Sensible Heat and Enthalpy Calculations

Similar documents
Sensible Heat and Enthalpy Calculations

Name: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry

Types of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy

MME 2010 METALLURGICAL THERMODYNAMICS II. Fundamentals of Thermodynamics for Systems of Constant Composition

Chapter 3 PROPERTIES OF PURE SUBSTANCES. Thermodynamics: An Engineering Approach, 6 th Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2008

Ch 9 Practice Problems

Chapter 17: Spontaneity, Entropy, and Free Energy

Temperature C. Heat Added (Joules)

Ch. 17 Thermochemistry

Chemistry Heat Review. Heat: Temperature: Enthalpy: Calorimetry: Activation energy:

The Nature of Energy Energy is the ability to do work or produce Heat, q or Q, is ; flows due to temperature differences (always to )

Enthalpies of Reaction

Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes

17.4 Calculating Heats Essential Understanding Heats of reaction can be calculated when it is difficult or

Chapter 5 Thermochemistry

Warm up. 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]?

Introduction to Chemical Engineering Thermodynamics. Chapter 4. KFUPM Housam Binous CHE 303

Question 4. Calculate q when 0.10 g of ice is cooled from 10.ºC to -75ºC. (c ice = J/g ºC) A) -18 J B) -14 J C) -8.5 J D) + 14 J E) +18 J 5-4

1. III only 2. II, III. 3. II only. 4. I only 5. I, III. 6. I, II, III correct

Energy. Different types of energy exist (heat, potential, kinetic, chemical, nuclear etc.)

Chapter 12 Intermolecular Forces of Attraction

Chapter Eighteen. Thermodynamics

THE ENERGY OF THE UNIVERSE IS CONSTANT.

Heat. Heat Terminology 04/12/2017. System Definitions. System Definitions

So far changes in the state of systems that occur within the restrictions of the first law of thermodynamics were considered:

= (25.0 g)(0.137 J/g C)[61.2 C - (-31.4 C)] = 317 J (= kj)

Energy and Chemical Change

Chemical reaction equilibria

10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics

Chemistry Chapter 16. Reaction Energy

Exam 4, Enthalpy and Gases

Chemistry 123: Physical and Organic Chemistry Topic 2: Thermochemistry

Slide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c

Thermodynamics. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Energy and Chemical Change

Chapter 8 Thermochemistry: Chemical Energy

To calculate heat (q) for a given temperature change: heat (q) = (specific heat) (mass) ( T) where T = T f T i

Name: Class: Date: ID: A

Section 9: Thermodynamics and Energy

The Nature of Energy. Chapter Six: Kinetic vs. Potential Energy. Energy and Work. Temperature vs. Heat

10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics

ENTHALPY CHANGE CHAPTER 4

Entropy, Free Energy, and Equilibrium

Advanced Chemistry Practice Problems

AAE THERMOCHEMISTRY BASICS

Exothermic process is any process that gives off heat transfers thermal energy from the system to the surroundings. H 2 O (l) + energy

Ch 17 Free Energy and Thermodynamics - Spontaneity of Reaction

CP Chapter 17 Thermochemistry

Chapter 17 Thermochemistry

Chapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics

Thermodynamics of solids 5. Unary systems. Kwangheon Park Kyung Hee University Department of Nuclear Engineering

Thermochemistry-Part 1

CHEMISTRY 109 #25 - REVIEW

2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.

Selected Questions on Chapter 5 Thermochemistry

Chapter 11 Spontaneous Change and Equilibrium

Thermochemistry: Heat and Chemical Change

General Chemistry 1 CHM201 Unit 3 Practice Test

Ch. 6 Enthalpy Changes

Thermodynamics. Thermodynamics of Chemical Reactions. Enthalpy change

Enthalpy. Enthalpy. Enthalpy. Enthalpy. E = q + w. Internal Energy at Constant Volume SYSTEM. heat transfer in (endothermic), +q

Chemical Thermodynamics

Energy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy

Mr Chiasson Advanced Chemistry 12 / Chemistry 12 1 Unit B: Thermochemical Changes

Class work on Calorimetry. January 11 and 12, 2011

2. If the volume of a container holding a gas is reduced, what will happen to the presure within the container?

Homework Problem Set 6 Solutions

Chemistry Lab Fairfax High School Invitational January 7, Team Number: High School: Team Members Names:

THERMOCHEMISTRY & DEFINITIONS

Energy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy

Thermochemistry HW. PSI Chemistry

Learning Check. How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C?

