the number of moles of H2O2 required to completely react with 400ml of 0.5N KMnO4 in acidic medium are

According to the law of gram equivalents, the reacting portions of the reactants always have equal gram equivalents (Geq). Therefore,

Geq of KMnO4 = Normality × Volume
= 0.5 × 400/1000
= 0.2

Geq of H2O2 = No. of moles (x) × n factor
= 2x

∴ 2x = 0.2
x = 0.1

Kuch nahi

To find the number of moles of H2O2 required to react with 400 ml of 0.5N KMnO4 in an acidic medium, we need to determine the balanced chemical equation for the reaction between H2O2 and KMnO4.

The balanced equation for this reaction is as follows:

2KMnO4 + 5H2O2 + 6H+ -> 2Mn2+ + 5O2 + 2K+ + 8H2O

From the balanced equation, we can see that it takes 5 moles of H2O2 to react with 2 moles of KMnO4.

To calculate the number of moles of KMnO4 in 400 ml of 0.5N solution, we can use the formula:

moles = volume (in liters) x Normality

First, we need to convert the volume from milliliters to liters:

volume = 400 ml = 400/1000 = 0.4 liters

Next, we can calculate the number of moles of KMnO4:

moles of KMnO4 = 0.4 liters x 0.5N = 0.2 moles

Since the mole ratio between H2O2 and KMnO4 is 5:2, we can calculate the number of moles of H2O2 required:

moles of H2O2 required = (0.2 moles of KMnO4) x (5/2) = 0.5 moles

Therefore, the number of moles of H2O2 required to completely react with 400 ml of 0.5N KMnO4 in an acidic medium is 0.5 moles.

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