## What is/are Equilibrium Adsorption?

Equilibrium Adsorption - Furthermore, Langmuir, Freundlich and Temkin isotherms were employed to analyze the equilibrium adsorption data.^{[1]}The equilibrium adsorption capacities (mg/g) of MO and FG using M–biochar (MO = 0.

^{[2]}Equilibrium adsorption capacity is determined by a series of different experimental conditions such as pH, time, and concentration of dye solution.

^{[3]}The equilibrium adsorption experiments showed S-shaped isotherms following the Freundlich model and an increase in adsorption capacity as equilibrium concentration increased.

^{[4]}The equilibrium adsorption data were analyzed by Langmuir, Freundlich and Dubinin–Radushkevich isotherm models.

^{[5]}The equilibrium adsorption data were analyzed using Weber–van Vliet, Fritz–Schlunder and Hill isotherm models to find the best-fit isotherm.

^{[6]}The Langmuir, Freundlich and Temkin models were fitted into equilibrium adsorption data and the calculated results depict a better and satisfactory correlation for Langmuir with higher linear regression coefficients (Pb2+, 0.

^{[7]}The batch adsorption results on the effects of Na2CO3 impregnation ratio showed that equilibrium adsorption capacities were more than 0.

^{[8]}The equilibrium adsorption capacities for the adsorbent in the initial concentrations of Sr2+ of 50, 100, 150, 200, and 250 mg/g were 48.

^{[9]}Furthermore, the equilibrium adsorption isotherm was well-fitted by Langmuir models.

^{[10]}Most probably due the smooth morphology and more uniform configuration of the M-CuO-NPs, the changes between equilibrium adsorption (qe) and equilibrium concentration (Ce) were more regular than those of the A-CuO-NPs and R-CuO-NPs.

^{[11]}Results showed that equilibrium adsorption of ZrO2-surfactant and SiO2-surfactant solutions onto the adsorbent surface is best fitted with the Langmuir model, suggesting the feasibility of monolayer coverage of nanoparticles-surfactants solutions onto the rock surfaces.

^{[12]}Batch kinetics and equilibrium adsorption experiments confirmed the proper affinity of organoclays to a zwitterion antibiotic: the amoxicillin (AMX) which was quickly adsorbed (at a time below 30 min) at large amounts (up to 1.

^{[13]}The equilibrium adsorption data were investigated by Langmuir, Freundlich and Dubinin-Radushkevich isotherm models.

^{[14]}The equilibrium adsorption time of MO in the presence of TiO2 is reached after 50 min of contact.

^{[15]}Langmuir isotherm best fits the equilibrium adsorption data and the maximum capacity was 35.

^{[16]}Notably, the nanofiber carbon aerogel was able to adsorb 80% of the equilibrium adsorption capacity within 1 min and reach equilibrium within 15 min.

^{[17]}The equilibrium adsorption capacities of nHEP and MCH on UiO-66(2.

^{[18]}The equilibrium adsorption data are well described by the Freundlich adsorption model.

^{[19]}The results showed that the equilibrium adsorption data was found to fit better to the Langmuir adsorption model, and the adsorption capacity for the removal of MB on Bent-APTES was 217.

^{[20]}Langmuir and Freundlich isotherm model were applied to describe the equilibrium adsorption.

^{[21]}We also investigated the equilibrium adsorption of Cu(II) and rhodamine B (RB) on CFA–HAp1–4.

^{[22]}This work explains a detailed methodology for the obtention of adsorption enthalpy, entropy and Gibbs energy of protein adsorption, by using ITC together with equilibrium adsorption isotherms.

^{[23]}In batch MOAC runs, the equilibrium adsorption capacities of 105.

^{[24]}We demonstrate that the adsorption kinetics of all the four types of emulsifiers near their equilibrium adsorption states can be well approximated by the ‘two adsorbing species model’ discussed in our previous work (Tripathi and Tabor, 2016).

^{[25]}Besides, the equilibrium adsorption uptake of water onto the composite adsorbents is measured gravimetrically at three different temperatures, 30, 50, and 70 °C.

^{[26]}In this study the equilibrium adsorption of MB and MO present in the water was investigated using nDCPD as bioadsorbent, an eco-economic and environmentally friendly material.

^{[27]}The equilibrium adsorption capacity of QAMCM for HISADP was 98.

