For the elementary gas-phase reaction O3 + NO NO2 + O2, one finds that Ea = 2.5 kcal/mole and A = 6 X 108 dm3mol-1s-1 for the temperature range 220 – 320 K. Calculate ΔG0c‡, ΔHoc‡, and ΔSoc‡ for the midpoint of this temperature range.
Ea = 2.5 KCal / mol
Ea = 2.5 x 4.184 kJ/mol
Ea = 10.46 kJ/mol
we know that
according to arhenius equaiton
k = Ae^-(Ea/RT)
so
using given values
k = 6 x 10^8 x e^(-10.46 x 1000 / 8.314 x 270)
k = 5.68 x 10^6
now
we know that
dGo = -RT ln k
so
dGo = -8.314 x 270 x ln 5.68 x 10^6
dGo = -34912 J/mol
dGo = -34.912 kJ /mol
now
Ea = dHo + RT
so
10.46 x 1000 = dHo + ( 8.314 x 270)
dHo = 8215.22
so
dHo = 8.215 kJ/mole
now
dGo = dHo - TdSo
so
-34912 = 8215.22 - ( 270 x dSo)
dSo = 159.7
so
dSo = 159.7 J/mol
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