for depolarization of 1 mole of KMnO4, the moles of H2O2 required is_________

5/2 mole of h2o2 is required

To determine the moles of H2O2 required for the depolarization of 1 mole of KMnO4, we need to first determine the balanced equation for the reaction between KMnO4 and H2O2.

The reaction between KMnO4 and H2O2 can be represented by the following balanced equation:

2 KMnO4 + 3 H2O2 → 2 MnO2 + 2 KOH + 3 O2 + 2 H2O

From the balanced equation, we can see that 2 moles of KMnO4 react with 3 moles of H2O2.

So, the moles of H2O2 required for the depolarization of 1 mole of KMnO4 is (3 moles of H2O2 / 2 moles of KMnO4) = 1.5 moles of H2O2.

To determine the moles of H2O2 required for the depolarization of 1 mole of KMnO4, we need to consider the balanced chemical equation for the reaction between these two compounds.

The balanced equation for the depolarization of KMnO4 (potassium permanganate) can be represented as follows:

2 KMnO4 + 3 H2O2 + 2 H2SO4 → 2 MnSO4 + 3 O2 + 5 H2O + K2SO4.

From this equation, we can deduce that it takes 3 moles of H2O2 to depolarize 2 moles of KMnO4.

Therefore, if we want to find out the moles of H2O2 required for the depolarization of 1 mole of KMnO4, we can set up a proportion as follows:

(3 moles H2O2) / (2 moles KMnO4) = x moles H2O2 / (1 mole KMnO4).

By cross-multiplying and solving for x, we can find the value of x, which represents the moles of H2O2 required for the depolarization of 1 mole of KMnO4.

5/2 mole of H2O2 is required.

Here,

2MnO4^- + 5H2O2 —————> 2Mn^(2+)+5H2O+9O2+6e^(-)

Here,
2 moles of KMnO4 is decolourised by 5 moles of H2O2
1 mole of KMnO4 is decolourised by 5/2 moles of H2O2