Chemical Thermodynamics. Chemical Thermodynamics. Changes of State. Chemical Thermodynamics. State Functions. State Functions 11/25/13

Homework 11 - Second Law & Free Energy

Energy Relationships in Chemical Reactions

Thermochemistry Chapter 8

Module Tag CHE_P10_M6

Thermochemistry. Energy and Chemical Change

Name Date Class THE FLOW OF ENERGY HEAT AND WORK

Unit 7 Thermochemistry Chemistry 020, R. R. Martin

Chapter 6 Thermochemistry 許富銀

Lecture 4. The Second Law of Thermodynamics

Name Date Class THERMOCHEMISTRY

Spontaneity, Entropy, and Free Energy

1. Fill in the blanks with the following: kinetic, potential, chemical, thermal. One word will be used twice.

Chapter 3 PROPERTIES OF PURE SUBSTANCES

Name Class Date. As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings.

Please pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED

Chapter 8. Thermochemistry

Thermochemistry. Energy and Chemical Change

Thermochemistry: Energy Flow and Chemical Reactions

Thermodynamics: Entropy, Free Energy, and Equilibrium

Energy Transformations

Thermochemistry. Section The flow of energy

CHEM Exam 2 - October 11, INFORMATION PAGE (Use for reference and for scratch paper)

TODAY 0. Why H = q (if p ext =p=constant and no useful work) 1. Constant Pressure Heat Capacity (what we usually use)

General Chemistry I. Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University. Module 4: Chemical Thermodynamics

Chapter 5 Thermochemistry. 許富銀 ( Hsu Fu-Yin)

Chapter 11. Thermochemistry: Heat & Chemical Change

Chemistry Grade : 11 Term-3/Final Exam Revision Sheet

Transcription:

Sensible Heat and Enthalpy Calculations

Sensible Heat - The amount of heat that must be added when a substance undergoes a change in temperature from 298 K to an elevated temperature without a change in phase T H = n 298 T C P dt = 298 a + bt + c T 2 = at + b 2 T2 c T a 298 + b 2 2982 c 298 constant = A H = H T H 298 = A + BT + CT 2 + D T Enthalpy increment equation B = a, C = b, D = C 2 Sensible heat at any temperature can be calculated by replacing that temperature in the enthalpy increment equation Enthalpy increment equation can also be used to calculate enthalpy change between any two temperatures H = H T2 H T1 = H T2 H 298 (H T1 H 298 )

Enthalpy Increments with Phase Changes Seperate the enthalpy increments to steps when there is a phase change during heating of a substance, for example melting: 298 to T m Heat supplied increases the temperature of the solid phase ΔH = H T H 298 = 298 T CP(s) dt at T m Each mole of substance absorbs ΔH m, latent heat of fusion or enthalpy of melting ΔH = nδh m T m to T v Heat supplied increases the temperature of the liquid phase ΔH = H T H 298 = Tm 298 C P s dt + H m + T Tm C P l dt

Enthalpy Increments with Phase Changes Seperate the enthalpy increments to steps when there is a phase change during heating of a substance, for example melting: at T v Each mole of liquid substance absorbs ΔH V, latent heat of evaporation or enthalpy of evaporation ΔH = nδh v T v to T Heat supplied increases the temperature of the gas phase ΔH = H T H 298 = Tm 298 C P s dt + H m + Tv Tm C P l dt + H v + T Tv C P g dt Allotropic transformations are incorporated into enthalpy computations the same way as latent heats of melting and evaporation

