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Answer :
The temperature of a reaction can be determined using the Gibbs free energy equation, which states that
ΔG° = -RTlnK,
where ΔG° is the standard free energy change of the reaction,
R is the gas constant,
T is the temperature in Kelvin, and
K is the equilibrium constant.
By rearranging the equation, we can solve for the temperature (T) as T = -ΔG°/ (RlnK).
In this problem, we are given that K = 1.2 x 10^-6 and ΔG° = +36.9 kJ/mol. We can substitute these values into the equation and solve for the temperature as:
T = -(+36.9 kJ/mol) / (8.314 J/mol K * ln(1.2 x 10^-6))
T = 548.7 K or 275.7°C
Therefore, the temperature of the reaction is approximately 275.7°C if K = 1.2 x 10^-6 when ΔG° = +36.9 kJ/mol.
If the temperature is changed, the value of K will also change, indicating whether the reaction will favor the formation of products or reactants at the new temperature.
To know more about Gibbs free energy here
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