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93×105C.

## How many coulombs of electricity are required for the oxidation of 1 mole of h2o to?

The electric charge required to oxidise 1 mole of [{{text{H}}_{text{2}}}{text{O}}] to [{text{O}}]is 193000 Coulomb. Thus, the correct option is (B).

## How much electricity is required in Coulomb for the oxidation of 1 mole?

The charge required is 1 F. So, the amount of charge required is 96500 C.

## How many coulombs of electricity are required for the oxidation?

93×105C.

## How many coulombs of electricity are required for the reduction of 1 mole of mno4 − 1 to Mn 2?

5. 62×105C.

## How many coulombs are required for the reduction of 1 mole of cu2+ to CU?

How much charge is required for the reduction of 1 mole of Cu^(2+) to Cu. =2×96500=193000C.

## How many coulombs are required for the oxidation of 1 mole of h2 o2 co2?

3×102C.

## What is the value of quantity of electricity for 1 Faraday?

That is 96500 coulombs per mole. So 96500 coulombs is called 1 faraday. Notice the small “f” when it is used as a unit. Whenever you have an equation in which you have 1 mole of electrons, that is represented in an electrical circuit by 1 faraday of electricity – in other words, by 96500 coulombs.

## How many coulombs of electricity are required for reduction of 1 mole of cr2o7?

1×96500 C.

## How many coulombs of electricity are required for the oxidation of 1 mole of mno4?

9. 65×106C.

## How many Faraday of electricity is required to reduce 1 mole of mno4 minus ions to Mn 2 ions?

Hence , 5 faraday will be needed for the reduction of 1 mole of MnO_{4}^{–} .

## How many electrons are required for the reduction of 1 mole of mno4?

Therefore, 5 mol of electrons are required to reduce 1 mol of MnO-4 ions).