The neutral Fe atoms gained 3 electrons to become Fe 3+ . [0 + (-3) = +3] The Fe

Question

The neutral Fe atoms gained 3 electrons to become Fe3+. [0 + (-3) = +3]

The Fe3+ ions lost 3 electrons to become neutral Fe. [+3 - (-3) = 0]

The neutral Fe atoms lost 3 electrons to become Fe3+. [0 - (-3) = +3]

The Fe3+ ions gained 3 electrons to become neutral Fe. [+3 + (-3) = 0]

Reduction is the process of gaining electrons. Oxidation is the process of losing electrons. Did Fe3+ undergo reduction or oxidation to become Fe?
The reaction above shows the reduction of an hematite ore (Fe2O3) to iron (Fe). In the half reaction, what does it mean to write the electrons as a reactant?

This is all one question on my homework.

The neutral Fe atoms gained 3 electrons to become Fe3+. [0 + (-3) = +3]

The Fe3+ ions lost 3 electrons to become neutral Fe. [+3 - (-3) = 0]

The neutral Fe atoms lost 3 electrons to become Fe3+. [0 - (-3) = +3]

The Fe3+ ions gained 3 electrons to become neutral Fe. [+3 + (-3) = 0]

Explanation / Answer

Ans d) The Fe3+ ions gained 3 electrons to become neutral . fe [ +3 + (-3) = 0 ]

To balance the reaction , equalise the number of atoms on the left side of the reaction to the ones present on the right .

So the balanced reaction is :

2Fe2O3 + 3C = 4Fe + 3CO2

During this reaction Iron has oxidation state of +3 in Fe2O3 , which reduces to 0 in Fe ( products side ) . hence Fe3+ ions have got reduced to Fe , each gaining three electrons .

The charge on Fe which was +3 earlier has become 0 or neutral in Fe.

Fe3+ has undergone reduction in this reaction , by gaining three electrons and not losing them.

Yes in the reduction half reaction electrons can be shown as the reactants .

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