Consider the following half-reactions and their standard reduction potentials th

Question

Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions.

Mn2+(aq) + 2 e- <=> Mn(s) E° = -1.18 V

Fe3+(aq) + 3 e- <=> Fe(s) E° = -0.036 V

The correct answer is : Mn (s) | Mn 2+(aq, 1.0 M) || Fe3+(aq, 1.0 M) | Fe(s)

I'm not sure how to do it. Thanks in advance for help.

Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions.

Mn2+(aq) + 2 e- <=> Mn(s) E° = -1.18 V

Fe3+(aq) + 3 e- <=> Fe(s) E° = -0.036 V

The correct answer is : Mn (s) | Mn 2+(aq, 1.0 M) || Fe3+(aq, 1.0 M) | Fe(s)

I'm not sure how to do it. Thanks in advance for help.

Explanation / Answer

Quest1:- What is electrochemical cell?

Ans1:- It is a cell in which chemical enery converted into electrical energy by a redox reaction is called electrochemical reaction. In this cell

NOTE:- More negative reductin potential means more reducing power it means it act as a good reducing agent to reduce other element by oxidising itsel.

It means it can easily donate electron. If it is donating electron then definately it will be metal amd oxidise itself and occur at anode.

For the above equations MANGANESE has more negative reduction potential than iron thats why manganese at oxidation and iron electrod present at cathode. In representation oxidation occurs at LHS and reduction represent at RHS. Hence the correct representation given below

Mn(s)|Mn+2(1M) || Fe+3(1.0M) | Fe(s)

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