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Liquids: comparison with experiment
Published in Michael de Podesta, Understanding the Properties of Matter, 2020
was proportional to p, the number atoms per chemical formula unit of the substance. Thus the molar heat capacity of NaCl is close to twice the value of an elemental solid because there are twice as many atoms present. Thus the reason for the increase in molar heat capacity of substances as a function of molecular complexity is simply that there are more atoms present in a mole, and thus the possibility of more degrees of molecular vibration and rotation.
Enthalpy and Heat Capacity
Published in Jean-Louis Burgot, Thermodynamics in Bioenergetics, 2019
The notion of heat capacity C of a system has already be mentioned in Chapter 2. It can be considered as being the proportionality constant of the following equation: Q = C(T2 − T1) where Q is the heat quantity given to the system for an increase of its absolute temperature from T1 to T2. C is proportional to the mass of the system. For 1 g of it, its value is called the specific heat. The heat capacity for 1 mole of material is named the molar heat capacity.
Energy Metrics
Published in John Andraos, Synthesis Green Metrics, 2018
Heat capacity is the energy required to change the temperature of a unit mass (specific heat) or mole (molar heat capacity) of the material by one degree. Units: J/(kg deg K); J/(mol deg K). The formal thermodynamic definition is given by the derivative shown in Equation (5.25). Cp=(∂H∂T)p
Modeling of the HCPB Helium Coolant Purification System for EU-DEMO: Process Simulations of Molecular Sieves and NEG Sorbents
Published in Fusion Science and Technology, 2023
Jonas C. Schwenzer, Alessia Santucci, Christian Day
where = molar heat capacity of the fluid= specific surface area of the sorbents= heat transfer coefficient= mass of the sorbents= sorbents mass heat capacity= loading of the sorbents (mol‧kg−1)= heat of adsorption= molar heat capacity of the sorbate.
An improved correlation for thermophysical properties of binary liquid mixtures
Published in Chemical Engineering Communications, 2023
Gustavo A. Iglesias-Silva, José J. Cano-Gómez, Mariana Ramos-Estrada, Kenneth R. Hall
The mixtures F113 (1) + oxygenated and hydrocarbon solvents (Dohnal et al. 1993) show different behaviors at 298.15 K. For example, the excess molar heat capacity of F113 (1) + dipropyl ether (2) has positive and negative deviations from ideality. Again, Equation (4) could correlate correctly the molar heat capacity, but it did not predict correctly the excess molar heat capacity. Equation (16) correlates and predicts correctly within ± 0.025 and 0.031 J·K−1·mol−1, respectively, as shown in Figure 11. Also, Equation (17) works within ± 0.019 and 0.024 J·K−1·mol−1. Table 1 contains the number of parameters and the values of the objective function. The excess molar heat capacity of F113 (1) + diisopropyl ether (2) shows positive deviations from ideality. As is apparent in Figure 11, the prediction of the excess molar heat capacity from Equation (4) is almost correct except that it misses the maximum and the concavity of the function. The prediction of Equation (17) with only two parameters is better than Equation (16).
Simulation of underground coal gasification based on a coupled thermal-hydraulic-chemical model
Published in Combustion Theory and Modelling, 2022
Wu Gao, Renato Zagorščak, Hywel Rhys Thomas, Ni An
Thermal properties such as thermal conductivity and heat capacity of gas and solid are important for heat transport [12,24–26]. In this model, thermal conductivity and heat capacity of gas and solid are considered as function of temperature. For instance, the temperature-dependent thermal conductivity of mixed gases can be calculated by the following equation [25]: where , , , , and are constant coefficients. Temperature-dependent molar heat capacity of the ith gas component can be expressed by [25]: where , , , , and are constant coefficients, and is the molar weight of the ith gas component.