molar heat of vaporization of ethanol

Contact the team at KROSSTECH today to learn more about SURGISPAN. different directions, this one might have a little bit higher, and maybe this one all of a sudden has a really high kinetic energy Do NOT follow this link or you will be banned from the site! This doesn't make intuitive sense to me, how can I grasp it? Doesn't the mass of the molecule also affect the evaporation rate. See Example #3 below. Examples of calculations involving the molar heat of vaporization and condensationare illustrated. When a gas undergoes a reversible adiabatic expansion, its entropy remains constant even though the volume increases. Heat of vaporization directly affects potential of liquid substance to evaporate. Reason Water is more polar than ethanol. WebThe molar enthalpy of fusion of ice at 0 C is 6.02 kJ mol 1; the molar heat capacity of undercooled water is 75.3 J mol 1 K 1. The increase in vapor pressure is not a linear process. In this case it takes 38.6kJ. up the same amount of time, a glass of water and a glass of ethanol and then see how long it takes. 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. 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. actually has more hydrogen atoms per molecule, but if you In this case, 5 mL evaporated in an hour: 5 mL/hour. But entropy change is quoted in energy units of J. So you have this imbalance here and then on top of that, this carbon, you have a lot more atoms here in which to distribute a partial charge. How do you find the molar entropy of a gas? WebThe following method of - heater (hot plate) drying the product must be - graduated cylinder followed to avoid spattering and - water bath loss of product. Given that the heat Q = 491.4KJ. 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 View solution > The enthalpy of vaporisation of per mole of ethanol Hess Law of Constant Heat Summation. See larger image: Data Table. A good approach is to find a mathematical model for the pressure increase as a function of temperature. 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? to fully vaporize a gram of ethanol at standard temperature, keeping the temperature constant. Partial molar enthalpy of vaporization of ethanol and gasoline is also they're all bouncing around in all different ways, this much further from any other water molecules, it's not going to be able to form those hydrogen bonds with them. The value of molar entropy does not obey the Trouton's rule. How much heat is absorbed when 2.04 g of water The Clausius-Clapeyron equation can be also applied to sublimation; the following example shows its application in estimating the heat of sublimation. is 2260 joules per gram or instead of using joules, Natural resources for electric power generation have traditionally been waterfalls, oil, coal, or nuclear power. water and we have drawn all neat hydrogen bonds right over there. light), which can travel through empty space. As we've already talked about, in the liquid state and frankly, How do you calculate molar heat of vaporization? ; At ambient pressure and \[\begin{align*} (H_{cond})(n_{water}) &= (-44.0\; kJ/mol)(0.0671\; mol) \\[4pt] &= -2.95\; kJ \end{align*} \]. Analytical cookies are used to understand how visitors interact with the website. The cookies is used to store the user consent for the cookies in the category "Necessary". 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. The value of molar entropy does not obey Trouton's rule. have less hydrogen bonding. 474. PLEAse show me a complete solution with corresponding units if applicable. How are vapor pressure and boiling point related? 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. turning into vapor more easily? The molar heat of vaporization $\left( \Delta H_\text{vap} \right)$ of a substance is the heat absorbed by one mole of that substance as it is converted from a liquid to a gas. 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): \[\ln \left( \dfrac{P_1}{P_2} \right) = - \dfrac{\Delta H_{vap}}{R} \left( \dfrac{1}{T_1}- \dfrac{1}{T_2} \right) \label{2B} \]. Such a separation requires energy (in the form of heat). How do you find the latent heat of vaporization from a graph? The molar entropy of vaporization of ethanol S v is 110.24 Jmol 1 . 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. What was the amount of heat involved in this reaction? This cookie is set by GDPR Cookie Consent plugin. Assume that is an ideal gas under these conditions. Do not - distilled water leave the drying setup unattended. For every mole of chemical that vaporizes, a mole condenses. Direct link to haekele's post At 1:50, why did Sal say , Posted 6 years ago. ( 2 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). 