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Grigull, Ulrich; Straub, Johannes; Schiebener, Peter

doi:10.1007/978-3-642-95604-1_3

Cited by 5 publications

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“…98 C, p c ¼ 22.05 MPa, and r c ¼ 322 kg/m 3 . Table 2 lists volumetric properties of the liquid from 0 to 100 C [8,9]. Here, r is the mass density; a p ¼ (1/V )(qV/qT ) p , the thermal expansion coefficient; and c T ¼ (1/V )(qV/qp) T , the isothermal compressibility.…”

Section: P -V -T Data and Invariant Pointsmentioning

confidence: 99%

“…in the liquid state, where it remains almost unchanged up to 100 C [8,9] (a very shallow minimum is found near 35 C) ( Table 3). The specific heat is particularly amenable to molecular interpretation and has often been used to estimate the extent of hydrogen bonding in water [2,3].…”

mentioning

confidence: 94%

“…The vapor pressure at saturation is given in Table 3 [9]. The slope of the vapor pressure curve yields the latent heat of vaporization D g l h [8,9], which is ca. 2500 kJ/kg at the normal melting point.…”

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confidence: 99%

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Water, 1. Properties, Analysis and Hydrological Cycle

Weingärtner¹,

Franck²,

Wiegand³

et al. 2011

Ullmann's Encyclopedia of Industrial Chemistry

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The article contains sections titled: 1. Water as a Solvent 1.1. Properties of Pure Water 1.1.1. Molecular Properties 1.1.2. Hydrogen Bonding and Water Structure 1.1.3. Bulk Properties of Liquid Water 1.2. Aqueous Solutions 1.2.1. General Solvent Properties 1.2.2. Solutions of Simple Nonpolar Gases 1.2.3. Solutes with Hydrophilic Groups 1.2.4. Electrolyte Solutions 2. Water at High Pressure and Temperature 2.1. Properties of Ice 2.1.1. Thermodynamic Properties 2.1.2. Transport Properties 2.1.3. Electrolytic Properties 2.1.4. Mechanical Properties 2.2. Properties of Fluid Water 2.2.1. Thermodynamic Properties 2.2.2. Transport Properties 2.2.3. Electrolytic Properties 2.2.4. Other Physical Properties 2.3. Properties of Water Vapor 2.4. Water in the Supercritical State 3. Water Analysis 3.1. Sampling and Sample Preservation 3.2. Physicochemical and Sum Parameters 3.3. Inorganic Analysis 3.3.1. Determination of Cations 3.3.2. Anion Analysis 3.3.3. Determination of Dissolved Gases 3.3.4. Quick Test Processes 3.4. Organic Analysis 3.4.1. Spectrometric Methods 3.4.2. Gas and Liquid Chromatography 3.5. Biochemical Methods 4. Hydrological Cycle and Water Use 4.1. World Water Balance 4.2. Hydrological Cycle 4.3. Demand for Water 4.4. Source of Water Used 4.5. Water Treatment 5. Acknowledgement

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Section: P -V -T Data and Invariant Pointsmentioning

confidence: 99%

mentioning

confidence: 94%

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Water, 1. Properties, Analysis and Hydrological Cycle

Weingärtner¹,

Franck²,

Wiegand³

et al. 2011

Ullmann's Encyclopedia of Industrial Chemistry

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“…In this appendix, we calculate and estimate various parameters used in the model from the available material parameters of water [60] and nitrogen [1,61]. We want to point out that the dynamic van der Waals theory is employed to model the Leidenfrost droplets with a small set of material parameters: the molecular mass m, the energy parameter ε, the volume parameter v 0 , the coefficient C for the gradient contribution to entropy density, and the kinematic viscosity ν.…”

Section: Appendix: Materials Parametersmentioning

confidence: 99%

“…From the critical properties in Table II, we TABLE II. Parameters for water [60] and nitrogen [61]. (ii) The characteristic interfacial thickness can be calculated from the surface tension γ .…”

