Question

Розрахуйте зміну вільної енергії Гіббса ΔG при перенесенні 3 моль неполярного з'єднання з розчинника у воду при температурі t = 27 °С, якщо відомо, що ентропія S при цьому зменшується на 80 Дж/(моль∙К), та ентальпія H зменьшується на 10 кДж/моль

Answer 1

To calculate the change in Gibbs free energy (ΔG) when transferring 3 moles of a nonpolar compound from a solvent to water at a temperature of 27 °C, we need to use the equation:

ΔG = ΔH - TΔS

where ΔH is the change in enthalpy, ΔS is the change in entropy, and T is the temperature in Kelvin.

Given that the entropy change (ΔS) is -80 J/(mol∙K) and the enthalpy change (ΔH) is -10 kJ/mol, we can proceed with the calculation.

Conversion of Units:

First, let's convert the enthalpy change from kilojoules per mole to joules per mole: -10 kJ/mol = -10,000 J/mol

Calculation:

Now, we can substitute the values into the equation: ΔG = -10,000 J/mol - (27 + 273) K * (-80 J/(mol∙K))

Simplifying the equation: ΔG = -10,000 J/mol - 300 K * (-80 J/mol)

Calculating the change in Gibbs free energy: ΔG = -10,000 J/mol + 24,000 J/mol

ΔG = 14,000 J/mol

Therefore, the change in Gibbs free energy (ΔG) when transferring 3 moles of the nonpolar compound from a solvent to water at a temperature of 27 °C is 14,000 J/mol.

Please note that the calculation assumes ideal conditions and may not account for all factors that could affect the system.