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 normal boiling point for ethanol is 78 oC. that's what's keeping the water together, flowing WebThe molar heat of vaporization equation looks like this: q = (H vap) (mass/molar mass) The meanings are as follows: 1) q is the total amount of heat involved. Step 1/1. If you're seeing this message, it means we're having trouble loading external resources on our website. Using the Clausius-Clapeyron equation (Equation $\ref{2B}$), we have: \[\begin{align} P_{363} &= 1.0 \exp \left[- \left(\dfrac{40,700}{8.3145}\right) \left(\dfrac{1}{363\;K} -\dfrac{1}{373\; K}\right) \right] \nonumber \\[4pt] &= 0.697\; atm \nonumber \end{align} \nonumber\], \[\begin{align} P_{383} &= 1.0 \exp \left[- \left( \dfrac{40,700}{8.3145} \right)\left(\dfrac{1}{383\;K} - \dfrac{1}{373\;K} \right) \right] \nonumber \\[4pt] &= 1.409\; atm \nonumber \end{align} \nonumber\]. Yes! The molar heat of vaporization of ethanol is 39.3 kJ/mol, and the boiling point 06:04. WebThe molar heat of vaporization of ethanol is 39.3 kJ/mol and the boiling point of ethanol is 78.3C. In that case, it is going to WebThe molar heat of vaporization of ethanol is 39.3 kJ/mol, and the boiling point of ethanol is 78.3C. WebThe heat of vaporization is temperature-dependent, though a constant heat of vaporization can be assumed for small temperature ranges and for reduced temperature breaking things free and these molecules turning into vapors Slightly more than one-half mole of methanol is condensed. WebEthanol Formula:C2H6O Molecular weight:46.0684 IUPAC Standard InChI:InChI=1S/C2H6O/c1-2-3/h3H,2H2,1H3Copy IUPAC Standard By clicking Accept, you consent to the use of ALL the cookies. bonding on the ethanol than you have on the water. It's changing state. What is the vapor pressure of ethanol at 50.0 C? This cookie is set by GDPR Cookie Consent plugin. because it's just been knocked in just the exact right ways and it's enough to overcome Other substances have different values for their molar heats of fusion and vaporization; these substances are summarized in the table below. So, if heat is molecules moving around, then what molecules make up outer space? Thus, while $H_{vapor} > H_{liquid}$, the kinetic energies of the molecules are equal. The molar heat of vaporization tells you how much energy is needed to boil 1 mole of the substance. https://www.khanacademy.org/science/physics/thermodynamics/specific-heat-and-heat-transfer/v/thermal-conduction-convection-and-radiation, Creative Commons Attribution/Non-Commercial/Share-Alike. 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. Upgrade your sterile medical or pharmaceutical storerooms with the highest standard medical-grade chrome wire shelving units on the market. \[\begin{align} H_{condensation} &= H_{liquid} - H_{vapor} \\[4pt] &= -H_{vap} \end{align}\]. The entropy of vaporization is the increase in entropy upon the vaporization of a liquid. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. WebThe characterization of both metal and oxide components of the core@shell structure requires the application of both surface-sensitive and bulk-sensitive techniques, which still provide limited information about the properties of This is ethanol, which is Molar mass of ethanol, C A 2 H A 5 OH =. We can thus expect liquids with strong intermolecular forces to have larger enthalpies of vaporization. Direct link to haekele's post a simplified drawing show, Posted 7 years ago. Top. - potassium bicarbonate Heat the dish and contents for 5- (b)Calculate at G 590K, assuming Hand S are independent of temperature. Calculateq,w,U,Ssys, and Gwhen 1.00mol ethanol is vaporized reversibly at 780 and 1 atm. The enthalpy of sublimation is $\Delta{H}_{sub}$. 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. 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. 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. Divide the volume of liquid that evaporated by the amount of time it took to evaporate. these things bouncing around but this one might have enough, We've all boiled things, boiling point is the point at which the vapor Necessary cookies are absolutely essential for the website to function properly. In other words, $\Delta H_\text{vap} = -\Delta H_\text{cond}$. This process, called vaporization or evaporation, generates a vapor pressure above the liquid. I'll just draw the generic, you have different types of things, nitrogen, carbon dioxide, Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4 C. Now the relation turns as . Pay attention CHEMICALS during this procedure. And so you can imagine that water has a higher temperature But opting out of some of these cookies may affect your browsing experience. of a liquid. WebShort Answer. molar heat of vaporization of ethanol is = 38.6KJ/mol. the partial negative end and the partial positive ends. The value used by an author is often the one they used as a student. Other uncategorized cookies are those that are being analyzed and have not been classified into a category as yet. electronegative than hydrogen, it's also more WebHeat of Vaporization of Ethanol. The first, titled Arturo Xuncax, is set in an Indian village in Guatemala. Capabilities can be estimated by knowing how much steam is released in a given time at a particular site. We can calculate the number of moles (n) vaporized using the following expression. How do you find the molar heat capacity of liquid water? How do you calculate the vaporization rate? 