Given
MO2 (s) ==> M(s) + O2(g) ΔG° = 289.8 kJ/mol
Temperature = 25°C = (25+273) K = 298 K
Other reaction is conversion of graphite to carbon dioxide
C (s) + O2 (g) ==> CO2 (g) ΔG° = - 394.4 kJ/mol
Chemical equation of coupled process is
Adding both the equations give
MO2 (s) ==> M (s) + O2 (g). ΔG° = 289.8 kJ/mol
C(s) + O2 (g) ==> CO2 (g). ΔG° = -394.4 kJ/mol
-------------------------------------------
MO2 (s) + C(s) + O2 (g) ==> M(s) + O2(g) + CO₂(g)
MO2 (s) + C(s) ==> M(s) + CO2 (g)
The above one is the chemical equation of coupled process
Now
ΔG⁰ = 289.8 kJ/mol -394.4 kJ/mol
= -104. 6 kJ/mol
We know that
ΔG°=−RT lnK
K = e^( - ΔG/RT)
= e^((104.6 kJ/mol) / (8.314 J/mol K * 298 K))
= 2.16 * 10^(18)
Hence thermodynamic equilibrium constant for the coupled reaction is
2.16 * 1018
What is the chemical equation of this coupled process? Show that the reaction is in equilibrium....
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