^{[28]}The decrease of compression pressure markedly enhanced the equilibrium adsorption capacity (qe, exp), owing to the decreased diffusion resistance and blockage of diffusion pathways inside briquettes.

^{[29]}998, while the equilibrium adsorption study showed that the Langmuir isotherm was obeyed, which suggested that the adsorption is a monolayer and homogenous.

^{[30]}The arsenic removal performance was evaluated by testing the equilibrium adsorption isotherm, adsorption kinetics, and packed-bed operation.

^{[31]}The equilibrium adsorption data is well fit by the Langmuir isotherm; the linear model explains the aggregation of the solute by the adsorbent that is directly proportional to the solution concentration.

^{[32]}The equilibrium adsorption time for Cu(II) is 150 min in both solutions, while these for Zn(II) are 130 and 160 min in ethanol and aqueous solution.

^{[33]}The equilibrium adsorption behavior data was fitted well to Langmuir and Freundlich adsorption isotherm models.

^{[34]}The equilibrium adsorption capacity (mg/g) was found to be 12.

^{[35]}The equilibrium adsorption capacities of biochar for Cd(II) ranked as follows: 49.

^{[36]}The equilibrium adsorption time was obtained at 90 min for Cd(II), Cu(II) and Pb(II), as well as 120 min for Cr(VI) and Zn(II), respectively, for the mentioned metal ions removal.

^{[37]}The Langmuir isotherm model exhibited the best fit of the equilibrium adsorption data.

^{[38]}The results showed that the Langmuir isotherm model best describes the equilibrium adsorption with a high correlation coefficient.

^{[39]}Equilibrium adsorption capacities (qeth) of F+-MgO are 549.

^{[40]}In addition, the equilibrium adsorption capacity of NP10EO by MGO at 298K, 308K, and 318K can reach 87.

^{[41]}The samples’ equilibrium adsorption capacities for oxygen and argon (25°С and atmospheric pressure) and the separation coefficient of the argon–oxygen mixture as the ratio of Henry’s coefficients have been determined.

^{[42]}The equilibrium adsorption isotherms resulted in a metal ion uptake greater than 84%, and the Freundlich model fitted well the data.

^{[43]}The kinetic experiments show the equilibrium adsorption of MG on GW and AGW were attained after 360 min.

^{[44]}The physicochemical properties of the Pz1 and Pz2 compounds were studied using Langmuir adsorption isotherms, where the equilibrium adsorption data were found to follow it accurately.

^{[45]}The initial concentration was studied from 50 to 600 mg L-1, and the equilibrium adsorption capacities of Cs+, Co2+, and Sr2+ were found to increase from 8.

^{[46]}The kinetics and equilibrium adsorption data were analyzed using the common adsorption models.

^{[47]}The data from the equilibrium adsorption were fitted by linear and non-linear isotherm models; the optimal capacity of FAG/As(V) removal was calculated from the Langmuir model at 31.

^{[48]}The results showed that the equilibrium adsorption behavior of metal ions onto CS-ECH and PVA could be fitted to Langmuir model.

^{[49]}Fluorine adsorption by ES-800 reached 70% of the equilibrium adsorption amount within 15 min and gradually increased until 24 h.

^{[50]}

## pseudo second order

The value of the regression coefficient showed that the data The experimental results corresponded best to the pseudo-second order (PSO) model, while the Langmuir adsorption isotherms best described the equilibrium adsorption data with the highest qm of 43.^{[1]}Kinetic studies confirmed that the process followed a pseudo-second-order and that the Langmuir isotherm best fitted the equilibrium adsorption of nitrate.

^{[2]}All the equilibrium adsorption kinetics of Pb(II) are fitted well to the pseudo-second-order model.

^{[3]}The adsorption process of the CTA-StNPs onto kaolin could be divided into rapid adsorption, stable adsorption and equilibrium adsorption and followed pseudo second-order kinetic equation very well (R2 > 0.

^{[4]}Based on the adsorption kinetics of pharmaceuticals onto the FMC in synthetic urine, equilibrium adsorption was reached in 120 min, and it followed a pseudo-second-order model.

^{[5]}Langmuir isotherm was found to better describe the equilibrium adsorption data, while adsorption kinetic was conformed to the Pseudo second-order.

^{[6]}Equilibrium adsorption results followed the Freundlich isotherm, whereas the experimental kinetics data were best fitted to the pseudo-second-order equation.

