Question

E value for mn3+/mn2+ couple is much more positive than that for fe3+/fe2+

Answer 1

Answer:

Step-by-step explanation:

We want to prove that the value for mn3+/mn2+ couple is much more positive than that for fe3+/fe2+.

We know that for a reaction, del G is the same as -nFE.

Let n be the number of electrons involved.

Let F be the constant of Faraday.

Let E be the electrode potential.

In order to have a feasible reaction, thermo dynamically del G needs to be less than 0.

Thus, E >0.

If we have more thermo dynamically feasible the reaction is then we also have more electrode potential

$Mn^{3} +---- > Mn^{2}$+

Then:

$Mn^{3} + = 3d^{4}4s^{0}$

$Mn^{2} + = 3d^{5}4s^{0}$

Hence, we can conclude that this reaction is better than:

$Cr^{3} +---- > Cr^{2}$+

Now:

$Cr^{3} + = 3d^{3}4s^{0}$

$Cr^{2} + = 3d^{4}4s^{0}$

As we know that reactant is better the reaction is unfavorable, E < 0.

Thus:

$Fe^{3} +---- > Fe^{2}$+

Now:

$Fe^{3} + = 3d^{5}4s^{0}$

$Fe^{2} + = 3d^{6}4s^{0}$

As we know that the reactant is better then reaction is not favorable.

Then E < 0.

Thus, the first reaction E will be greater than the others.

Answer 2

Answer:

Step-by-step explanatio

We know that for a reaction, del G is the same as -nFE.

Let n be the number of electrons involved.

Let F be the constant of Faraday.

Let E be the electrode potential.

In order to have a feasible reaction, thermo dynamically del G needs to be less than 0.

Thus, E >0.

If we have more thermo dynamically feasible the reaction is then we also have more electrode potential

+

Then:

Hence, we can conclude that this reaction is better than:

+

Now:

As we know that reactant is better the reaction is unfavorable, E < 0.

Thus:

+

Now:

As we know that the reactant is better then reaction is not favorable.

Then E < 0.

Thus, the first reaction E will be greater than the others.

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