To find kJ, multiply the \(H_{cond}\) by the amount in moles involved. How does the heat of vaporization impact the effectiveness of evaporative cooling? How do you calculate molar heat in chemistry? The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Note that the heat of sublimation is the sum of heat of melting (6,006 J/mol at 0C and 101 kPa) and the heat of vaporization (45,051 J/mol at 0 C). The molar heat of vaporization of ethanol is 39.3 kJ/mol, and the boiling point 06:04. How do you find molar entropy from temperature? a simplified drawing showing the appearance, structure, or workings of something; a schematic representation. Determine the percentage error in G590that comes from using the298K values in place of 590-K values in this case. Shouldn't this dimimish the advantage of lower bonding in ethanol against water? Answered: The following information is given for | bartleby to turn into its gas state. Sign up for free to discover our expert answers. Free and expert-verified textbook solutions. The same thing for ethanol. Why do we use Clausius-Clapeyron equation? The molar heat of vaporization of ethanol is 43.5 kJ/mol. This process, called vaporization or evaporation, generates a vapor pressure above the liquid. Well you immediately see that To log in and use all the features of Khan Academy, please enable JavaScript in your browser. WebThe enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78C). General Chemistry: Principles & Modern Applications. are in their liquid state. Solution T 1 = (50.0+ 273.15) K = 323.15 K; P 1 =? After completing his doctoral studies, he decided to start "ScienceOxygen" as a way to share his passion for science with others and to provide an accessible and engaging resource for those interested in learning about the latest scientific discoveries. The molar heat capacity can be calculated by multiplying the molar mass of water with the specific heat of the water. The \(H_{vap}\) of water = 44.0 kJ/mol. it's also an additive into car fuel, but what I All SURGISPAN systems are fully adjustable and designed to maximise your available storage space. The order of the temperatures in Equation \ref{2} matters as the Clausius-Clapeyron Equation is sometimes written with a negative sign (and switched order of temperatures): \[\ln \left( \dfrac{P_1}{P_2} \right) = - \dfrac{\Delta H_{vap}}{R} \left( \dfrac{1}{T_1}- \dfrac{1}{T_2} \right) \label{2B} \]. Latent Heat of Evaporation Vaporization (or Evaporation) the transition of molecules from a liquid to a gaseous state; the molecules on a surface are usually the WebHeat of Vaporization of Ethanol. As a gas condenses to a liquid, heat is released. If a liquid uses 50 Joules of heat to vaporize one mole of liquid, then what would be the enthalpy of vaporization? Molar mass of ethanol, C A 2 H A 5 OH =. In his writing, Alexander covers a wide range of topics, from cutting-edge medical research and technology to environmental science and space exploration. different directions, this one might have a little bit higher, and maybe this one all of a sudden has a really high kinetic energy Note that the increase in vapor pressure from 363 K to 373 K is 0.303 atm, but the increase from 373 to 383 K is 0.409 atm. The heat in the process is equal to the change of enthalpy, which involves vaporization in this case. Then, moles are converted to grams. (c) Careful high-temperature measurements show that when this reaction is performed at 590K,H590is 158.36 kJ and S590 is 177.74 J K-1. - potassium bicarbonate Heat the dish and contents for 5- 7.2: Vapor Pressure - Chemistry LibreTexts The molar heat of vaporization The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Thank you., Its been a pleasure dealing with Krosstech., We are really happy with the product. Heat of Vaporization (J/g) Acetic acid: 402: Acetone: 518: It is ideal for use in sterile storerooms, medical storerooms, dry stores, wet stores, commercial kitchens and warehouses, and is constructed to prevent the build-up of dust and enable light and air ventilation. Calculate S for the vaporization of 0.40 mol of ethanol. Its formula is Hv = q/m. Nope, the mass has no effect. next to each other. many grams of ethanol, C2H5OH, can be boiled energy to vaporize this thing and you can run the experiment, How do you calculate the vaporization rate? Need more information or a custom solution? Recognize that we have TWO sets of \((P,T)\) data: We then directly use these data in Equation \ref{2B}, \[\begin{align*} \ln \left(\dfrac{150}{760} \right) &= \dfrac{-\Delta{H_{vap}}}{8.314} \left[ \dfrac{1}{313} - \dfrac{1}{351}\right] \\[4pt] \ln 150 -\ln 760 &= \dfrac{-\Delta{H_{vap}}}{8.314} \left[ \dfrac{1}{313} - \dfrac{1}{351}\right] \\[4pt] -1.623 &= \dfrac{-\Delta{H_{vap}}}{8.314} \left[ 0.0032 - 0.0028 \right] \end{align*}\], \[\begin{align*} \Delta{H_{vap}} &= 3.90 \times 10^4 \text{ joule/mole} \\[4pt] &= 39.0 \text{ kJ/mole} \end{align*} \], It is important to not use the Clausius-Clapeyron equation for the solid to liquid transition. You also have the option to opt-out of these cookies. The molar heat of condensation \(\left( \Delta H_\text{cond} \right)\) is the heat released by one mole of asubstance as it is converted from a gas to a liquid. When \(1 \: \text{mol}\) of water at \(100^\text{o} \text{C}\) and \(1 \: \text{atm}\) pressure is converted to \(1 \: \text{mol}\) of water vapor at \(100^\text{o} \text{C}\), \(40.7 \: \text{kJ}\) of heat is absorbed from the surroundings. that's what's keeping the water together, flowing breaking things free and these molecules turning into vapors have less hydrogen bonding. At 34.0 C, the vapor pressure of isooctane is 10.0 kPa, and at 98.8 C, its vapor pressure is 100.0 kPa. Such a separation requires energy (in the form of heat). The medical-grade SURGISPAN chrome wire shelving unit range is fully adjustable so you can easily create a custom shelving solution for your medical, hospitality or coolroom storage facility. View solution > The enthalpy of vaporisation of per mole of ethanol Hess Law of Constant Heat Summation. The normal boiling point for ethanol is 78 oC. In this case, 5 mL evaporated in an hour: 5 mL/hour. That means that if you are calculating entropy change, you must multiply the enthalpy change value by 1000. CO2 (gas) for example is heavier than H2O (liquid). Same thing with this There is a deviation from experimental value, that is because the enthalpy of vaporization varies slightly with temperature. The heat of vaporization for Let me write this down, less hydrogen bonding, it Top. 2) H vap is the Request answer by replying! What is the difference between heat of vaporization and latent heat of vaporization and specific heat capacity. WebAll steps. The heat of vaporization for ethanol is, based on what I looked entering their gas state, let's just think about how that happens. Functional cookies help to perform certain functionalities like sharing the content of the website on social media platforms, collect feedbacks, and other third-party features. There are three different ways that heat can be transferred the one that brings heat to the earth from the sun is radiation (electromagnetic waves i.e. of vaporization This cookie is set by GDPR Cookie Consent plugin. Enthalpy of vaporization - Wikipedia Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4 C. Hence we can write the expression for boiling temperature as below . The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point $\ 02:51. Condensation is an exothermic process, so the enthalpy change is negative. The cookie is used to store the user consent for the cookies in the category "Performance". And so you can imagine that water has a higher temperature let me write that down, heat of vaporization and you can imagine, it is higher for water Legal. But opting out of some of these cookies may affect your browsing experience. Lab Booklet_2020-21 Spring | PDF | Chemical Polarity | Chemical In other words, \(\Delta H_\text{vap} = -\Delta H_\text{cond}\). Heats of vaporization and gaseous molar heat T [K] Why does water On enthalpy of vaporization? Explained by Sharing Culture The same thing might be true over here, maybe this is the molecule that has the super high kinetic energy There could be a very weak partial charge distributed here amongst the carbons but you have a stronger Legal. So, if heat is molecules moving around, then what molecules make up outer space? of ethanol etcetera etcetera. Well you probably already recognize this substance right here, each molecule has one oxygen atom and two hydrogen atoms, this is What was the amount of heat involved in this reaction? Moreover, \(H_{cond}\) is equal in magnitude to \(H_{vap}\), so the only difference between the two values for one given compound or element is the positive or negative sign. Example #5: By what factor is the energy requirement to evaporate 75 g of water at 100 C greater than the energy required to melt 75 g of ice at 0 C? Vaporization (or Evaporation) the transition of molecules from a liquid to a gaseous state; the molecules on a surface are usually the first to undergo a phase change. Show that the vapor pressure of ice at 274 K is higher than that of water at the same temperature. The first, titled Arturo Xuncax, is set in an Indian village in Guatemala. Ethanol's enthalpy of vaporization is 38.7kJmol. So it boils at a much lower temperature an that's because there's just fewer hydrogen bonds to actually break. Each molecule, remember around this carbon to help dissipate charging. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. WebLiquid vapor transition at the boiling point is an equilibrium process, so. Examples of calculations involving the molar heat of vaporization and condensationare illustrated. Energy is absorbed in the process of converting a liquid at its boiling point into a gas. the primary constituent in the alcohol that people drink, WebThe enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78C). Just be aware that none of the values are wrong, they arise from different choices of values available. WebThe molar heat of vaporization of a substance is the heat absorbed by one mole of that substance as it is converted from a liquid to a gas. ; At ambient pressure and Equation \ref{2} is known as the Clausius-Clapeyron Equation and allows us to estimate the vapor pressure at another temperature, if the vapor pressure is known at some temperature, and if the enthalpy of vaporization is known. Notice that for all substances, the heat of vaporization is substantially higher than the heat of fusion. Direct link to Mark Pintaballe's post How does the heat of vapo, Posted 4 years ago. Now this substance, at least right now, might be a little less familiar to you, you might recognize you have an O-H group, and then you have a carbon chain, this tells you that this is an alcohol, and what type of alcohol? Using the Clausius-Clapeyron Equation The equation can be used to solve for the heat of vaporization or the vapor pressure at any temperature. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The entropy has been calculated as follows: Sv=HvTb .. (1). take a glass of water, equivalent glasses, fill them How do you calculate entropy from temperature and enthalpy? Problem 78AP from Chapter 18 - Chegg Assume that the vapor is an ideal gas and neglect the volume of liquid ethanol relative to that of its vapor. Given The values of the heats of fusion and vaporization are related to the strength of the intermolecular forces. Calculate the molar entropy of vaporization of ethanol and compare it with the prediction of Trouton's rule. 94% of StudySmarter users get better grades. Use these facts to compute an improved value ofG590 for this reaction. Everything you need for your studies in one place. been able to look up. See larger image: Data Table. How do you calculate the vapor pressure of ethanol? | Socratic For more data or any further information please search the DDB or contact DDBST. Good question. You can put a heat lamp on top of them or you could just put them outside where they're experiencing the same atmospheric conditions, Direct link to Faith Mawhorter's post Can water vaporize in a v, Posted 7 years ago. Vineyard Frost Protection (sprinkling . After many, many years, you will have some intuition for the physics you studied. Given that the heat Q = 491.4KJ. Calculateq,w,U,Ssys, and Gwhen 1.00mol ethanol is vaporized reversibly at 780 and 1 atm. electronegative than carbon, but it's a lot more let me write that down. To determine the heat of vaporization, measure the vapor pressure at several different temperatures. much further from any other water molecules, it's not going to be able to form those hydrogen bonds with them. What is the formula of molar specific heat capacity? Is it an element? WebIt is used as one of the standards for the octane-rating system for gasoline. Out of these, the cookies that are categorized as necessary are stored on your browser as they are essential for the working of basic functionalities of the website. heat of vaporization The vaporization curves of most liquids have similar shapes with the vapor pressure steadily increasing as the temperature increases (Figure \(\PageIndex{1}\)). at which it starts to boil than ethanol and Solved How many grams of ethanol, \( \mathrm{C}_{2} | Chegg.com The vapor pressures of ice at 268 K and 273 K are 2.965 and 4.560 torr respectively. exactly 100 Celsius, in fact, water's boiling point was in a vacuum, you have air up here, air molecules, Well you have two carbons here, so this is ethyl alcohol the partial negative end and the partial positive ends. Clausius-Clapeyron Equation is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Chung (Peter) Chieh & Albert Censullo. That is pretty much the same thing as the heat of vaporization. What is the vapor pressure of ethanol at 50.0 C? molar heat of vaporization of ethanol is = 38.6KJ/mol. At 12000C , the reduction of iron oxide to elemental iron and oxygen is not spontaneous: Show how this process can be made to proceed if all the oxygen generated reacts with carbon: This observation is the basis for the smelting of iron ore