You are given the following three half-reactions: (1) Fe3+(aq) + e−→Fe2+(aq) Eo  = +0.77 V   (2) Fe2+(aq) + 2e−→Fe(s) Eo  = −0.44 V   (3) Fe3+(aq) + 3e−  →  Fe(s)  Part 1 out of 3 (a) CalculateΔGo  for (1) and (2) from their Eo  values. ΔGo  for (1) = ×10 J Enter your answer in scientific notation. ΔGo  for (2) = ×10 J Enter your answer in scientific notation.

Question
Asked Dec 6, 2019
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You are given the following three half-reactions:
 
(1) Fe3+(aq) + e
Fe2+(aq)
 
E
o
 
 
= +0.77 V
     
(2) Fe2+(aq) + 2e
Fe(s)
 
E
o
 
 
= −0.44 V
     
(3) Fe3+(aq) + 3e  
  Fe(s)
   

Part 1 out of 3  
(a) Calculate
Δ
G
o
 
 
for (1) and (2) from their E
o
 
 
values.
 
Δ
G
o
 
 
for (1) =
 
×
10
 
J
 
Enter your answer in scientific notation.
 
Δ
G
o
 
 
for (2) =
 
×
10
 
J
 
Enter your answer in scientific notation.
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Expert Answer

Step 1

Calculation for ΔGo fo...

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Fe+3 (aq) + e → Fe+2 E° = +0.77 V AGº -nFE cell AG° = -1 mol e¯ x 96500 C/mol e x 0.77 V AG° = –7.4 x 104 J

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