The present study as designed to assess the CO2 and N2 adsorption isotherms on activated carbon (AC). The AC was characterized with SEM, XRD and N2 isotherm. The CO2 and the N2 adsorption experiments on the AC are performed at 298, 308 and 328 K and modelled by Langmuir model. The preferred selectivity (αCO2/N2) was obtained with the use of the Langmuir properties and the Henry coefficient (KH) was found from the viral equation. The thermodynamic analysis of CO2 and N2 adsorption which include the entropy loss (ΔS), the Gibbs free energy change (ΔG) and the surface potential (Ω) was calculated. The results reveal that the order of CO2 uptake on AC is higher than that of N2. Moreover, the reduction of temperature increases the separation coefficients of CO2 on N2. The adsorption affinity and the adsorption spontaneity of CO2 is the highest, while N2 has the lowest adsorption spontaneity. Subsequently the CO2 has a higher interaction with AC, while the N2-AC interaction is the lightest. Subsequently, CO2 exhibits a higher interaction with AC, in contrast to N2 which displays a slight interaction.