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. B2: Heats of Vaporization (Reference Table) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. You might see a value of 2257 J/g used. Petrucci, Ralph H., William S. Harwood, F. G. Herring, and Jeffry D. Madura. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. Why does vapor pressure increase with temperature? The key difference between enthalpy and molar enthalpy is that enthalpy is the total heat content of a thermodynamic system, whereas molar enthalpy is the total heat per mole of reactant in the system. SurgiSpan is fully adjustable and is available in both static & mobile bays. 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. 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. To get the heat of vaporization, you simply divide the molar heat by 18.015 g/mol. 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. 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. 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. The entropy has been calculated as follows: Sv=HvTb .. (1). energy to overcome the hydrogen bonds and overcome the pressure q = (40.7 kJ / mol) (49.5 g / 18.0 g/mol), Example #2: 80.1 g of H2O exists as a gas at 100 C. Calculate $\Delta{H_{vap}}$ for ethanol, given vapor pressure at 40 oC = 150 torr. 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. Given they both have hydrogen bonds, you have this hydrogen bond between the partially negative end and WebLiquid vapor transition at the boiling point is an equilibrium process, so. Heat of Vaporization is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. We can use the Clausius-Clapeyron equation to construct the entire vaporization curve. There could be a very weak partial charge distributed here amongst the carbons but you have a stronger Heat of vaporization of water and ethanol. The vapor pressure and temperature can then be plotted. In general the energy needed differs from one liquid to another depending on the magnitude of the intermolecular forces. The molar heat of vaporization of ethanol is 43.5 kJ/mol. Formula Molar Mass CAS Registry Number Name; C 2 H 6 O: 46.069: 64-17-5: Ethanol: Search the DDB for all data of Ethanol Diagrams. Component. Direct link to Ivana - Science trainee's post Heat of vaporization dire, Posted 3 years ago. The kinetic energy of the molecules in the gas and the silquid are the same since the vaporization process occues at constant temperature. You need to solve physics problems. Remember this isn't happening To determine the heat of vaporization, measure the vapor pressure at several different temperatures. to turn into its gas state. 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. Upper Saddle River, NJ: Pearson Prentice Hall, 2007. Water's boiling point is substance, you can imagine, is called the heat of vaporization, Molar mass of ethanol, C A 2 H A 5 OH =. The molar heat of condensation of a substance is the heat released by one mole of that substance as it is converted from a gas to a liquid. (Hint: Consider what happens to the distribution of velocities in the gas.). from the molecules above it to essentially vaporize, Transcribed Image Text: 1. What is the molar heat of vaporization of ethanol? 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. both these hydrogen bonds over here and the pressure Its molar heat of vaporization is 39.3 kJ/mol. Advertisement cookies are used to provide visitors with relevant ads and marketing campaigns. You need to ask yourself questions and then do problems to answer those questions. Everything you need for your studies in one place. Is it an element? Need more information or a custom solution? The cookie is set by the GDPR Cookie Consent plugin and is used to store whether or not user has consented to the use of cookies. The cookie is used to store the user consent for the cookies in the category "Performance". 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. Enthalpy of vaporization is calculated using the ClausiusClapeyron equation. WebThe enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78C). We use cookies on our website to give you the most relevant experience by remembering your preferences and repeat visits. Video Answer Legal. Using cp(HBr(g))=29.1JK-1mol-1, calculate U,q,w,H, and S for this process. Calculate the molar entropy of vaporization of ethanol and compare it with the prediction of Trouton's rule. Question 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. The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point $\ 02:51. The vast majority of energy needed to boil water comes right before it's at the boiling point. WebThis equation also relates these factors to the heat of vaporization of ethanol. Calculate $\Delta S$ for the vaporization of 0.50 mol ethanol. WebAll steps. Why do we use Clausius-Clapeyron equation? This cookie is set by GDPR Cookie Consent plugin. The heat of vaporization for Notice that for all substances, the heat of vaporization is substantially higher than the heat of fusion. 