^{[7]}The adsorption kinetics showed that both As(III) and As(V) adsorption followed a pseudo second-order kinetic model, and the equilibrium adsorption isotherm was best fitted using the Langmuir model.

^{[8]}The equilibrium adsorption of As(III) using NA41 was achieved within 24 h, and the obtained results corresponded to a pseudo-second-order model with correlation coefficient value of 0.

^{[9]}The Langmuir isotherm and pseudo-second-order kinetic models were observed to best describe the equilibrium adsorption and kinetic processes, respectively.

^{[10]}The adsorption kinetics showed that the experimental data were in good agreement with the pseudo-second-order kinetic model, and the equilibrium adsorption isotherm data fitted well with the Freundlich model.

^{[11]}Equilibrium adsorption data had the best agreement to the Freundlich isotherm model and pseudo-second-order kinetics model.

^{[12]}98 mg/g, and equilibrium adsorption data were more consistent with the Langmuir isotherm and pseudo-second-order kinetic model.

^{[13]}The adsorption process followed a pseudo-second-order reaction model, and the equilibrium adsorption was well fit by the Langmuir model.

^{[14]}The adsorption kinetics followed the pseudo-second-order model well while equilibrium adsorption from the pseudo-first order and Langmuir exhibited a large difference with experimental data.

^{[15]}Adsorption kinetics and the equilibrium adsorption isotherm were fitted by a pseudo-second-order alongside intraparticle diffusion kinetic models and Langmuir isotherm respectively.

^{[16]}The fitting results revealed that the equilibrium adsorption isotherms and adsorption kinetics followed the Langmuir model and pseudo-second-order model, respectively.

^{[17]}The best equilibrium adsorption capacity with KCG was observed to be 140 mg/g under pH 6 within 120 min, following a pseudo-second-order kinetic model.

^{[18]}The Langmuir isotherm and the pseudo-second-order kinetic models were the best fit for the equilibrium adsorption and kinetics experiments, and the maximum monolayer adsorption capacity (qmax) was found to be 353.

^{[19]}Adsorption of estrone, 17β-estradiol, and 17α-ethinylestradiol followed pseudo-second-order kinetic model, while the equilibrium adsorption data were best fitted with the Langmuir isotherm model.

^{[20]}Moreover, the comparison between the experimental and calculated data of equilibrium adsorption capacity demonstrated that the pseudo second-order kinetic equation fitted well with 38.

^{[21]}The results showed that the equilibrium adsorption data were found to fit better to the Langmuir adsorption model and the kinetic process of adsorption could be described by the pseudo-second-order model.

^{[22]}The adsorption kinetics data were best fitted by pseudo-second-order model and equilibrium adsorption was achieved within 5 min, indicating a rapid chemical adsorption efficiency.

^{[23]}Langmuir isotherm and a pseudo second order kinetic equation were fit models to describe the equilibrium adsorption and the kinetic behavior of MB on the adsorbents, respectively.

^{[24]}The equilibrium adsorption isotherm and kinetic data of ZnO-Hal were fitted well with Freundlich and pseudo-second-order models, respectively.

^{[25]}The adsorption kinetics and the equilibrium adsorption data indicated that the adsorption process of BPA and TC was more compatible with the pseudo-second-order kinetic model and the Langmuir model, respectively.

^{[26]}Freundlich model was the best in describing the equilibrium adsorption data with respect to both MO and RhB with the kinetic data for the two dyes both obeying pseudo-second-order kinetics model.

^{[27]}

## maximum adsorption capacity

The equilibrium adsorption data better fitted to the Freundlich isotherm model having a maximum adsorption capacity (qmax) of 319.^{[1]}After optimized condition experiment, Ni(ii)-IIP5 possessed maximum adsorption capacity and better imprinting factor under optimal experimental conditions which indicated by equilibrium adsorption experiments.

^{[2]}Equilibrium adsorption data were consistent with the Langmuir isotherm model, indicating surface homogeneity, with maximum adsorption capacity of 158.

^{[3]}For the equilibrium adsorption experiments, the target maximum adsorption capacity of 122 mg/g was predicted by a target optimizer and desirability function at the conditions following the pH of 4.

^{[4]}Langmuir isotherm model was best fit to the equilibrium adsorption data (maximum adsorption capacity of SS derived AC = 102 mg/g) whereas pseudo-second order model showed the best fit to adsorption kinetic data (adsorption capacity = 77.

