sulphite ion will react with (0.4 x 158)=31.6g of KMnO4.

How many moles of KMnO4 would be required to oxidize a mixture of one mole each of ferrous oxalate ferrous sulphate?

∴35mole of KMnO4 for one mole ferrous oxalate.

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 kmno4 are required in acidic medium?

6 mol of MnO4− in acidic medium.

How many moles of HCl are needed to oxidize 1 mole of KMnO4?

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. For the following reaction: 2KMnO4 + 16 HCl = 2 MnCl2 + 5 Cl2 + 2KCl + 8H2O 8 moles of HCl are needed to react with 1 mole of KMnO4.

How many moles of MnO4 will it take to oxidize 5fec2o4?

So,1 mole of 5FeC2​O4​react with 53​moles of MnO4−​. ∴0.6 moles of MnO4−​are required to oxidise one mole of ferrous sulphate completely in acidic medium. Hence, correct option is (C)

What is the n-factor of KMnO4 and SnCl2?

For KMnO4 n-factor is 5. Let moles be ‘m’. So equivalents of KMnO4 = 5xm = 5m. n-factor for SnCl2 is 2 as it goes from +2 to +4 oxidation state. It’s moles is 1. So equivalents is 2. Hope it helps. All the best. In redox reaction basically at equivalent point multiplication of no.

How do you calculate the equivalent weight of KMnO4 to MnSO4?

KMnO4 ( Mn oxidation state+ VII) gets reduced to MnSO4 (Mn oxidation state+2) i.e. 5 electron change. Thus eqivalent weight is =molar mass /number of electrons transferred i.e.5= 0.2*molar mass Equivalent weight= molar mass/1. Well, we should write the redox equations. Permanganate is (typically) reduced to colourless Mn (+II) ion.