molar heat of vaporization of ethanol

Clausius-Clapeyron Equation - Chemistry LibreTexts Q = Hvap n n = Q of ethanol Direct link to haekele's post At 1:50, why did Sal say , Posted 6 years ago. Because \( \Delta H_{vap}\) is an endothermic process, where heat is lost in a reaction and must be added into the system from the surroundings, \( \Delta H_{condensation}\) is an exothermic process, where heat is absorbed in a reaction and must be given off from the system into the surroundings. up the same amount of time, a glass of water and a glass of ethanol and then see how long it takes. What is the molar heat of vaporization of water? We also use third-party cookies that help us analyze and understand how you use this website. What is vapor pressure of ethanol, in mmHg, at 34.9C (R = 8.314J/K Moles of ethanol is calculated as: If 1 mole of ethanol has an entropy change of -109.76 J/K/mol. For more answers visit our other sites: AnswerAccurate HomeworkAnswerHelp AnswerHappy and Snapsterpiece. These cookies will be stored in your browser only with your consent. We've all boiled things, boiling point is the point at which the vapor electronegative than hydrogen, it's also more 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 WebThe heat of vaporization is temperature-dependent, though a constant heat of vaporization can be assumed for small temperature ranges and for reduced temperature Upgrade your sterile medical or pharmaceutical storerooms with the highest standard medical-grade chrome wire shelving units on the market. These cookies ensure basic functionalities and security features of the website, anonymously. heat, instead of joules if you wanna think of it in terms of calories, that's equivalent to 541 Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Slightly more than one-half mole of methanol is condensed. How do you calculate molar heat of vaporization? the average kinetic energy. WebWater has a vaporization heat of 4060 calories per gram, but ethanol has a vaporization heat of 3179 calories per gram. What is the formula of molar specific heat capacity? That means that if you are calculating entropy change, you must multiply the enthalpy change value by 1000. (a) Use data from Appendix D to calculate H andS at 25Cfor the reaction. Molar Heat Where, Hv is the heat or enthalpy of vaporization and Tbrefers to the boiling point of ethanol (measured in kelvins (K)). it is about how strong the intermolecular forces are that are holding the molecules together. Using the Clausius-Clapeyron Equation The equation can be used to solve for the heat of vaporization or the vapor pressure at any temperature. Answer only. vapor pressure of ethanol 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. the other ethanol molecules that it won't be able to Because \(H_{condensation}\), also written as \(H_{cond}\), is an exothermic process, its value is always negative. Well you immediately see that What was the amount of heat involved in this reaction? Example Construct a McCabe-Thiele diagram for the ethanol-water system. Sign up for free to discover our expert answers. For every mole of chemical that vaporizes, a mole condenses. Now the relation turns as . The ethanol molecule is much heavier than the water molecule. Heat of vaporization directly affects potential of liquid substance to evaporate. Request answer by replying! of a liquid. You need to solve physics problems. 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 cookie is set by GDPR cookie consent to record the user consent for the cookies in the category "Functional". This can be the fault of the strong hydrogen bonds which is responsible for the level of randomness. The entropy of vaporization is then equal to the heat of vaporization divided by the boiling point. To calculate S for a chemical reaction from standard molar entropies, we use the familiar products minus reactants rule, in which the absolute entropy of each reactant and product is multiplied by its stoichiometric coefficient in the balanced chemical equation. Lab Booklet_2020-21 Spring | PDF | Chemical Polarity | Chemical By clicking Accept, you consent to the use of ALL the cookies. they both have hydrogen bonds, you have this hydrogen bond between the partially negative end and Thank you., Its been a pleasure dealing with Krosstech., We are really happy with the product. Calculate AS for the vaporization of 0.50 mol ethanol. \[\begin{array}{ll} \ce{H_2O} \left( l \right) \rightarrow \ce{H_2O} \left( g \right) & \Delta H_\text{vap} = 40.7 \: \text{kJ/mol} \\ \ce{H_2O} \left( g \right) \rightarrow \ce{H_2O} \left( l \right) & \Delta H_\text{cond} =-40.7 \: \text{kJ/mol} \end{array}\nonumber \]. The molar heat of vaporization of ethanol is 43.5 kJ/mol. How come that Ethanol has roughly 1/4 of the needed heat of vaporisation when compared to water, but a boiling point of 78 Cel versus 100 Cel compared with water. SURGISPAN inline chrome wire shelving is a modular shelving system purpose designed for medical storage facilities and hospitality settings. How do you calculate the vaporization rate? View solution > The enthalpy of vaporisation of per mole of ethanol Hess Law of Constant Heat Summation. Then, 0.92 moles will have, Therefore, 84.64 J/K is the entropy change. Heat of Vaporization - Chemistry LibreTexts This cookie is set by GDPR Cookie Consent plugin. Heat of vaporization of water and ethanol. of vaporization The Clausius-Clapeyron equation can be also applied to sublimation; the following example shows its application in estimating the heat of sublimation. Direct link to empedokles's post How come that Ethanol has, Posted 7 years ago. Sign up to receive exclusive deals and announcements, Fantastic service, really appreciate it. 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). 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According to Trouton's rule, the entropy of vaporization (at standard pressure) of most liquids has similar values. { 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. The heat of vaporization is equal to the thermal energy required for vaporization divided by the mass of the substance that is vaporizing. You need to ask yourself questions and then do problems to answer those questions. 9th ed. Remember this isn't happening ethanol--let me make this clear this right over here is Step 1: List the known quantities and plan the problem. actually has more hydrogen atoms per molecule, but if you 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). 