Allotropes are different structural modifications of an element. The atoms of the element are bonded together in a different form Allotropy refers only to different forms of an element within the same phase For example there are three allotropic forms of solid iron at atmospheric pressure: alpha iron (α) ferrite, gamma iron (γ) austenite, and delta iron ΔH = H 1500 H 298 = 1183 298 C P s(α iron) dt + H A + 1500 1183 C P s(γ iron) dt

Enthalpy increment equations incorporate phase transformations Example Calculate the heat required to heat 500 gram of zinc from room temperature to 1500 K a) Using heat capacities b) Using enthalpy increment equations C P (s) = 22.4 + 0.01005*T J/mol K C P (l) = 31.4 J/mol K C P (g) = 20.76 J/mol K ΔH m = 7388 J/mol at 693 K ΔH v = 115366 J/mol at 1180 K (H T -H 298 ) Zn(g) = 124376+20.76*T J/m

Phase transformations result in the coexistence of two phases Gibbs phase rule requires that a two phase system consisting of a single species is univariant and its state is determined by specification of one intensive property: T Clapeyron equation helps calculate the latent heats of transformation H αβ When Clapeyron equation is applied to the vaporization of a pure liquid, dp sat dt dp sat dt = Hαβ T V αβ H αβ = T V αβ dpsat dt is the slope of the vapor pressure-temperature curve at a temperature T, V αβ is the difference between molar volumes of saturated vapor and saturated liquid and H αβ is the latent heat of vaporization Latent heats may be measured calorimetrically and experimental values at selected temperature are available for many substances

Estimation of the latent heats, especially latent heats of vaporization is possible by approximate methods: H n RT n 10 Trouton s rule gives rough estimates of latent heats of vaporization for pure liquids at their normal boiling points H n = 1.092(ln P c 1.013) RT n 0.930 T rn Riedel s equation is an accurate approximation of latent heat of vaporization where Pc is the critical pressure, T rn is the reduced temperature or T n /T c For example, applied to water it gives: H n RT n = 1.092(ln 220.55 1.013) 0.930 0.577 = 13.56 H n = 13.56 8.314 373.15 = 42.065 J/m 3.4% higher than real

Estimates of the latent heat of vaporization of a pure liquid at any temperature from the known value at a single temperature is derived from Riedel s equation by Watson: H 2 H 1 = 1 T r2 1 T r1 0.38 Example Estimate the latent heat of vaporization for water at 300 C, given that its latent heat of vaporization at 100 C is 2257 J/g T r1 = T 1 T c = 373.15 647.1 = 0.577 T r2 = T 1 T c = 573.15 647.1 = 0.886 H 2 = 2257 1 0.886 H 1 1 0.577 0.38 = 2257 0.270 0.38 = 1371 J/g The value given in steam tables is 1406 J/g

One can determine the amount of heated material through division of the amount of heat given by the heat required per mole Example What is the amount of ice cube at 0.0 C added to 500 ml of tea at 20.0 C to make ice tea if the temperature of the tea when the ice cube has just melted is 11.0 C? Take the density of water (and ice tea) constant = 1.00 g/ml over the range 0 C 20 C C P (l) = 75.312 J/(mol.K) C P (s) = 37.116 J/(mol.K), ΔH m = 6.01 kj/mol.

Superheating or boiling delay is the phenomenon by which a liquid is heated to a temperature higher than its boiling point Superheating is achieved by heating a homogeneous substance in a clean container, free of nucleation sites Nucleation free energy Heterogeneous nucleation around a surface pit

Supercooling or freezing delay is the phenomenon by which a liquid is cooled below its freezing point A liquid below its freezing point will crystallize in the presence of a seed crystal around which a crystal structure can form creating a solid Liquid phase can be maintained while cooling to the temperature at which crystal homogeneous nucleation occurs

