Lecture05 Week 02
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The document discusses using enthalpy vs composition plots, also known as Ponchon-Savarit plots, to obtain information about separation problems involving energy balances based on enthalpy. It explains that these plots show three phases - solid, liquid, and vapor - with temperature represented by tie lines. Points between saturated lines represent two-phase systems, and azeotropes are indicated by vertical isotherms.
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The Antoine equation often is used to describe vapor pressures: lnP = A B /(T + C) . For
temperatures near the normal boiling point:
a. Derive an expression that gives the behavior of Hvap as a function of temperature which is
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The Antoine equation is a mathematical expression of the relation between the vapour pressure
and the temperturer of pure substances. The equation was first proposed by Ch. Antoine, a french
researcher, in 1888. The basic form of the equation is:
lnP = A - B / ( T + C )
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where: P is the absolute vapor pressure of a substance
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specific constants.
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273.150 < T 373.150: A = 16.5699, B = 3984.92, C = 39.724
373.150 < T 647.096: A = 16.7285, B = 4169.84, C = 28.665
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that supercritical water behaves like an ideal gas. Now if we define Tc = 647.096 K, we can
write
P(T Tc) = Antoine(T)
P(T > Tc) = 235.88 (T Tc) + Antoine(Tc)
Hence, the behaviour of delta hvap as a function of temperature which is termodynamically
consistent with the the antoine equation is derived ..
chapter31.ppt
This document discusses chemical equilibrium. It begins by explaining that many chemical reactions do not go to completion, but rather reach a state of dynamic equilibrium where the rates of the forward and reverse reactions are equal. This equilibrium state occurs when the concentrations of reactants and products remain constant over time.
It then introduces the equilibrium constant expression (K), which relates the concentrations or pressures of products and reactants at equilibrium. The value of K is unique to a particular chemical reaction at a given temperature. Examples are provided to demonstrate how K is calculated from experimental equilibrium concentrations. The summary concludes by noting that K can be expressed in terms of either molar concentrations (Kc) or partial pressures (Kp), and the relationship between these two expressions
Chapter 4 Energy Analysis of Closed System.pdf
This chapter discusses energy analysis of closed systems. It examines moving boundary work in reciprocating devices like engines. The first law of thermodynamics states the principle of conservation of energy for closed systems. The chapter develops the general energy balance applied to closed systems and defines specific heats at constant volume and pressure. It relates specific heats to changes in internal energy and enthalpy of ideal gases and incompressible substances. Methods to solve energy balance problems involving heat, work, and closed systems are presented.
1649011617114008.hhgggggggggfffffffffffffff
This document provides an overview of properties of pure substances and phase change processes. It introduces key concepts such as pure substances, phases of matter, phase change diagrams, property tables, and the ideal gas law. Specific topics covered include saturated liquids and vapors, phase change temperatures and pressures, property diagrams, determining properties from tables, and using the ideal gas equation of state to model real gases. The document uses water as an example pure substance to illustrate these concepts through diagrams and examples.
VLE VAPOR LIQUID EQUILIBRIUM - Introduction
This document discusses vapor/liquid equilibrium (VLE) and provides models for predicting VLE using simple models like Raoult's law and Henry's law. It defines key terms like mass fraction, mole fraction, molar concentration. Duhem's theorem is introduced which states that the equilibrium state is determined by fixing any two independent variables for a closed system. Simple calculations are shown for using Raoult's law to determine the bubble point and dew point temperatures and pressures of a binary system from its phase compositions or known temperature. P-x-y and T-x-y diagrams are used to illustrate the VLE behavior between the phases.
Chem II Review 2.pptx
This document summarizes key concepts in chemistry including:
1) Equilibrium occurs when forward and reverse reaction rates are equal, and concentrations remain constant. The equilibrium constant K relates concentrations.
2) Kc and Kp describe equilibrium using concentrations or pressures. They are related by Kp = Kc(RT)Δn.
3) Le Chatelier's principle states a system at equilibrium will adjust to counteract stresses like concentration changes.
4) Acid-base equilibria involve proton transfer. Water autoionizes and pH relates to [H+]. Buffers resist pH changes.
heat capacity of sitric acid0c96051e8eb63eea58000000
This document summarizes thermodynamic properties of the citric acid-water binary system determined through various experimental methods. Key findings include:
- The phase diagram exhibits eutectic and peritectic behavior with solid-liquid and vapor-liquid equilibria measured.
- Enthalpies of formation for citric acid monohydrate, solution, transition, and vaporization were determined via calorimetry and vapor pressure measurements.
- Specific heat capacity and solubility data were also collected to characterize the phase behavior and thermodynamic functions of citric acid and its monohydrate over a range of temperatures.
Problem and solution i ph o 20
1) The boiling points of liquids A and B were determined to be 77°C and 100°C respectively based on their vapor pressure ratios given in the table.
2) The temperature t1 was found to be 67°C, which is the common boiling point of liquids A and B where the total vapor pressure of their mixture equals atmospheric pressure.
3) At t1, the individual vapor pressures of liquids A and B were calculated to be 0.734p0 and 0.267p0 respectively, with their ratio matching the given molecular mass ratio.
slides-enbal-2up.pdf
1. The document discusses energy balances for chemical reactors, deriving equations to determine reactor temperature based on heat and work terms.
