Chemical Forums

Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Cynonian_raj on August 28, 2019, 03:31:24 PM

Title: Problems in relating ∆G with Galvanic Cell (Electrode Potential)
Post by: Cynonian_raj on August 28, 2019, 03:31:24 PM

For the Reaction Fe^+3 + 3e^- = Fe,   E° is -0.036V and E° for Fe^+3 +e^- = Fe^+2 is 0.771V.
Calculate E° for Fe^+2 +2e^- = Fe.

In solution according to Book,

Let Fe^+2 +2e^- = Fe -----------(1)


Firstly, find ∆G for each equation with given E° and then combine equation (and ∆G also) . After combining equation, we get required equation and ∆G for the required equation and then use simply for ∆G = -nFE
 And we get required E°.

Here my problem is -
1. How do I get equation (1) after combining those equation (Like mathematics)
 How does ot work.
 
2. How we get ∆G for equation (1)  after combining those equation's ∆G.

**Is there any alternate ways for solving this question**

Title: Re: Problems in relating ∆G with Galvanic Cell (Electrode Potential)
Post by: Vidya on August 29, 2019, 12:59:09 AM

Fe⁺³ + 3e^- ---->Fe ---- (2)  -0.036V
Fe⁺³ +e^- -----> Fe⁺² ----(3) 0.771V.
Reverse equation 3 and add it in equation 2 to get equation 1  .As you reverse equation 3 its cell potential value will become negative.
Now add cell potential values to get cell potential for equation 1 
Now ΔG°= nFE°cell
Plug in n = electrons transferred in that reaction
F= 96500C
E°cell  calculated above
you will get ΔG° for equation
Similarly you can calculate ΔG° for equation 2 and 3
When you flip equation3, ΔG° sign will also flipped.
Add two ΔG° values to get ΔG° for equation 1