Question

balance the reaction Fe2+ +cr2o72- -> Fe3+ +cr3+​

Answer 1

I Think Your Question is incorrect because you write , O 72

Answer 2

The balanced chemical equation in a acidic solution is,

$6Fe^{2+}+Cr_2O_7^{2-}+14H^+\rightarrow 6Fe^{3+}+2Cr^{3+}+7H_2O$

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

Rules for the balanced chemical equation in acidic solution are :

First we have to write into the two half-reactions.

Now balance the main atoms in the reaction.

Now balance the hydrogen and oxygen atoms on both the sides of the reaction.

If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the less number of oxygen are present.

If the hydrogen atoms are not balanced on both the sides then adding hydrogen ion $(H^+)$ at that side where the less number of hydrogen are present.

Now balance the charge.

The given chemical reaction is,

$Fe^{2+}+Cr_2O_7^{2-}\rightarrow Fe^{3+}+Cr^{3+}$

The oxidation-reduction half reaction will be :

Oxidation : $Fe^{2+}\rightarrow Fe^{3+}$

Reduction : $Cr_2O_7^{2-}\rightarrow Cr^{3+}$

First balance the main element in the reaction.

Oxidation : $Fe^{2+}\rightarrow Fe^{3+}$

Reduction : $Cr_2O_7^{2-}\rightarrow 2Cr^{3+}$

Now balance oxygen atom on both side.

Oxidation : $Fe^{2+}\rightarrow Fe^{3+}$

Reduction : $Cr_2O_7^{2-}\rightarrow 2Cr^{3+}+7H_2O$

Now balance hydrogen atom on both side.

Oxidation : $Fe^{2+}\rightarrow Fe^{3+}$

Reduction : $Cr_2O_7^{2-}+14H^+\rightarrow 2Cr^{3+}+7H_2O$

Now balance the charge.

Oxidation : $Fe^{2+}\rightarrow Fe^{3+}+1e^-$

Reduction : $Cr_2O_7^{2-}+14H^++6e^-\rightarrow 2Cr^{3+}+7H_2O$

The charges are not balanced on both side of the reaction. Now we are multiplying oxidation reaction by 6 and then adding both equation, we get the balanced redox reaction.

Oxidation : $6Fe^{2+}\rightarrow 6Fe^{3+}+6e^-$

Reduction : $Cr_2O_7^{2-}+14H^++6e^-\rightarrow 2Cr^{3+}+7H_2O$

The balanced chemical equation in acidic medium will be,

$6Fe^{2+}+Cr_2O_7^{2-}+14H^+\rightarrow 6Fe^{3+}+2Cr^{3+}+7H_2O$

Learn more about : oxidation reduction half reaction

https://brainly.com/question/11118888

https://brainly.com/question/13896138

#learnwithbrainly