Section: Appendix: Materials Parametersmentioning

confidence: 99%

Hydrodynamics of Leidenfrost droplets in one-component fluids

Qian

2013

Phys. Rev. E

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Using the dynamic van der Waals theory [Phys. Rev. E 75, 036304 (2007)], we numerically investigate the hydrodynamics of Leidenfrost droplets under gravity in two dimensions. Some recent theoretical predictions and experimental observations are confirmed in our simulations. A Leidenfrost droplet larger than a critical size is shown to be unstable and break up into smaller droplets due to the Rayleigh-Taylor instability of the bottom surface of the droplet. Our simulations demonstrate that an evaporating Leidenfrost droplet changes continuously from a puddle to a circular droplet, with the droplet shape controlled by its size in comparison with a few characteristic length scales. The geometry of the vapor layer under the droplet is found to mainly depend on the droplet size and is nearly independent of the substrate temperature, as reported in a recent experimental study [Phys. Rev. Lett. 109, 074301 (2012)]. Finally, our simulations demonstrate that a Leidenfrost droplet smaller than a characteristic size takes off from the hot substrate because the levitating force due to evaporation can no longer be balanced by the weight of the droplet, as observed in a recent experimental study [Phys. Rev. Lett. 109, 034501 (2012)].

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Spectroscopy of Hydrothermal Reactions. 1. The CO₂−H₂O System and Kinetics of Urea Decomposition in an FTIR Spectroscopy Flow Reactor Cell Operable to 725 K and 335 bar

1996

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A combined microflow reactor and short-path-length spectroscopy cell along with the accompanying process controls are described to obtain real-time, in situ transmission IR spectra of reaction components of aqueous solutions up to 725 K and 335 bar. Quantitation of the spectra was required to obtain kinetics and equilibrium constants. The extinction coefficient of CO2 in H2O at 275 bar was found to increase monotonically from 1.52 × 106 at 298 K to 2.26 × 106 cm2 mol-1 at 573 K. Also, CO2 dissolved in H2O was rotationally quenched on the IR time scale below 375 K but progressed into rotational diffusion around 625 K and finally essentially free rotation above 700 K. The kinetics and pathway of hydrothermolysis of urea to CO2 and NH3 were determined directly from spectral data at 473−573 K. Good agreement was obtained between experimental and calculated concentration−time data by using a reaction model consisting of (NH2)2CO → NH4 + + OCN- and NH4 + + OCN- + H2O → CO2 + 2NH3. The Arrhenius parameters for the first-order reaction are E a = 84.2 kJ mol-1 and ln A (s-1) = 17.5, and for latter pseudo-second-order reaction are E a = 58.5 kJ mol-1 and ln A (L mol-1 s-1) = 17.1. The global rate of formation of CO2 without the kinetic model is first-order and has different Arrhenius parameters. As part of this study, the species of 0.1 m (NH4)2CO3 equilibrium were determined at 298−650 K and 275 bar. The equilibrium shifted from the hydrolyzed ionic components at lower temperature to the neutral CO2, NH3, and H2O components at higher temperature. Therefore, the (NH4)2CO3 equilibrium does not influence the kinetic model of urea above about 475 K.

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Diagrams

Cited by 5 publications

References 0 publications

Water, 1. Properties, Analysis and Hydrological Cycle

Water, 1. Properties, Analysis and Hydrological Cycle

Hydrodynamics of Leidenfrost droplets in one-component fluids

Spectroscopy of Hydrothermal Reactions. 1. The CO₂−H₂O System and Kinetics of Urea Decomposition in an FTIR Spectroscopy Flow Reactor Cell Operable to 725 K and 335 bar

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Diagrams

Cited by 5 publications

References 0 publications

Water, 1. Properties, Analysis and Hydrological Cycle

Water, 1. Properties, Analysis and Hydrological Cycle

Hydrodynamics of Leidenfrost droplets in one-component fluids

Spectroscopy of Hydrothermal Reactions. 1. The CO2−H2O System and Kinetics of Urea Decomposition in an FTIR Spectroscopy Flow Reactor Cell Operable to 725 K and 335 bar

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Spectroscopy of Hydrothermal Reactions. 1. The CO₂−H₂O System and Kinetics of Urea Decomposition in an FTIR Spectroscopy Flow Reactor Cell Operable to 725 K and 335 bar