^{[5]}The equilibrium adsorption data were fitted well by the Langmuir model and the maximum adsorption capacity of 863.

^{[6]}

## data fitted well

The equilibrium adsorption and kinetic data fitted well with the Freundlich adsorption isotherm and pseudo first order kinetics model respectively for CV.^{[1]}The equilibrium adsorption data fitted well with Langmuir and Freundlich isotherm models.

^{[2]}The equilibrium adsorption data fitted well with the Langmuir isotherm model with a maximum monolayer adsorption capacity of 55.

^{[3]}The equilibrium adsorption data fitted well with the Langmuir model.

^{[4]}Thanks to the synergistic effect of BC and rG, Pc-rGBC had good adsorption capacity to phenol molecules, and the equilibrium adsorption data fitted well with the Freundlich model.

^{[5]}

## pseudo first order

The equilibrium adsorption capacities (qe) of ACBC500 predicted by the pseudo-first-order and pseudo-second-order models for endrin were 245.^{[1]}In addition to it, associated Δ G ∙ (standard Gibbs free energy change), ΔH° (standard enthalpy change), ΔS° (standard entropy change), adsorption kinetics involved by pseudo-first-order, second order model and equilibrium adsorption by Langmuir and Freundlich isotherms are also debated.

^{[2]}The equilibrium adsorption had an alignment with Langmuir isotherms, while the kinetics were most accurately modelled using pseudo- first-order and second order models according to the regression analysis.

^{[3]}The equilibrium adsorption results fitted better with the Langmuir model, and the kinetic adsorption data provided a better fit with the pseudo-first-order model.

^{[4]}

## second order kinetic

Results indicated that the equilibrium adsorption data were best fitted with Langmuir and Temkin isotherms and kinetic data were well described by pseudo-first and second-order kinetic models.^{[1]}

## second order model

The kinetic results showed that the adsorption process of this polymer for organic dyes could be described with quasi-second-order models, and Langmuir isotherm adsorption models demonstrated that the maximum equilibrium adsorption capacity for methylene blue and toluidine blue was reached to 1806.^{[1]}

## Maximum Equilibrium Adsorption

The maximum equilibrium adsorption capacity was 1.^{[1]}The equilibrium data was fitted by modified Langmuir–Freundlich isotherm and the maximum equilibrium adsorption was 243.

^{[2]}The maximum equilibrium adsorption capacities of lignite for Cu and Zn were 67.

^{[3]}The maximum equilibrium adsorption capacity of naproxen on β-CD/rGO at 313 K was 361.

^{[4]}The maximum equilibrium adsorption capacity was 55 mg g-1.

^{[5]}AC-KOH-1-1 and AC-KMnO4-1-3 presented the maximum equilibrium adsorption capacities of 637.

^{[6]}The kinetic results showed that the adsorption process of this polymer for organic dyes could be described with quasi-second-order models, and Langmuir isotherm adsorption models demonstrated that the maximum equilibrium adsorption capacity for methylene blue and toluidine blue was reached to 1806.

^{[7]}The maximum equilibrium adsorption capacity of MO on WWR-800 was 454.

^{[8]}9 m2 g-1) and enhances the surface functional groups, leading to an improved maximum equilibrium adsorption amount from 21.

^{[9]}The maximum equilibrium adsorption capacity of copper ion is 80.

^{[10]}The results revealed that the maximum equilibrium adsorption capacity of 663 mg/g was achieved by MIL-100(Fe) with the highest specific surface area and pore volume.

^{[11]}0 had greater adsorption performance for BTH and 2-OH-BTH than Na-AMt (acidified Na-Mt), and the maximum equilibrium adsorption capacities of CPMMt-1.

^{[12]}The maximum equilibrium adsorption capacity was (37 mg/g).

^{[13]}The maximum equilibrium adsorption capacity value was 137.

^{[14]}Its CR adsorption behaviour was affected by such factors as pH, initial CR concentration and contact time, and had reached a maximum equilibrium adsorption capacity of ~941 mg/g under the neutral pH condition (~7.

^{[15]}The maximum equilibrium adsorption capacity was 1.

^{[16]}

## Experimental Equilibrium Adsorption

Moreover, the experimental equilibrium adsorption data were fitted to the Freundlich isotherm model with R 2 = 0.^{[1]}Langmuir, Freundlich, and Dubinin-Radushkevich (D-R) isotherm models were employed to correlate the experimental equilibrium adsorption data.

