The value of ΔG°( gibbs free energy change) by two different methods are 257kj and 259kj .
Given ,
the oxidation reaction ,
CO(g) + 1/2 O2 (g) → CO2 (g)
Method-1 :
We know ,
ΔGrxn = sum of ΔG (product ) - sum of ΔG (reactant )
ΔGrxn =-394.39 - (-137.16) = -257.23kj
Method-2 :
We know ,
ΔG = ΔH -TΔS
T =298K
Thus , ΔHrxn = sum of ΔH (product ) - sum of ΔH (reactant )
ΔHrxn =-393.5 -(-110.522) = -282.978kj
ΔSrxn = sum of ΔS (product ) - sum of ΔS( reactant )
ΔSrxn = 51.07j/molK - 4.6j/molK = 46.47j/molK
ΔSrxn = 0.04647kj/molK
Thus , ΔG = ΔH - TΔS
ΔG = -282.978kj - ( 298 × 0.04647 kj )
ΔG = - 259kj
Hence , the value of ΔG° is 259kj .
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