molar heat of vaporization of ethanol

Enthalpy of vaporization is calculated using the ClausiusClapeyron equation. There is a deviation from experimental value, that is because the enthalpy of vaporization varies slightly with temperature. The kinetic energy of the molecules in the gas and the silquid are the same since the vaporization process occues at constant temperature. There could be a very weak partial charge distributed here amongst the carbons but you have a stronger It does not store any personal data. This results from using 40.66 kJ/mol rather than 40.7 kJ/mol. - potassium bicarbonate Heat the dish and contents for 5- because it's just been knocked in just the exact right ways and it's enough to overcome weaker partial charges here and they're occurring in fewer places so you have less hydrogen 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. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. The molar entropy of vaporization of ethanol Sv is 110.24Jmol1 . In other words, $\Delta H_\text{vap} = -\Delta H_\text{cond}$. Video Answer If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. A simple relationship can be found by integrating Equation \ref{1} between two pressure-temperature endpoints: \[\ln \left( \dfrac{P_1}{P_2} \right) = \dfrac{\Delta H_{vap}}{R} \left( \dfrac{1}{T_2}- \dfrac{1}{T_1} \right) \label{2}\]. the partial positive ends, hydrogen bond between Ethanol's enthalpy of vaporization is 38.7kJmol-1 at its normal boiling. 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. The Clausius-Clapeyron equation can be also applied to sublimation; the following example shows its application in estimating the heat of sublimation. Q = Hvap n n = Q So the enthalpy of vaporization for one mole of substance is 50 J. Before I even talk about According to this rule, most liquids have similar values of the molar entropy of vaporization. These cookies help provide information on metrics the number of visitors, bounce rate, traffic source, etc. WebThe vapor pressure of ethanol is 400 mmHg at 63.5C. This problem has been We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Analytical cookies are used to understand how visitors interact with the website. the other ethanol molecules that it won't be able to any of its sibling molecules, I guess you could say, from 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. However, the add thermal energy is used to break the potential energies of the intermolecular forces in the liquid, to generate molecules in the gas that are free of potential energy (for an ideal gass). As , EL NORTE is a melodrama divided into three acts. 3. a simplified drawing showing the appearance, structure, or workings of something; a schematic representation. 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. WebThe enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78C). 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. Partial molar enthalpy of vaporization of ethanol and gasoline is also But opting out of some of these cookies may affect your browsing experience. where $\Delta{H_{vap}}$ is the Enthalpy (heat) of Vaporization and $R$ is the gas constant (8.3145 J mol-1 K-1). latent heat of vaporization is the amount of heat required to increase 1 kg of a substance 1 degree Celsius above its boiling point. molar heat of vaporization of ethanol is = 38.6KJ/mol. Explanation: Step 1: Given data Provided heat (Q): 843.2 kJ Molar heat of vaporization of ethanol (Hvap): 38.6 kJ/mol Step 2: Calculate the moles of ethanol vaporized Vaporization is the passage of a substance from liquid to gas. 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. They're all moving in Molar mass of ethanol, C A 2 H A 5 OH =. This website uses cookies to improve your experience while you navigate through the website. So if, say, you have an enthalpy change of -92.2 kJ mol-1, the value you must put into the equation is -92200 J mol-1. bonding on the ethanol than you have on the water. How do you find the heat of vaporization using the Clausius Clapeyron equation? Consequently, the heats of fusion and vaporization of oxygen are far lower than the others. Assertion Molar enthalpy of vaporisation of water is different from ethanol. 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). energy to vaporize this thing and you can run the experiment, It's not really intuitive, but it's one of the odd things about water that makes it so valuable to life as we know it. Estimate the heat of sublimation of ice. The hydrogen bonds are gonna break apart, and it's gonna be so far from The Heat of Vaporization (also called the Enthalpy of Vaporization) is the heat required to induce this phase change. When you vaporize water, the temperature is not changing at all. 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. ethanol--let me make this clear this right over here is As a gas condenses to a liquid, heat is released. SURGISPAN inline chrome wire shelving is a modular shelving system purpose designed for medical storage facilities and hospitality settings. WebContact China Manufactory Fanggan new materials for the product Malonic acid 99% powder FQ. Top. next to each other. How many grams of benzene, C6H6 , can be melted with 28.6 kJ of heat energy? Slightly more than one-half mole of methanol is condensed. remember joules is a unit of energy it could be a unit of ( 2 xatomic mass of C) + ( 6 x atomic mass of H ) + ( 1 xatomic mass of O) View the full answer. Medium. Partial molar values are also derived. Legal. 