Answer :
Final answer:
The change in Gibbs free energy (">">ΔG") for the reaction at 298 K is calculated using the equation ">">ΔG = ΔH - TΔS". Given ">">ΔH = 134.1 kJ" and ">">ΔS = 35.0 J/K", after appropriate conversion and calculation, the result is ">">123.67 kJ".None of the Given option are correct and the correct answer for the Question is 123.67 kJ.
Explanation:
To calculate the change in free energy (">">">ΔG") for the reaction at 298 K, you can use the Gibbs free energy equation:
">">ΔG = ΔH - TΔS", where ">">ΔH" is the change in enthalpy, ">">T" is the temperature in Kelvin, and ">">ΔS" is the change in entropy.
In the given question, ">">ΔH = 134.1 kJ" and ">">ΔS = 35.0 J/K". To use the correct units, you must convert ">">ΔS" to kJ by dividing by 1000, giving ">">ΔS = 0.035 kJ/K".
Substituting the given values into the equation:
">">ΔG = ΔH - TΔS
ΔG = 134.1 kJ - (298 K)(0.035 kJ/K)
ΔG = 134.1 kJ - 10.43 kJ
ΔG = 123.67 kJ", which is not among the answers provided.
However, as there may have been an error in the question since none of the answer choices match the calculated ">">ΔG". It's important to double-check the question and the answer choices for any mistakes.