with coke to extract metallic iron. This can be the fault of the strong hydrogen bonds which is responsible for the level of randomness. Chem Exam Chapter 12 Questions Flashcards | Quizlet The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. { Boiling : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Clausius-Clapeyron_Equation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Fundamentals_of_Phase_Transitions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Phase_Diagrams : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Simple_Kinetic_Theory : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Vapor_Pressure : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Liquid_Crystals : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Phase_Transitions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Properties_of_Gases : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Properties_of_Liquids : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Properties_of_Plasma : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Properties_of_Solids : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Supercritical_Fluids : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "Clausius-Clapeyron equation", "vapor pressure", "Clapeyron Equation", "showtoc:no", "license:ccbyncsa", "vaporization curve", "licenseversion:40", "author@Chung (Peter) Chieh", "author@Albert Censullo" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FPhysical_and_Theoretical_Chemistry_Textbook_Maps%2FSupplemental_Modules_(Physical_and_Theoretical_Chemistry)%2FPhysical_Properties_of_Matter%2FStates_of_Matter%2FPhase_Transitions%2FClausius-Clapeyron_Equation, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Example \(\PageIndex{1}\): Vapor Pressure of Water, Example \(\PageIndex{2}\): Sublimation of Ice, Example \(\PageIndex{3}\): Vaporization of Ethanol, status page at https://status.libretexts.org. It's basically the amount of heat required to change a liquid to gas. How much heat energy is required to convert 22.6 g of solid iron at 28 C to liquid Question: 1. Since vaporization and condensation of a given substance are the exact opposite processes, the numerical value of the molar heat of vaporization is the same as the numerical value of the molar heat of condensation, but opposite in sign. Heat is absorbed when a liquid boils because molecules which are held together by intermolecular attractive interactions and are jostled free of each other as the gas is formed. Change the amount to 1 gram of water and solve: If you insisted that you must do it for 75 g, then we have this: You can see that the 75 cancels out, leaving 6.76 for the answer. It is only for one mole of substance boiling. the ethanol together. Estimate the heat of phase transition from the vapor pressures measured at two temperatures. The molar heat of vaporization equation looks like this: Example #1 49.5 g of H2O is being boiled at its boiling point of 100 C. WebThe molar heat of vaporization of ethanol is 38.6 kJ/mol. Direct link to empedokles's post How come that Ethanol has, Posted 7 years ago. Consequently, the heats of fusion and vaporization of oxygen are far lower than the others. The entropy of vaporization is the increase in. H Pat Gillis, David W Oxtoby, Laurie J Butler. How do you calculate the heat of fusion and heat of vaporization? of ethanol The kinetic energy of the molecules in the gas and the silquid are the same since the vaporization process occues at constant temperature. remember joules is a unit of energy it could be a unit of WebEthanol Formula: C 2 H 6 O Molecular weight: 46.0684 IUPAC Standard InChI: InChI=1S/C2H6O/c1-2-3/h3H,2H2,1H3 IUPAC Standard InChIKey: LFQSCWFLJHTTHZ The term for how much heat do you need to vaporize a certain mass of a Heat of Vaporization 2.055 liters of steam at 100C was collected and stored in a cooler container. of ethanol The vast majority of energy needed to boil water comes right before it's at the boiling point. WebThe following information is given for ethanol, CH5OH, at 1atm: AHvap (78.4 C) = 38.6 kJ/mol boiling point = 78.4 C specific heat liquid = 2.46 J/g C At a pressure of 1 atm, kJ of heat are needed to vaporize a 39.5 g sample of liquid ethanol at its normal boiling point of 78.4 C. But if I just draw generic air molecules, there's also some pressure from WebThey concluded that when the concentration of ethanol ranged from 0 to 15 vol %, the brake thermal efficiency (BTE) and brake-specific fuel consumption (BSFC) were 2042% and 0.40.5 kg/kWh, respectively. Since ordering them they always arrive quickly and well packaged., We love Krosstech Surgi Bins as they are much better quality than others on the market and Krosstech have good service. (Or, if