Enthalpy change for transformations of superheated and supercooled matter A solid at a higher temperature T m than its melting point is a superheated solid. Enthalpy change for the transformation of superheated solid to liquid phase is ΔH m A liquid at a lower temperature T m than its freezing point is a supercooled liquid. Enthalpy change for the transformation of supercooled liquid to solid phase is ΔH m T m is reversible melting point L H T -H 298 ΔH m ΔH m ΔH m S T m T m T m

Enthalpy change for transformations of superheated and supercooled matter Enthalpy change through ABC and ADC paths are equal since enthalpy is a state function ΔH m can be calculated using the known enthalpy change values along these paths H T -H 298 H ABC = H ADC H AB + H BC = H m + H AD + H DC = H m = H m + B A T m Tm T m Tm C D T m Tm ΔH m C P (l) dt C P (s) dt + H m C P (l) dt T m Tm C P (s) dt T m T m

ΔH solidification = - ΔH m H m = H m + H v = H v + T m Tm T v Tv C P l C P (s) dt C P g C P (l) dt ΔH condensation = - ΔH v Example Derive an equation for the enthalpy of melting for lead as a function of temperature C P (s) = 24.36 + 0.00796*T J/mol K C P (l) = 28.46 J/mol K T m = 600K T m ΔH m = 5128 J/mole H m = H m + C P l C P (s) dt Enthalpy of melting at any temperature T is ΔH m (T) = ΔH m Tm Hence H m (T) = 5128 + T 600 (28.46 24.36 0.00796 T) dt H m T = 4101 + 4.1 T 0.00398 T 2 J/mole

When a superheated material is kept in an adiabatic enclosure, fraction of the liquid may be determined from the ratio of extra heat supplied H x to enthalpy of melting L H T -H 298 ΔH x S T m T m X l = H x Hm

When a supercooled material is kept in an adiabatic enclosure, fraction of the solid may be determined from the ratio of extra heat H x taken from the liquid below its melting point to the enthalpy of melting L H T -H 298 ΔH x S T m T m X s = H x Hm

Example Calculate the enthalpy of solidification for supercooled liquid zinc at 400 C. Find out the fraction of solid zinc if the supercooled liquid is allowed to solidify adiabatically C P (s) = 22.4 + 0.01005*T J/mol K C P (l) = 31.4 J/mol K T m T m = 693 K H ΔH m = 7388 J/mole m = H m + (C P l C P s ) dt H m = 7388 + L Tm 673 H m = 7345 J/mole (C P l C P s ) dt 693 C P l C P s = 9 0.01005 T H T -H 298 ΔH x X s = H x Hm S 673 693

Heat Effects of Chemical Reactions So far change of state of a system through change in P,V or T by heat or work was considered The state of a system can also change if chemical identity of constituents are altered by chemical reaction Chemical reactions are accompanied either by the transfer of heat or by change in temperature during the process, in some cases by both Heat and temperature changes are due to the differences in molecular structure of the products and reactants A reaction is exothermic if it supplies heat to the surroundings (-ΔH) Reactions that require heat from the surroundings are endothermic (+ΔH) The reaction aa + bb yields cc + dd may be carried out in many different conditions so each reaction carried out in a specific condition is accompanied by a different heat effect

Tabulation of all heat effects for all possible reactions is impossible Calculation of all heat effects is possible from data for reactions carried out in a standard way Example Consider formation of CO 2 from C and O 2 ac + bo 2 yields cco2 The standard heat of reaction is defined as the enthalpy change when a moles of C and b moles of O 2 in their standard states at temperature T react to form c moles of CO 2 in its standard state at the same temperature T Only enthalpy of formation of compounds can be measured, standard enthalpy of formation of pure elements in their standard states is zero ΔH CO2 = f(p,t) Enthalpy of formations are tabulated at 298 K under standard atmospheric pressure (101.33 kpa): ΔH o 298(CO 2 (g)) = -393690 J/mole at 298 K standard enthalpy of formation Standard state for gases: The pure substance in the ideal gas state at 1 atm For Liquids and solids: The real pure liquid or solid at 1 atm pressure