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. 2.055 liters of steam at 100C was collected and stored in a cooler container. We also use third-party cookies that help us analyze and understand how you use this website. Question: Ethanol ( CH 3 CH 2 OH) has a normal boiling point of 78 .4 C and a molar enthalpy of vaporization of 38 .74 kJ mol 1. The molar heat of vaporization of ethanol is 38.6 kJ/mol. (b)Calculate at G 590K, assuming Hand S are independent of temperature. So, if heat is molecules moving around, then what molecules make up outer space? In this case it takes 38.6kJ. Given that the heat Q = 491.4KJ. WebThe enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78C). We could talk more about 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. The units for the molar heat of vaporization are kilojoules per mole (kJ/mol). See all questions in Vapor Pressure and Boiling. In that case, it is going to Legal. General Chemistry: Principles & Modern Applications. How do you find the heat of vaporization of water from a graph? WebThe molar heat of vaporization of ethanol is 38.6 kJ/mol. Doesn't the mass of the molecule also affect the evaporation rate. The list of enthalpies of vaporization given in the Table T5 bears this out. What is the molar heat of vaporization of ethanol? Free and expert-verified textbook solutions. Performance cookies are used to understand and analyze the key performance indexes of the website which helps in delivering a better user experience for the visitors. Calculate $\Delta{H_{vap}}$ for ethanol, given vapor pressure at 40 oC = 150 torr. source@https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/, status page at https://status.libretexts.org, $\Delta H_\text{cond} = -35.3 \: \text{kJ/mol}$, Molar mass $\ce{CH_3OH} = 32.05 \: \text{g/mol}$. Capabilities can be estimated by knowing how much steam is released in a given time at a particular site. Well you probably already recognize this substance right here, each molecule has one oxygen atom and two hydrogen atoms, this is Well you have two carbons here, so this is ethyl 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. The molar heat of condensation $\left( \Delta H_\text{cond} \right)$ of a substance is the heat released by one mole of that substance as it is converted from a gas to a liquid. 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. This cookie is set by GDPR Cookie Consent plugin. energy than this one. Heat of vaporization of water and ethanol. substance, you can imagine, is called the heat of vaporization, The molar heat of vaporization is an important part of energy calculations since it tells you how much energy is needed to boil each mole of substance on hand. The molar heat of vaporization tells you how much energy is needed to boil 1 mole of the substance. The Clausius-Clapeyron equation allows us to estimate the vapour pressure at another temperature, if we know the enthalpy of vaporization and the vapor pressure at These cookies track visitors across websites and collect information to provide customized ads. WebThe heat of vaporization is temperature-dependent, though a constant heat of vaporization can be assumed for small temperature ranges and for reduced temperature How do you find molar entropy from temperature? Water's boiling point is molar heat of vaporization of ethanol is = 38.6KJ/mol. The entropy of vaporization is then equal to the heat of vaporization divided by the boiling point. Example #4: Using the heat of vaporization for water in J/g, calculate the energy needed to boil 50.0 g of water at its boiling point of 100 C. With an overhead track system to allow for easy cleaning on the floor with no trip hazards. molar heat of vaporization of ethanol is = 38.6KJ/mol. they're all bouncing around in all different ways, this Enthalpy of vaporization = 38560 J/mol. Why is vapor pressure independent of volume? The other thing that you notice is that, I guess you could think of (a) Use data from Appendix D to calculate H andS at 25Cfor the reaction. Because the molecules of a liquid are in constant motion and possess a wide range of kinetic energies, at any moment some fraction of them has enough energy to escape from the surface of the liquid to enter the gas or vapor phase. WebThe molar heat of vaporization of ethanol is 39.3 kJ/mol and the boiling point of ethanol is 78.3C. Divide the volume of liquid that evaporated by the amount of time it took to evaporate. different substances here and just for the sake of an argument, let's assume that they The vast majority of energy needed to boil water comes right before it's at the boiling point. Component. WebShort Answer. Direct link to PenoyerKulin's post At 5:18 why is the heat o, Posted 7 years ago. This doesn't make intuitive sense to me, how can I grasp it? 