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Starting with the standard free energies of formation from the following table, calculate the values of ΔG° and E°cell of the following reactions.  Substance ΔΔG°f (kJ/mol) FeO(s) -255.2 H2(g) 0 Fe(s) 0 H2O(l) -237.2 Pb(s) 0 O2(g) 0 H2SO4(aq) -744.5 PbSO4(s) -813.0   FeO(s)+H2​(g)Fe(s)+H2​O(l)  ΔΔG° =     kJ       FeO(s)+H2​(g)Fe(s)+H2​O(l)  E°cell =     V       2Pb(s)+O2​(g)+2H2​SO4​(aq)2PbSO4​(s)+2H2​O(l)   ΔΔG° =     kJ         Pb(s)+O2​(g)+2H2​SO4​(aq)2PbSO4​(s)+2H2​O(l)   E°cell =     V

Starting with the standard free energies of formation from the following table, calculate the values of ΔG° and E°cell of the following reactions.  Substance ΔΔG°f (kJ/mol) FeO(s) -255.2 H2(g) 0 Fe(s) 0 H2O(l) -237.2 Pb(s) 0 O2(g) 0 H2SO4(aq) -744.5 PbSO4(s) -813.0   FeO(s)+H2​(g)Fe(s)+H2​O(l)  ΔΔG° =     kJ       FeO(s)+H2​(g)Fe(s)+H2​O(l)  E°cell =     V       2Pb(s)+O2​(g)+2H2​SO4​(aq)2PbSO4​(s)+2H2​O(l)   ΔΔG° =     kJ         Pb(s)+O2​(g)+2H2​SO4​(aq)2PbSO4​(s)+2H2​O(l)   E°cell =     V

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section18.4: Entropy Measurement And Values
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Starting with the standard free energies of formation from the following table, calculate the values of ΔG° and E°cell of the following reactions.
 
Substance ΔΔG°f (kJ/mol)
FeO(s) -255.2
H2(g) 0
Fe(s) 0
H2O(l) -237.2
Pb(s) 0
O2(g) 0
H2SO4(aq) -744.5
PbSO4(s) -813.0
 
FeO(s)+H2​(g)Fe(s)+H2​O(l)
 ΔΔG° =     kJ   

 
 
FeO(s)+H2​(g)Fe(s)+H2​O(l)
 E°cell =     V   

 
 
2Pb(s)+O2​(g)+2H2​SO4​(aq)2PbSO4​(s)+2H2​O(l)
  ΔΔG° =     kJ   
 

 

 
Pb(s)+O2​(g)+2H2​SO4​(aq)2PbSO4​(s)+2H2​O(l)
  E°cell =     V   
 
 
 
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