Question

Calculate charge in columbs required 1 mole of feo to fe2o3

Answer 1

Answer:

Fe2+ → Fe3+ + e-1

Electricity required for the oxidation of 1 mol of FeO to Fe2O3

= 1 F

= 96487 C

Answer 2

Answer:

Charge required = 96500 C

Explanation:

It is given :

1 mole of FeO to Fe₂O₃

For this oxidation :  Fe²⁺ -----> Fe³⁺

So, 1 mole is required to oxidize it.

Therefore, Charge required  = 1 x 96500 coulomb

or, Charge required = 96500 C

• We know that in one mole of an element the charge present is 96500 C

• As there are 6.023 x 10²³ electrons per mole in an element.

• So, we can get the charge in one mole of electrons present, which is  = (1.6 x 10⁻¹⁶) x (6.023 x 10²³) = 96500 C

• It can also be called as 1 Faraday

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Answer 3

Charge in coulombs required 1 mole of $FeO$ to $Fe2O3$ is calculated as $96500$ coloumbs.

Explanation:

One coulomb is equal to the amount of charge from a current of one ampere flowing for one second

Charge in Coulombs = Current in Amperes × Time in Seconds

1 mole of $FeO$ to $Fe2O3$

here the oxidation of Fe takes place where      $Fe^{2+}$ →$Fe^{3+}$

Oxidation of one mole of $Fe^{2+}$   will require 1×$96500=96500$C.

Electricity required to oxidise 1 moles FeO to Fe2O3

=1F=$96,500C$

=$9.65$×$10^{4}$C

Charge in coulombs required 1 mole of $FeO$ to $Fe2O3$ is calculated as $96500$ coloumbs.

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