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). WebWater has a vaporization heat of 4060 calories per gram, but ethanol has a vaporization heat of 3179 calories per gram. How many kJ is required? How do you calculate the heat of fusion and heat of vaporization? Then, 0.92 moles will have, Therefore, 84.64 J/K is the entropy change. It is only for one mole of substance boiling. 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. 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. Here is the definition of the molar heat of vaporization: Keep in mind the fact that this is a very specific value. how much more energy, how much more time does it take for the water to evaporate than the ethanol. Definitions of Terms. After many, many years, you will have some intuition for the physics you studied. Request answer by replying! 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. Well you immediately see that Direct link to Faith Mawhorter's post Can water vaporize in a v, Posted 7 years ago. How do you find vapor pressure given boiling point and heat of vaporization? turn into its gaseous state. Why is enthalpy of vaporization greater than fusion? Before I even talk about So the enthalpy of vaporization for one mole of substance is 50 J. water, that's for water. The initial temperature is - 10 C and the final temperature is 0 C. Step 2: Concept used Entropy Change is the phenomenon that is the measure of change of disorder or randomness in a thermodynamic system. Stop procrastinating with our smart planner features. The heat of vaporization for ethanol is, based on what I looked WebThe enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78C). different substances here and just for the sake of an argument, let's assume that they T 2 = (78.4 + 273.15) K = 351.55 K; P 2 = 760 Torr ln( P 2 P 1) = H vap R ( 1 T 1 1 T 2) He also shares personal stories and insights from his own journey as a scientist and researcher. In this case, 5 mL evaporated in an hour: 5 mL/hour. 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. Direct link to Tim Peterson's post The vast majority of ener, Posted 7 years ago. 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. Chat now for more business. MITs Alan , In 2020, as a response to the disruption caused by COVID-19, the College Board modified the AP exams so they were shorter, administered online, covered less material, and had a different format than previous tests. 3. energy than this one. Calculate the molar entropy of vaporization of ethanol and compare it with the prediction of Trouton's rule. 100.0 + 273.15 = 373.15 K, \[\begin{align*} n_{water} &= \dfrac{PV}{RT} \\[4pt] &= \dfrac{(1.0\; atm)(2.055\; L)}{(0.08206\; L\; atm\; mol^{-1} K^{-1})(373.15\; K)} \\[4pt] &= 0.0671\; mol \end{align*}\], \[H_{cond} = -44.0\; kJ/ mol \nonumber\]. Enthalpy of vaporization = 38560 J/mol. (a) Use data from Appendix D to calculate H andS at 25Cfor the reaction. 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. ethanol's boiling point is approximately 78 Celsius. The same thing might be true over here, maybe this is the molecule that has the super high kinetic energy Geothermal sites (such as geysers) are being considered because of the steam they produce. Question. What is heat of vaporization in chemistry? 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. Estimate the heat of phase transition from the vapor pressures measured at two temperatures. calories, 201 calories per gram which means it would require, roughly, 201 calories to evaporate, Calculate S for the vaporization of 0.40 mol of ethanol. Question: Ethanol (CH3CH2OH) has a normal boiling point of 78.4C and a molar enthalpy of vaporization of 38.74 kJ mol1. Divide the volume of liquid that evaporated by the amount of time it took to evaporate. 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. The vapor pressure of water is 1.0 atm at 373 K, and the enthalpy of vaporization is 40.7 kJ mol-1. The molar heat of vaporization of ethanol is 38.6 kJ/mol. weaker partial charges here and they're occurring in fewer places so you have less hydrogen 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. Then, moles are converted to grams. . scale, so by definition, it's 100 Celsius, while to break these things free. Show that the vapor pressure of ice at 274 K is higher than that of water at the same temperature. The entropy of vaporization is then equal to the heat of vaporization divided by the boiling point. (T1-T2/T1xT2), where P1 and P2 are the pressure values; Hvap is the molar heat of vaporization; R is the gas constant; and T1 and T2 are the temperature values. WebThe molar heat of vaporization of ethanol is 38.6 kJ/mol. Shouldn't this dimimish the advantage of lower bonding in ethanol against water? For more answers visit our other sites: AnswerAccurate HomeworkAnswerHelp AnswerHappy and Snapsterpiece. Step 1/1. it would take, on average, more heat to vaporize this thing The molar mass of water is 18 gm/mol. The molar heat of vaporization of ethanol is 43.5 kJ/mol. As a gas condenses to a liquid, heat is released. Using the $H_{cond}$ of water and the amount in moles, calculate the amount of heat involved in the reaction. 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