## Nomenclature  
\(A_{o},A_{1},A_{2}\) coefficients of the three-parametric Equation (40), \(A_{1}\) in K, pre-exponential factor, s\({}^{-1}\),  
\(B\)=2.08364\(\cdot 10^{10}(\mathbf{K}\cdot\mathbf{s})^{-1}\),  
\(C\) integrals constant,  
\(CQF\) Compensation Quality Factor as in [48; 49],  
\(E\) activation energy, J mol\({}^{-1}\),  
kinetics functions,  
\(\Delta G\) free enthalpy, J mol\({}^{-1}\)  
\(H=6.62607\times 10^{-34}\) Js,  
Planck constant  
\(H=\Delta G^{+}(T_{c})\)  
\(\Delta H\) enthalpy, Jmol\({}^{-1}\),  
\(k_{\mathbf{K}\mathbf{T}\mathbf{S}}\) rate constant and dependent on \(T\), s\({}^{-1}\),  
\(k_{\mathbf{B}}=1.38065\cdot 10^{-23}\) JK\({}^{-1}\) Boltzmann constant,  
\(k_{iso}\) average value of the isokinetic constant, s\({}^{-1}\),  
\(K\) position of coalescence as in [49], or position parameter,  
\(m\) coefficients,  
\(n\) exponent,  
\(N\) number of data,  
\(p\) pressure, Pa,  
\(r^{2},R^{2}\) coefficients of linear or multiple determination,Analysis of _KCE_ for Experimental Data  
The _KCE_ resulting from the analysis of the experimental data on the thermal dissociation of calcite in nitrogen is presented in Figure 11. While Figure 11 presents the _KCE_ resulting from the analysis of data according to Equation (35) for seven different heating rates. Figure 10b presents the KCE for six different heating rates, omitting data for q = 1/60 K\(\cdot\)s\({}^{-1}\). Despite the small variability of the parameters of the Arrhenius law, they meet the _KCE_ at a sufficient level of significance. The average results provided in the description of Figure 11 are consistent with the data presented by [PERSON] [21] for the 0 th order kinetics (E = 191 kJ\(\cdot\)mol\({}^{-1}\), ln\(A\) = 15.4/\(A\) in s\({}^{-1}\)). The average values obtained with the use of the kinetic function (37) are slightly different, as presented in Figure 12.  
In relation to the analysis presented in Figure 12. the isoconversional approach of Equation (37) for the average values of \(E\) and ln \(A\) is not too much of an outlier and falls within the ranges presented in [21] but with an unsatisfactory coefficient of determination. However, it should be noted that the calculated isokinetic temperatures differ significantly depending on the data selection method. In the case of experimental research, when we analyze only the available range of increase in the conversion rate from temperature (here \(\alpha\in[0.1-0.9]\)) a different type of _KCE_ is observed for the constant heating rate analyses and a different type for the isoconversional method. The position presented in [5] is thus confirmed. Figures A3 and A4 show the _KCE_ resulting from the analysis of experimental data of thermal dissociation of calcite in nitrogen from Equations (36) and (38). Physicochemical sense of isokinetic temperature  
Temperature \(T^{*}\) in Equation (46) follows from implication, when:  
\[\left|\frac{1}{T_{min}}-\frac{1}{T_{high}}\right|<\left|\frac{1}{T_{min}}-\frac {1}{T_{low}}\right|\text{.then }T^{*}=T_{low}\] (A1)  
\[\left|\frac{1}{T_{min}}-\frac{1}{T_{high}}\right|>\left|\frac{1}{T_{min}}-\frac {1}{T_{low}}\right|\text{.then }T^{*}=T_{high}\] (A2)  
In Equation (48), the quantity 0.29 \(\approx\) 1-\(\sqrt{\frac{1}{2}}\) is the _CQF_ threshold for an infinite number of \(N\) measurements. The individual temperatures denote the test temperature interval: \(T_{low}\) is the arithmetic mean of the initial temperatures, \(T_{high}\) is the mean temperature of the end of the interval and \(T_{hm}\) is the harmonic mean of the temperatures \(T_{low}\). \(T_{high}\). For Equation (46) limit values are observed:  
* in the simplest variant: \(r^{2}\equiv 1\)\(CQF=1\)when \(T^{*}=T_{iso}.CQF=1-\sqrt{r^{2}}=1-r\) (A3) which means that the isokinetic temperature is the beginning/end of the temperature interval.