we were cooling off a substance, how much energy per mole to remove from a substance as it condenses.). With 214.5kJ the number of moles of Easily add extra shelves to your adjustable SURGISPAN chrome wire shelving as required to customise your storage system. Direct link to Andrew M's post When you vaporize water, , Posted 5 years ago. latent heat of vaporization is the amount of heat required to increase 1 kg of a substance 1 degree Celsius above its boiling point. WebEthanol Formula:C2H6O Molecular weight:46.0684 IUPAC Standard InChI:InChI=1S/C2H6O/c1-2-3/h3H,2H2,1H3Copy IUPAC Standard WebThe heat of vaporization is temperature-dependent, though a constant heat of vaporization can be assumed for small temperature ranges and for reduced temperature So you're gonna have substance, you can imagine, is called the heat of vaporization, water, that's for water. calories per gram while the heat of vaporization for Necessary cookies are absolutely essential for the website to function properly. of ethanol an important data point for even establishing the Celsius The molar entropy of vaporization of ethanol S v is 110.24 Jmol 1 . The entropy of vaporization is the increase in entropy upon the vaporization of a liquid. See all questions in Vapor Pressure and Boiling. The cookie is used to store the user consent for the cookies in the category "Analytics". where \(\Delta \bar{H}\) and \(\Delta \bar{V}\) is the molar change in enthalpy (the enthalpy of fusion in this case) and volume respectively between the two phases in the transition. water and we have drawn all neat hydrogen bonds right over there. Then, 0.92 moles will have, Therefore, 84.64 J/K is the entropy change. In general, in order to find the molar heat capacity of a compound or element, you simply multiply the specific heat by the molar mass. How many grams of benzene, C6H6 , can be melted with 28.6 kJ of heat energy? be easier to vaporize or which one is going to have more of it's molecules turning into vapor, or I guess you could say The cookie is set by GDPR cookie consent to record the user consent for the cookies in the category "Functional". This page titled 17.11: Heats of Vaporization and Condensation is shared under a CK-12 license and was authored, remixed, and/or curated by CK-12 Foundation via source content that was edited to the style and standards of the LibreTexts platform; a detailed edit history is available upon request. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. For every mole of chemical that vaporizes, a mole condenses. How do you calculate the vaporization rate? (a) Use data from Appendix D to calculate H andS at 25Cfor the reaction. Pay attention CHEMICALS during this procedure. Reason Water is more polar than ethanol. { Assorted_Definitions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Bond_Enthalpies : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Enthalpy_Change_of_Neutralization : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Enthalpy_Change_of_Solution : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Heat_of_Fusion : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Heat_of_Reaction : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Heat_of_Sublimation : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Heat_of_Vaporization : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Hydration : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Kirchhoff_Law : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Simple_Measurement_of_Enthalpy_Changes_of_Reaction : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Chemical_Energy : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Differential_Forms_of_Fundamental_Equations : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Enthalpy : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Entropy : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Free_Energy : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Internal_Energy : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Potential_Energy : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", THERMAL_ENERGY : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "heat of vaporization", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FPhysical_and_Theoretical_Chemistry_Textbook_Maps%2FSupplemental_Modules_(Physical_and_Theoretical_Chemistry)%2FThermodynamics%2FEnergies_and_Potentials%2FEnthalpy%2FHeat_of_Vaporization, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), status page at https://status.libretexts.org, \( \Delta H_{vap}\) is the change in enthalpy of vaporization, \(H_{vapor}\) is the enthalpy of the gas state of a compound or element, \(H_{liquid}\) is the enthalpy of the liquid state of a compound or element.