What is the value of `E^(@)` cell in the following reaction? `Cr|Cr^(3+) (0.1 M)||Fe^(2+) (0.01 M)|Fe` Given, `E_(Cr^(3+)//Cr)^(@)=-0.74 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V`A. `+ 0.2606 V`B. `0.5212 V`C. `+ 01303 V`D. `-0.2606 V`

What is the value of `E^(@)` cell in the following reaction? `Cr|Cr^(3

1.	What is the value of `E^(@)` cell in the following reaction? `Cr\|Cr^(3+) (0.1 M)\|\|Fe^(2+) (0.01 M)\|Fe` Given, `E_(Cr^(3+)//Cr)^(@)=-0.74 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V`A. `+ 0.2606 V`B. `0.5212 V`C. `+ 01303 V`D. `-0.2606 V`
Answer» Correct Answer - A The cell reaction is `2Cr+3Fe^(2+) rarr 2Cr^(3+)+3Fe(n=6)` from Nernst equation, `E_("cell")=E_("cell")^(@)-0.059/n "log" ([Cr^(3+)]^(2))/([Fe^(2+)]^(3))` `=[-0.44+0.74]- 0.059/6 xx"log" ((0.1)^(2))/((0.01)^(3))` `=+0.2606 V`

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What is the value of `E^(@)` cell in the following reaction? `Cr|Cr^(3+) (0.1 M)||Fe^(2+) (0.01 M)|Fe` Given, `E_(Cr^(3+)//Cr)^(@)=-0.74 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V`A. `+ 0.2606 V`B. `0.5212 V`C. `+ 01303 V`D. `-0.2606 V`

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