^{[2]}Freundlich isotherm yielded the best fit to the experimental equilibrium adsorption data with a correlation coefficient (R) of 0.

^{[3]}The experimental equilibrium adsorption data fitted best and well to the Freundlich isotherm model for CR dye adsorption and Langmuir Isotherm for MG adsorption.

^{[4]}The experimental equilibrium adsorption data were tested by the Temkin isotherm model with R2 > 0.

^{[5]}

## Isothermal Equilibrium Adsorption

In this paper, isothermal equilibrium adsorption experiments are done on phosphorus to study the influence of EPS on the adsorption characteristics of sediment particles, and the Langmuir adsorption isotherm is applied to analyze the adsorption rule of sediment particles under the impact of EPS.^{[1]}Further, the isothermal equilibrium adsorption study reveals the monolayer adoption of the metal ion by the Langmuir model with experimental and theoretical parameters, optimized by the linear regression analysis using the curve fitting tool in MATLAB software.

^{[2]}In brown-red soil, the effect of phosphorus and citric acid co-existence on the adsorption of cadmium was studied using indoor experiments and isothermal equilibrium adsorption analysis.

^{[3]}

## Good Equilibrium Adsorption

The results show that the activated carbon (AC)-R410A working fluid pair has the best performance because of its good equilibrium adsorption characteristic.^{[1]}To perform a reliable modeling, a good equilibrium adsorption isotherm is mandatory.

^{[2]}

## Best Equilibrium Adsorption

The best equilibrium adsorption isotherm model of each process was investigated based on the experimental and calculated R2 values of Freundlich and Langmuir models.^{[1]}The best equilibrium adsorption capacity with KCG was observed to be 140 mg/g under pH 6 within 120 min, following a pseudo-second-order kinetic model.

^{[2]}

## Variou Equilibrium Adsorption

The adsorption data validity was estimated by applying various equilibrium adsorption models and fitted by linear and non-linear regression models (kinetic and isotherm models).^{[1]}The experimental adsorption data were tested by employing various equilibrium adsorption models, and the Freundlich and Dubinin-Radushkevich (D-R) isotherms best depicted the observations.

^{[2]}

## Achieved Equilibrium Adsorption

The achieved equilibrium adsorption capacity of 6.^{[1]}The results showed that BDB, SP, and BSP achieved equilibrium adsorption capacity of 96.

^{[2]}

## High Equilibrium Adsorption

The results show the suitability of using MPs to remove P in treated wastewater due to both their high equilibrium adsorption capacity (q) and P removal efficiency.^{[1]}Therefore, the mesoporous carbon had high equilibrium adsorption amounts (374.

^{[2]}

## equilibrium adsorption capacity

The equilibrium adsorption capacities (mg/g) of MO and FG using M–biochar (MO = 0.^{[1]}Equilibrium adsorption capacity is determined by a series of different experimental conditions such as pH, time, and concentration of dye solution.

^{[2]}The batch adsorption results on the effects of Na2CO3 impregnation ratio showed that equilibrium adsorption capacities were more than 0.

^{[3]}The equilibrium adsorption capacities for the adsorbent in the initial concentrations of Sr2+ of 50, 100, 150, 200, and 250 mg/g were 48.

^{[4]}Notably, the nanofiber carbon aerogel was able to adsorb 80% of the equilibrium adsorption capacity within 1 min and reach equilibrium within 15 min.

^{[5]}The results show that one of the carbons prepared (GAC-3) has high CH4 equilibrium adsorption capacity (3.

^{[6]}The equilibrium adsorption capacities of nHEP and MCH on UiO-66(2.

^{[7]}In batch MOAC runs, the equilibrium adsorption capacities of 105.

^{[8]}The equilibrium adsorption capacity of QAMCM for HISADP was 98.

^{[9]}The decrease of compression pressure markedly enhanced the equilibrium adsorption capacity (qe, exp), owing to the decreased diffusion resistance and blockage of diffusion pathways inside briquettes.

^{[10]}The equilibrium adsorption capacity (mg/g) was found to be 12.

^{[11]}The equilibrium adsorption capacities of biochar for Cd(II) ranked as follows: 49.

^{[12]}Equilibrium adsorption capacities (qeth) of F+-MgO are 549.

^{[13]}In addition, the equilibrium adsorption capacity of NP10EO by MGO at 298K, 308K, and 318K can reach 87.