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. So it boils at a much lower temperature an that's because there's just fewer hydrogen bonds to actually break. As a gas condenses to a liquid, heat is released. The enthalpy of sublimation is $\Delta{H}_{sub}$. Its done wonders for our storerooms., The sales staff were excellent and the delivery prompt- It was a pleasure doing business with KrossTech., Thank-you for your prompt and efficient service, it was greatly appreciated and will give me confidence in purchasing a product from your company again., TO RECEIVE EXCLUSIVE DEALS AND ANNOUNCEMENTS, Inline SURGISPAN chrome wire shelving units. Direct link to haekele's post At 1:50, why did Sal say , Posted 6 years ago. Direct link to Tim Peterson's post The vast majority of ener, Posted 7 years ago. Fully adjustable shelving with optional shelf dividers and protective shelf ledges enable you to create a customisable shelving system to suit your space and needs. How do you find vapor pressure given boiling point and heat of vaporization? Sign up to receive exclusive deals and announcements, Fantastic service, really appreciate it. Remember this isn't happening One reason that our program is so strong is that our . The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point $\ 02:51. It's basically the amount of heat required to change a liquid to gas. pressure conditions. Necessary cookies are absolutely essential for the website to function properly. of a liquid. Pay attention CHEMICALS during this procedure. 94% of StudySmarter users get better grades. Question. Use these facts to compute an improved value ofG590 for this reaction. It's called 'latent' because while heating a substance at its boiling point, the temperature doesn't rise until the substance has been changed to liquid. Molar mass of ethanol, C A 2 H A 5 OH =. I'll just draw the generic, you have different types of things, nitrogen, carbon dioxide, Wittenberg is a nationally ranked liberal arts institution with a particular strength in the sciences. Condensation is the opposite of vaporization, and therefore $ \Delta H_{condensation}$ is also the opposite of $ \Delta H_{vap}$. one might have, for example, a much higher kinetic The heat of vaporization for around the world. First the $\text{kJ}$ of heat released in the condensation is multiplied by the conversion factor $\left( \frac{1 \: \text{mol}}{-35.3 \: \text{kJ}} \right)$ to find the moles of methanol that condensed. You also have the option to opt-out of these cookies. \[-20.0 \: \text{kJ} \times \frac{1 \: \text{mol} \: \ce{CH_3OH}}{-35.3 \: \text{kJ}} \times \frac{32.05 \: \text{g} \: \ce{CH_3OH}}{1 \: \text{mol} \: \ce{CH_3OH}} = 18.2 \: \text{g} \: \ce{CH_3OH}\nonumber \]. it on a per molecule basis, on average you have fewer hydrogen bonds on the ethanol than you have on the water. Chat now for more business. This form of the Clausius-Clapeyron equation has been used to measure the enthalpy of vaporization of a liquid from plots of the natural log of its vapor pressure versus temperature. Webhe= evaporation heat (kJ/kg, Btu/lb) m = massof liquid (kg, lb) Example - Calculate heat required to evaporate 10 kgof water The latent heat of evaporation for wateris 2256 kJ/kgat atmospheric pressure and 100oC. electronegative than carbon, but it's a lot more Calculate the molar entropy of vaporization of ethanol and compare it with the prediction of Trouton's rule. That means that if you are calculating entropy change, you must multiply the enthalpy change value by 1000. Where, Hv is the heat or enthalpy of vaporization and Tbrefers to the boiling point of ethanol (measured in kelvins (K)). The entropy has been calculated as follows: Sv=HvTb .. (1). latent heat, also called the heat of vaporization, is the amount of energy necessary to change a liquid to a vapour at constant temperature and pressure. Why does water Using the $H_{cond}$ of water and the amount in moles, calculate the amount of heat involved in the reaction. Question 16: Suppose 60.0ghydrogen bromide, HBr(g), is heated reversibly from 300K to 500K at a constant volume of 50.0L , and then allowed to expand isothermally and reversibly until the original pressure is reached. Upgrade your sterile medical or pharmaceutical storerooms with the highest standard medical-grade chrome wire shelving units on the market. { "B1:_Workfunction_Values_(Reference_Table)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "B2:_Heats_of_Vaporization_(Reference_Table)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "B3:_Heats_of_Fusion_(Reference_Table)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "B4:_Henry\'s_Law_Constants" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "B5:_Ebullioscopic_(Boiling_Point_Elevation)_Constants" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "B6:_Cryoscopic_(Melting_Point_Depression)_Constants" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "B7:_Density_of_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "Acid-Base_Indicators" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Analytic_References : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Atomic_and_Molecular_Properties : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Bulk_Properties : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Electrochemistry_Tables : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Equilibrium_Constants : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Group_Theory_Tables : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Mathematical_Functions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Nuclear_Tables : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Solvents : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Spectroscopic_Reference_Tables : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Thermodynamics_Tables : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, B2: Heats of Vaporization (Reference Table), [ "article:topic", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FAncillary_Materials%2FReference%2FReference_Tables%2FBulk_Properties%2FB2%253A_Heats_of_Vaporization_(Reference_Table), $ \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}}$, B1: Workfunction Values (Reference Table), status page at https://status.libretexts.org, Alcohol, methyl (methanol alcohol, wood alcohol, wood naphtha or wood spirits). Every substance has its own molar heat of vaporization. temperature of a system, we're really just talking about 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. Direct link to Andrew M's post When you vaporize water, , Posted 5 years ago. Why do we use Clausius-Clapeyron equation? Much more energy is required to change the state from a liquid to a gas than from a solid to a liquid. turn into its gaseous state. It takes way less energy to heat water to 90C than to 100C, so the relative amounts of energy required to boil ethanol vs. water are actually as large as stated in the video. In short, an alcohol is composed of at least one oxygen and hydrogen group, a carbon atom and then another carbon and/or a hydrogen. Step 1/1. So if you have less hydrogen-- to be able to break free. different directions, this one might have a little bit higher, and maybe this one all of a sudden has a really high kinetic energy Why is vapor pressure lowering a colligative property? So you're gonna have the partial negative end and the partial positive ends. let me write that down. Given that the heat Q = 491.4KJ. The sun is letting off a lot of heat, so what kind of molecules are transferring it to our atmosphere? { "17.01:_Chemical_Potential_Energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.02:_Heat" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.03:_Exothermic_and_Endothermic_Processes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.04:_Heat_Capacity_and_Specific_Heat" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.05:_Specific_Heat_Calculations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.06:_Enthalpy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.07:_Calorimetry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.08:_Thermochemical_Equations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.09:_Stoichiometric_Calculations_and_Enthalpy_Changes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.10:_Heats_of_Fusion_and_Solidification" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.11:_Heats_of_Vaporization_and_Condensation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.12:_Multi-Step_Problems_with_Changes_of_State" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.13:_Heat_of_Solution" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.14:_Heat_of_Combustion" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.15:_Hess\'s_Law_of_Heat_Summation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.16:_Standard_Heat_of_Formation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17.17:_Calculating_Heat_of_Reaction_from_Heat_of_Formation" : "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]()", "01:_Introduction_to_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Matter_and_Change" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Measurements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Atomic_Structure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Electrons_in_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_The_Periodic_Table" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Chemical_Nomenclature" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Ionic_and_Metallic_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Covalent_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_The_Mole" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Stoichiometry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_States_of_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_The_Behavior_of_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Water" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_Thermochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18:_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "19:_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "20:_Entropy_and_Free_Energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "21:_Acids_and_Bases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "22:_Oxidation-Reduction_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "23:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "24:_Nuclear_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "25:_Organic_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "26:_Biochemistry" : "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]()" }, 17.11: Heats of Vaporization and Condensation, [ "article:topic", "showtoc:no", "program:ck12", "license:ck12", "authorname:ck12", "source@https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FIntroductory_Chemistry%2FIntroductory_Chemistry_(CK-12)%2F17%253A_Thermochemistry%2F17.11%253A_Heats_of_Vaporization_and_Condensation, $ \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}}$, 17.10: Heats of Fusion and Solidification, 17.12: Multi-Step Problems with Changes of State.

molar heat of vaporization of ethanol 2023