Answer :
Final answer:
For the given system, the change in Gibbs free energy (ΔG) is calculated to be approximately 175.26 kJ. As ΔG is positive, the reaction is considered to be non-spontaneous, signifying that it requires some form of energy input in order to proceed.
Explanation:
The given system can be evaluated according to the Gibbs free energy equation, which is ΔG = ΔH - TΔS. In this equation, ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, ΔS is the change in entropy, and T is the temperature in Kelvin. Before applying the values, it is important to convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. So, the Kelvin temperature equals 149 °C plus 273.15, which is 422.15 K. Plugging the values into the Gibbs free energy equation we get ΔG = 147 kJ - (422.15 K x -67.0 J/K x 1 kJ/1000 J). Simplified, this yields ΔG = 147 kJ - (-28.26415 kJ), which results in ΔG being approximately 175.26 kJ.
If the calculated quantity of ΔG is positive, as in this instance, the reaction is non-spontaneous. This is because a positive ΔG suggests that the reaction requires energy input to proceed, whereas a negative ΔG denotes a spontaneous reaction that proceeds without any energy input. The spontaneity of a process, in terms of the algebraic sign of its free energy change, is subsequently determined by the signs of the enthalpy and entropy changes, and in some scenarios, the absolute temperature.
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