^{[14]}The samples’ equilibrium adsorption capacities for oxygen and argon (25°С and atmospheric pressure) and the separation coefficient of the argon–oxygen mixture as the ratio of Henry’s coefficients have been determined.

^{[15]}The initial concentration was studied from 50 to 600 mg L-1, and the equilibrium adsorption capacities of Cs+, Co2+, and Sr2+ were found to increase from 8.

^{[16]}The maximum equilibrium adsorption capacity was 1.

^{[17]}The equilibrium adsorption capacities of DAF-HMSS were computed via the conductor-like screening models with segmented activity coefficients known as COSMO-SAC.

^{[18]}For the initial concentration of 100 mg/L of MB, the biomaterial obtained after acid treatment (HMCE) has an equilibrium adsorption capacity of 19.

^{[19]}The equilibrium adsorption capacities (qe) of ACBC500 predicted by the pseudo-first-order and pseudo-second-order models for endrin were 245.

^{[20]}The obtained 3D α-HH straw-sheaves are further used as an adsorbent to remove Pb2+ from water, exhibiting excellent Pb2+ removal performance with an equilibrium adsorption capacity of 79.

^{[21]}The high-efficiency of the MOF-808 hollow fibre adsorbent is exhibited by retainment of its equilibrium adsorption capacity of 796 mg g−1.

^{[22]}The synthesized polymers had larger equilibrium adsorption capacities toward e-caprolactam (qmax = 69.

^{[23]}Under this condition, acetone’s equilibrium adsorption capacity by modified activated carbon (1% KOH-AC) reached 0.

^{[24]}Equilibrium adsorption capacities and kinetic rates were quantified with batch experiments.

^{[25]}The maximum equilibrium adsorption capacities of lignite for Cu and Zn were 67.

^{[26]}Under the optimal conditions, the equilibrium adsorption capacity of Cd (II) was 43.

^{[27]}The equilibrium adsorption capacity of phenol on HPN-DCM-DCE reached 24.

^{[28]}Also, the amount of equilibrium adsorption capacity is 36 mg g–1 in the real sample.

^{[29]}It was established that an increase in the temperature of the model solution leads to an increase in the equilibrium constant and equilibrium adsorption capacity, at the same time as decreasing the accuracy of isotherm description.

^{[30]}It has been found that the activated carbons can effectively adsorb RhB due to high mesoporosity and RhB equilibrium adsorption capacity (qe) increased almost linearly with increasing total mesopore volumes, regardless of the activation agents.

^{[31]}The maximum equilibrium adsorption capacity of naproxen on β-CD/rGO at 313 K was 361.

^{[32]}The achieved equilibrium adsorption capacity of 6.

^{[33]}The maximum equilibrium adsorption capacity was 55 mg g-1.

^{[34]}The results show the suitability of using MPs to remove P in treated wastewater due to both their high equilibrium adsorption capacity (q) and P removal efficiency.

^{[35]}AC-KOH-1-1 and AC-KMnO4-1-3 presented the maximum equilibrium adsorption capacities of 637.

^{[36]}The equilibrium adsorption capacity (qe) increases with the increase of the initial concentration of T.

^{[37]}The adsorption experiment of RhB revealed that CAP7–27 had not only an equilibrium adsorption capacity of 198 mg·g−1, but also an adsorption rate of 162.

^{[38]}The equilibrium adsorption capacity of the coffee grounds was 4 mg/g for a reaction time of 40 min.

^{[39]}LAD adsorbed AR 73 solution with initial concentration of 100mg/L for 2h to reach equilibrium, with equilibrium adsorption capacity and adsorption rate of 47.

^{[40]}The equilibrium adsorption capacity was approximately 1100 μg/g.

^{[41]}170 kHz pre-treated sample exhibited an equilibrium adsorption capacity of 19.

^{[42]}The kinetic results showed that the adsorption process of this polymer for organic dyes could be described with quasi-second-order models, and Langmuir isotherm adsorption models demonstrated that the maximum equilibrium adsorption capacity for methylene blue and toluidine blue was reached to 1806.

^{[43]}The maximum equilibrium adsorption capacity of MO on WWR-800 was 454.

^{[44]}The equilibrium adsorption capacities of Cd (II), Ni (II), and Pb (II) for P.

^{[45]}The results showed that under the conditions of 308 K and pH = 5, NH2-CTS/MZ reached adsorption equilibrium within 180 min, and the equilibrium adsorption capacity was 749.

