Calculate ΔG0 for the following reactions at 25oC.
(a) N2(g) + O2(g) → 2NO(g)
ΔG0 = kJ/mol
(b) H2O(l) → H2O(g)
ΔG0 = kJ/mol
(c) 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l)
ΔG0 = kJ/mol
ΔG0 rxn=n Gfo (products)-mGfo (products)
Gfo-std gibbs energy of formation
n,m=coefficients of reactants
Gfo (N2)=0
Gfo (O2)=0
Gfo (NO)=87.6 KJ/mol
ΔG0 rxn=2*87.6 KJ/mol-0=175.2kj/mol
b) Gfo (H2O L)=-237.14 KJ/MOL
Gfo (H2O GAS)=0
ΔG0 rxn=0--237.14 KJ/MOL=-237.14 KJ/MOL
C)Gfo (C2H2))=209 KJ/mol
Gfo (o2)=0
Gfo (CO2)=-394.39kj/mol
Gfo (H2O L)=-237.14 KJ/MOL
G 0 rxn=[4*(-394.39)+2*(-237.14)]-[2*209+0]=-2051.84-418=-2469.84 kj/mol
Calculate ΔG0 for the following reactions at 25oC. (a) N2(g) + O2(g) → 2NO(g) ΔG0 =...
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