Thermodynamics Lab Report
3.2.2. Adsorption thermodynamics
The deduction of the thermodynamic Gibbs free energy (ΔG◦), enthalpy (ΔH◦) in addition to entropy change (ΔS◦) was carried out by examining the adsorption batches under different temperatures ranged between 20 and 400C.
After performing the adsorption under any definite temperature, the equilibrium constant (KC) were anticipated using the following equation.
KC = Cad / Ce (6) where Cad is the concentration of Hg(II) ions adsorbed on the resin at equilibrium (mg/g) and Ce is the equilibrium concentration of Hg(II) ions in the aqueous medium (mg/L).
Eq. (7) can be then employed to estimate ΔG◦ (kJ mol-1)
ΔGoads = −RT ln KC (7) where R = 8.314 J/mol K
Both ΔH◦ and ΔS◦ were finally anticipated by plotting the reciprocal of temperature (Kelvin) versus lnKC (Fig. 5).in accordance with Eq. 8. lnKC = ΔSoads/R − ΔHoads/RT
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