^{[46]}The maximum equilibrium adsorption capacity of copper ion is 80.

^{[47]}The adsorption kinetics and isotherm presented that the enhanced physicochemical properties of TB surface through the chemical activation with CaCl2 (CTB) and FeCl3 (FTB) were helpful in the adsorption capacities of PO43− (equilibrium adsorption capacity: FTB (1.

^{[48]}The equilibrium adsorption capacity reached 49.

^{[49]}The results showed that with the increase of Ca2+ concentration, the equilibrium adsorption capacity of illite increased, and the adsorption equilibrium was basically achieved at 60 min.

^{[50]}

## equilibrium adsorption datum

Furthermore, Langmuir, Freundlich and Temkin isotherms were employed to analyze the equilibrium adsorption data.^{[1]}The equilibrium adsorption data were analyzed by Langmuir, Freundlich and Dubinin–Radushkevich isotherm models.

^{[2]}The equilibrium adsorption data were analyzed using Weber–van Vliet, Fritz–Schlunder and Hill isotherm models to find the best-fit isotherm.

^{[3]}The Langmuir, Freundlich and Temkin models were fitted into equilibrium adsorption data and the calculated results depict a better and satisfactory correlation for Langmuir with higher linear regression coefficients (Pb2+, 0.

^{[4]}The equilibrium adsorption data were investigated by Langmuir, Freundlich and Dubinin-Radushkevich isotherm models.

^{[5]}Langmuir isotherm best fits the equilibrium adsorption data and the maximum capacity was 35.

^{[6]}Temperature dependent equilibrium adsorption data were modelled using non-linear regression in the range 303–323 K.

^{[7]}The equilibrium adsorption data are well described by the Freundlich adsorption model.

^{[8]}The results showed that the equilibrium adsorption data was found to fit better to the Langmuir adsorption model, and the adsorption capacity for the removal of MB on Bent-APTES was 217.

^{[9]}The value of the regression coefficient showed that the data The experimental results corresponded best to the pseudo-second order (PSO) model, while the Langmuir adsorption isotherms best described the equilibrium adsorption data with the highest qm of 43.

^{[10]}Freundlich and Langmuir isotherm models fitted in good agreement equilibrium adsorption data.

^{[11]}The equilibrium adsorption data fitted well with Langmuir and Freundlich isotherm models.

^{[12]}The equilibrium adsorption data is well fit by the Langmuir isotherm; the linear model explains the aggregation of the solute by the adsorbent that is directly proportional to the solution concentration.

^{[13]}The equilibrium adsorption data fitted well with the Langmuir isotherm model with a maximum monolayer adsorption capacity of 55.

^{[14]}The Langmuir isotherm model exhibited the best fit of the equilibrium adsorption data.

^{[15]}The equilibrium adsorption data better fitted to the Freundlich isotherm model having a maximum adsorption capacity (qmax) of 319.

^{[16]}The physicochemical properties of the Pz1 and Pz2 compounds were studied using Langmuir adsorption isotherms, where the equilibrium adsorption data were found to follow it accurately.

^{[17]}The kinetics and equilibrium adsorption data were analyzed using the common adsorption models.

^{[18]}In both bleaching methods, the equilibrium adsorption data follows the Toth isotherm model, presenting the sorption occurrence tends to be on a heterogeneous surface.

^{[19]}Also, different isotherms including Langmuir, Freundlich, and Dubinin-Radushkevich were applied to evaluate the equilibrium adsorption data.

^{[20]}The equilibrium adsorption data, tested against three classical nonlinear adsorption isotherms, was best described by the Freundlich model.

^{[21]}Langmuir isotherm was found to better describe the equilibrium adsorption data, while adsorption kinetic was conformed to the Pseudo second-order.

^{[22]}The equilibrium adsorption data were obeyed to Langmuir model.

^{[23]}Equilibrium adsorption data fitted the Langmuir adsorption isotherm well with R^2=0.

^{[24]}In this work, we present equilibrium adsorption data of H2 and CH4 on zeolite 13X, in addition to the already established CO2 isotherms.

^{[25]}Kinetic studies showed that the adsorption was well described by the pseudo–second-order model and the equilibrium adsorption data fitted Freundlich model.

^{[26]}The equilibrium adsorption data were analyzed by the theroy equations and thermodynamic study.

^{[27]}The