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Answer :
Final answer:
The value of ΔGº for this reaction is approximately -38.8 kJ.
Explanation:
To calculate the standard Gibbs free energy change (ΔGº) for a reaction, we can use the equation ΔGº = -RT ln(K), where R is the gas constant (8.31 J/(mol·K)), T is the temperature in Kelvin, and K is the equilibrium constant.
In this case, the given equilibrium constant (K) is 6.32 106 and the temperature (T) is 298 K.
Substituting these values into the equation, we have:
ΔGº = - (8.31 J/(mol·K)) * (298 K) * ln(6.32 106)
Calculating this expression, we find that ΔGº is approximately -38.8 kJ.
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