Apply gibb's free energy equation
Ag+
= 77.11 + (298x73.45)/1000 (Consider T = 298.15K/ 25 C)
= 98.99 kJ mol-1
Ag (s)
Enthaply (del H) for formation of an element is 0
= 0- (298x 42.6)/1000
= -12.69 kJ mol-1
Fe3+
Change in Gibb's free energy for reaction is 0 for spontaneous reaction
Del G = -12.69 - (77.11 - 84.94)
Del G = -12.69 +7.83
Del G = -4.86 kJ/mol
TS = -47.69 -(-4.86) = -- 42.86 KJ
S = -143.7 J/K
A student wishes to determine all the standard thermodynamic parameters for the Ag^+(aq) + Fe^+(aq) =...
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