Shradheya Raj Rajeshwar Gupta

Use the following formulas:

1. **From -logKd, -logKi, or -logIC50**:

- ΔG = -R × T × ln(10) × (-logK)

- Where:

- R is the universal gas constant (8.314 J/mol·K)

- T is the absolute temperature (typically 298.15 K for standard conditions)

- K is the dissociation constant (Kd, Ki, or IC50 in nM)

Example:

- Given: -logKd = 8

- ΔG = -8.314 J/mol·K × 298.15 K × ln(10) × (-8)

- ΔG = -47.85 kJ/mol

2. **From Ki or KD (in nM)**:

- ΔG = -R × T × ln(Ki or KD × 10^-9)

- Where:

- R is the universal gas constant (8.314 J/mol·K)

- T is the absolute temperature (typically 298.15 K for standard conditions)

- Ki or KD is the dissociation constant in nM

Example:

- Given: Ki = 9 nM

- ΔG = -8.314 J/mol·K × 298.15 K × ln(9 × 10^-9)

- ΔG = -46.75 kJ/mol

3. **From IC50 (in nM)**:

- ΔG = -R × T × ln(IC50 × 10^-9)

- Where:

- R is the universal gas constant (8.314 J/mol·K)

- T is the absolute temperature (typically 298.15 K for standard conditions)

- IC50 is the half-maximal inhibitory concentration in nM

Example:

- Given: IC50 = 4 nM

- ΔG = -8.314 J/mol·K × 298.15 K × ln(4 × 10^-9)

- ΔG = -48.58 kJ/mol

The key steps are:

1. Convert the given data (e.g., -logKd, Ki, IC50) to the corresponding dissociation constant (Kd, Ki, or IC50) in nM.

2. Use the appropriate formula to calculate the Gibbs free energy change (ΔG) based on the dissociation constant.

Good luck; partial credit ai

Mohammad Ima Thank you for your answer, I am not sure that calculating ΔG from IC50 with this equation " ΔG = -R × T × ln(IC50 × 10^-9) " work. I also tried AI, it is giving me the same answer but I am not sure if it is correct or not.