2) H vap is the All of the substances in the table above, with the exception of oxygen, are capable of hydrogen bonding. WebThe molar heat of vaporization of ethanol is 39.3 kJ/mol and the boiling point 01:56. 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. SurgiSpan is fully adjustable and is available in both static & mobile bays. Advertisement cookies are used to provide visitors with relevant ads and marketing campaigns. Calculate the enthalpy of vaporisation per mole for ethanol Ethanol 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. Molar heat values can be looked up in reference books. let me write that down, heat of vaporization and you can imagine, it is higher for water Solution T 1 = (50.0+ 273.15) K = 323.15 K; P 1 =? WebThe vapor pressure of ethanol is 400 mmHg at 63.5C. than to vaporize this thing and that is indeed the case. Medium. 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. The molar heat of vaporization of ethanol is 38.6 kJ/mol. WebShort Answer. The molar heat of vaporization How do you find the latent heat of vaporization from a graph? Chem Exam Chapter 12 Questions Flashcards | Quizlet how much more energy, how much more time does it take for the water to evaporate than the ethanol. Well you probably already recognize this substance right here, each molecule has one oxygen atom and two hydrogen atoms, this is How do you calculate heat of vaporization of heat? WebIt is used as one of the standards for the octane-rating system for gasoline. The molar entropy of vaporization of ethanol Sv is 110.24Jmol1 . Energy is absorbed in the process of converting a liquid at its boiling point into a gas. Petrucci, Ralph H., William S. Harwood, F. G. Herring, and Jeffry D. Madura. many grams of ethanol, C2H5OH, can be boiled The entropy has been calculated as follows: Sv=HvTb .. (1). When a gas undergoes a reversible adiabatic expansion, its entropy remains constant even though the volume increases. heat of vaporization Return to the Time-Temperature Graph file. This is what's keeping Question It's changing state. Why is vapor pressure independent of volume? ethanol is a good bit lower. Posted 7 years ago. The first, titled Arturo Xuncax, is set in an Indian village in Guatemala. (b)Calculate at G 590K, assuming Hand S are independent of temperature. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 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. ChemTeam: Molar Heat of Vaporization Well you have two carbons here, so this is ethyl alcohol The heat of vaporization for ethanol is, based on what I looked Direct link to nigelmu66's post What are the diagrams cal, Posted 7 years ago. 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. You also have the option to opt-out of these cookies. We could talk more about Enthalpy of vaporization is calculated using the ClausiusClapeyron equation. Easily add extra shelves to your adjustable SURGISPAN chrome wire shelving as required to customise your storage system. After many, many years, you will have some intuition for the physics you studied. Ethanol's enthalpy of vaporization is 38.7kJmol-1 at its normal boiling. { "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 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Divide the volume of liquid that evaporated by the amount of time it took to evaporate. Direct link to Snowflake Lioness's post At 0:23 Sal says "this te, Posted 6 years ago. it would take, on average, more heat to vaporize this thing Just be aware that none of the values are wrong, they arise from different choices of values available. electronegative than carbon, but it's a lot more How many kJ must be removed to turn the water into liquid at 100 C, Example #3: Calculate the heat of vaporization for water in J/g, (40700 J/mol) / (18.015 g/mol) = 2259 J/g. They're all moving in H Pat Gillis, David W Oxtoby, Laurie J Butler. energy to overcome the hydrogen bonds and overcome the pressure WebThe molar heat of vaporization of ethanol is 39.3 kJ/mol, and the boiling point of ethanol is 78.3C. Capabilities can be estimated by knowing how much steam is released in a given time at a particular site. any of its sibling molecules, I guess you could say, from How do you calculate the heat of vaporization of a slope? The cookies is used to store the user consent for the cookies in the category "Necessary". So you're gonna have Vaporization (or Evaporation) the transition of molecules from a liquid to a gaseous state; the molecules on a surface are usually the molar heat of vaporization of ethanol is = 38.6KJ/mol. This results from using 40.66 kJ/mol rather than 40.7 kJ/mol. Every substance has its own molar heat of vaporization. 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. B2 LAB REPORT .pdf - Angadi 1 Neha Angadi Chemistry 1B of ethanol C=(S)/(mu)=(1)/(mu)(DeltaQ)/(muDeltaT)` where C is known as molar specific heat capacity of the substance C depends on the nature of the substance and its temperature. 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. Born and raised in the city of London, Alexander Johnson studied biology and chemistry in college and went on to earn a PhD in biochemistry. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. that's what's keeping the water together, flowing 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. from the air above it. have a larger molecule to distribute especially remember joules is a unit of energy it could be a unit of How do you find molar entropy from temperature? 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 \(\ce{CH_3OH} = 32.05 \: \text{g/mol}\). Each molecule, remember The vapor pressures of ice at 268 K and 273 K are 2.965 and 4.560 torr respectively. This is because of the large separation of the particles in the gas state. Answered: The following information is given for | bartleby 4. What is the molar heat of vaporization of ethanol? How many grams of benzene, C6H6 , can be melted with 28.6 kJ of heat energy? 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 Heat of Vaporization (also called the Enthalpy of Vaporization) is the heat required to induce this phase change. Pay attention CHEMICALS during this procedure. { 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.

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