Question

What is the approximate value of ΔS° for binding of NAG3 to HEW at 27°C?ΔH° = -50 kJ/mol, ΔG° = -30 kJ/mol.-200 J/K-67 J/K67 J/K200 J/K

Answer 1

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).