Answer:
ΔS° ≈ -66.6 J/(mol*K)
Step-by-step explanation:
We can use the Gibbs-Helmholtz equation to relate the enthalpy and entropy changes to the free energy change:
ΔG° = ΔH° - TΔS°
where ΔG° is the standard free energy change, ΔH° is the standard enthalpy change, ΔS° is the standard entropy change, and T is the temperature in Kelvin.
Rearranging the equation, we can solve for ΔS°:
ΔS° = (ΔH° - ΔG°) / T
Substituting the given values, we get:
ΔS° = (-50 kJ/mol - (-30 kJ/mol)) / (27°C + 273.15) K
ΔS° = -20 kJ/mol / 300.15 K
ΔS° ≈ -66.6 J/(mol*K)
Therefore, the approximate value of ΔS° for the binding of NAG3 to HEW at 27°C is -66.6 J/(mol*K).