2. Special cases are considered, including constant pressure/volume reactors and incompressible fluids. Equations are presented for batch reactors under these conditions.
3. A example problem compares constant pressure and volume reactors for an irreversible decomposition reaction, showing the constant volume reactor proceeds faster due to less work required.
General Chemistry 2- Chemical Equilibirum
This document discusses chemical equilibrium. It defines chemical equilibrium as a state where the forward and reverse reactions of a chemical reaction are proceeding at the same rate, such that the concentrations of reactants and products remain constant. It introduces key concepts such as the equilibrium constant expression, how equilibrium can be approached from both directions, and Le Châtelier's principle which states that systems at equilibrium will shift in response to changes in conditions to counteract the effect of those changes. Examples of equilibrium calculations and how equilibrium is impacted by changes in conditions such as concentration, pressure and temperature are provided.
Soave1972
This document proposes a modification to the Redlich-Kwong equation of state by making the temperature-dependent parameter a(T) instead of a constant. This improves the equation's ability to model vapor pressures of pure substances and phase equilibria of mixtures. The modified equation represents vapor pressure data for hydrocarbons more accurately than the original equation. When combined with the original Redlich-Kwong mixing rules, the modified equation can also predict vapor-liquid equilibrium for mixtures of nonpolar fluids like hydrocarbons, with some limitations for hydrogen-containing mixtures.
TEMPERATURE AND PRESSURE EFFECTS ON CHEMIOCAL RESCTION
1) Temperature and pressure affect reaction equilibrium, rates, and product distribution. The optimal temperature progression minimizes reactor size by maintaining the maximum rate.
2) For reversible reactions, the equilibrium constant and conversion vary with temperature based on thermodynamics. Irreversible reactions proceed best at the maximum temperature allowed.
3) Reactor designs aim to approximate the optimal temperature-conversion profile. This involves determining heat effects and using techniques like heat exchange, multi-staging, and recycle to control temperatures.
Elizabeth Towle Batch Distillation of Ethanol Design
This document is a project report analyzing a batch distillation process to separate ethanol and water. Theoretical calculations using the Rayleigh equation and Aspen simulation software are compared to experimental data. The Rayleigh equation best matches the average distillate composition and total distillate volume, while Aspen POLYSRK most accurately predicts distillation time. Varying the column diameter and reflux ratio in Aspen affects distillation parameters like average distillate composition and time. Overall, the theoretical models provide reasonable approximations of the experimental batch distillation, validating it as a basis for process design.
1 s2.0-0378381289800755fazeremcasa-main
The document describes combining the UNIWAALS equation of state with an algorithm for calculating simultaneous chemical and phase equilibria (CPE). This allows CPE calculations for reactive systems containing gases, polar compounds, or both over a broad range of temperatures and pressures using a single thermodynamic model. Examples are given applying the new procedure to different multicomponent reaction systems. The results show good agreement with previous calculations using a different equation of state, demonstrating the capability of performing CPE calculations with UNIWAALS.
Enthalpy of vaporization of liquid
Seven students presented a detailed approach on thermodynamics. They restated the first law of thermodynamics and defined enthalpy. Common enthalpy changes were discussed, including enthalpy of vaporization. The characteristics and physical model of enthalpy of vaporization were described. An experiment was conducted to determine the enthalpy of vaporization of water at different pressures using a Clausius-Clapeyron analysis of temperature and pressure readings. The results were within 5% of accepted values. Applications of enthalpy of vaporization include steam power generation and distillation.
Q913 rfp w3 lec 10
This document provides an overview of key concepts for performing phase equilibrium calculations on reservoir fluids, including:
1) Cubic equations of state and properties required for components in mixtures like critical temperature, pressure, and acentric factor.
2) Calculating these properties for hydrocarbon components and lumping heavier fractions into pseudocomponents.
3) Using equations of state to relate fugacity coefficients to vapor-liquid equilibrium and calculate K-factors for flash calculations.
themodyamic paper
1. A new static analytical apparatus was designed for measuring vapour pressure and vapor-liquid equilibrium with an internal stirrer and view windows.
2. Vapour pressure data was collected for R245fa and R600a, and vapor-liquid equilibrium data was collected for the R600a + R245fa system, from 293.15K to 343.88K.
3. The data was correlated using theoretical models and showed good agreement with literature values, demonstrating the apparatus provides reliable measurements.
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Lecture05 Week 02
- 2. Enthalpy vs. Composition – Ponchon-Savarit Plot
- 9. Enthalpy vs. Composition – Bubble Point Temperature 82.2 o C
- 10. Enthalpy vs. Composition – 1 st Bubble Composition
- 11. Enthalpy vs. Composition – Dew Point Temperature 94.8 o C
- 12. Enthalpy vs. Composition – Last Liquid Drop Composition
- 14. Enthalpy vs. Composition – Enthalpy Determination 425 295 90
- 17. Other Equilibrium Relationships – Distribution Coefficient
- 22. T bp = - 9.5 o C
- 28. Other Equilibrium Relationships – DePriester Equation
- 29. Other Equilibrium Relationships – Mole Fraction – Vapor Pressure Relationship
- 30. Other Equilibrium Relationships – Distribution Coefficient – Vapor Pressure Relationship
- 31. Other Equilibrium Relationships – Relative Volatility
- 32. Other Equilibrium Relationships – Relative Volatility