Enthalpy change of any reaction can be calculated using Hess law H rxn = H products - H reactants Example Compound formation from elements ac + bo 2 yields cco2 Hess law states that enthalpy change accompanying a chemical reaction is the same whether it takes place in one or several stages since enthalpy is a state function It is useful in calculating the unknown enthalpy change of a reaction using known enthalpy change at standard conditions ac + bo 2 500 K, 1 a t m cco2 H rxn H rxn = H 1 + H std + H 2 H 1 H 2 298 K, 1 a t m ac + bo 2 cco2 H

Example What is the change in internal energy and enthalpy for the decomposition of CaCO 3 to CaO and CO 2 at 25 0 C and 1 atm.? CaCO 3(S) CaO (S) + CO 2 (g) H rxn = H products - H reactants H rxn = ((-635.5) + (-394)) - (-1207) = + 571 KJ H = U + P V, P V = n RT, Therefore H = U + n RT U = H - n RT n = moles of gaseous products moles of gaseous reactants (n = 1 0) = 1 U = (+571) - ((1) x 0.00831 x (25 + 273)) = +571 2.48 = 569 KJ

Example 1 ton of limestone (CaCO3) is calcined at 727 C according to reaction CaCO3(s) = CaO(s) + CO2(g) 180 kg of coke containing 100% C was used as fuel. If limestone, coke and air enter the furnace at room temperature, calculate a) The heat required for calcination b) The heat available when coke is burned with air (21% O2, 79% N2) to yield an exhaust gas (CO2-N2) at 727 C c) Thermal efficiency (ratio of the required heat to available heat of the process CaCO3(s) ΔH298=-1207 kj/mole Cp=104.57+0.02193T -2595000/T2 J/molK C(s) Cp=16.87+0.00477T -854000/T2 J/molK CaO ΔH298=-635.5 kj/mole, Cp=49.95+0.00489T -352000/T2 J/molK O2(g) Cp=29.97+0.00419T-167000/T2 J/moleK N2(g) Cp=27.88+0.00427T J/molK (HT-H298)= -8502+27.88T+0.00213T2 CO2(g) Cp=22.24+0.0598T -349900/T2 J/molK

Example 1 ton of limestone (CaCO3) is calcined at 727 C according to reaction CaCO3(s) = CaO(s) + CO2(g) 180 kg of coke containing 100% C was used as fuel. If limestone, coke and air enter the furnace at room temperature, calculate a) The heat required for calcination CaCO3(s) ΔH298=-1207 kj/mole Cp=104.57+0.02193T -2595000/T2 J/molK C(s) Cp=16.87+0.00477T -854000/T2 J/molK CaO ΔH298=-635.5 kj/mole, Cp=49.95+0.00489T -352000/T2 J/molK O2(g) Cp=29.97+0.00419T-167000/T2 J/moleK N2(g) Cp=27.88+0.00427T J/molK (HT-H298)= -8502+27.88T+0.00213T2 CO2(g) Cp=22.24+0.0598T -349900/T2 J/molK

Example 1 ton of limestone (CaCO3) is calcined at 727 C according to reaction CaCO3(s) = CaO(s) + CO2(g) 180 kg of coke containing 100% C was used as fuel. If limestone, coke and air enter the furnace at room temperature, calculate b) The heat available when coke is burned with air (21% O2, 79% N2) to yield an exhaust gas (CO2-N2) at 727 C c) Thermal efficiency (ratio of the required heat to available heat of the process CaCO3(s) ΔH298=-1207 kj/mole Cp=104.57+0.02193T -2595000/T2 J/molK C(s) Cp=16.87+0.00477T -854000/T2 J/molK CaO ΔH298=-635.5 kj/mole, Cp=49.95+0.00489T -352000/T2 J/molK O2(g) Cp=29.97+0.00419T-167000/T2 J/moleK N2(g) Cp=27.88+0.00427T J/molK (HT-H298)= -8502+27.88T+0.00213T2 CO2(g) Cp=22.24+0.0598T -349900/T2 J/molK

2024 © sciencedocbox.com Privacy Policy | Terms of Service | Feedback