Respuesta :
-806.859 kJ is the value of Gibb's free energy of the given reaction.
How we calculate the Gibb's free energy change?
We calculate the ΔG for the given reaction is as:
ΔG = ΔG° + RTlnKc, where
R = universal gas constant = 8.314 J/K.mole
ΔG° = standard Gibb's free energy which can be calculated as:
ΔG° = ΔH° - TΔS°, where
ΔH° = Change in enthalpy = -803 kJ (given) = -803000J
T = temperature = 293K (given)
ΔS° = Change in entropy = -4.05 J/K (given)
On putting all these values in the above equation, we get
ΔG° = -803000 - 293 × (-4.05) = -801813.35J
Also we have to calculate the value of equilibrium constant for the given reaction:
CH₄ (g) + 2O₂ (g) ⇄ CO₂ (g) + 2H₂O (g)
Kc = [CO₂][H₂O]² / [CH₄][O₂]²
Given that:
Concentration of CO₂ = 3.83 M
Concentration of H₂O = 6.41 M
Concentration of CH₄ = 14.51 M
Concentration of O₂ = 9.27 M
On putting all these values in the above equation, we get
Kc = (3.83)(6.41)² / (14.51)(9.27)² = 0.126
Now we put all the calculated values in the first equation of Gibb's free energy, we get
ΔG = -801813.35 + 8.314×293 ln(0.126)
ΔG = -806859.46J = -806.859 kJ
Hence, -806.859 kJ is the value of ΔG.
To know more about Gibb's free energy, visit the below link:
brainly.com/question/10012881
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