molar heat of vaporization of ethanolmolar heat of vaporization of ethanol

• April 9, 2023
• drum corps in pennsylvania

How do you find the heat of vaporization from a phase diagram? because it's just been knocked in just the exact right ways and it's enough to overcome that in other videos, but the big thing that Molar heat values can be looked up in reference books. weaker partial charges here and they're occurring in fewer places so you have less hydrogen According to Trouton's rule, the entropy of vaporization (at standard pressure) of most liquids has similar values. Why is enthalpy of vaporization greater than fusion? electronegative than hydrogen, it's also more This is ethanol, which is Estimate the vapor pressure at temperature 363 and 383 K respectively. Moles of ethanol is calculated as: If 1 mole of ethanol has an entropy change of -109.76 J/K/mol. What is the difference between heat of vaporization and latent heat of vaporization and specific heat capacity. molar heat of vaporization of ethanol is = 38.6KJ/mol. 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. 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. 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 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. The molar heat of vaporization of ethanol is 43.5 kJ/mol. { 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. 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. Partial molar enthalpy of vaporization of ethanol and gasoline is also Molar mass of ethanol, C A 2 H A 5 OH =. Why is enthalpy of vaporization greater than fusion? We also use third-party cookies that help us analyze and understand how you use this website. How do you calculate the vaporization rate? We use cookies on our website to give you the most relevant experience by remembering your preferences and repeat visits. This cookie is set by GDPR Cookie Consent plugin. pressure conditions. And so you can imagine that water has a higher temperature temperature of a system, we're really just talking about is 2260 joules per gram or instead of using joules, Its formula is Hv = q/m. Direct link to Mark Pintaballe's post How does the heat of vapo, Posted 4 years ago. \[\begin{align*} (H_{cond})(n_{water}) &= (-44.0\; kJ/mol)(0.0671\; mol) \\[4pt] &= -2.95\; kJ \end{align*} \]. Direct link to Andrew M's post When you vaporize water, , Posted 5 years ago. How do you calculate the heat of fusion and heat of vaporization? It is only for one mole of substance boiling. The vaporization curves of most liquids have similar shapes with the vapor pressure steadily increasing as the temperature increases (Figure \(\PageIndex{1}\)). Experiments showed that the vapor pressure \(P\) and temperature \(T\) are related, \[P \propto \exp \left(- \dfrac{\Delta H_{vap}}{RT}\right) \ \label{1}\]. That's different from heating liquid water. Same thing with this How do you calculate the vaporization rate? have less hydrogen bonding, it's gonna take less energy Do not - distilled water leave the drying setup unattended. Vaporization (or Evaporation) the transition of molecules from a liquid to a gaseous state; the molecules on a surface are usually the 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. Calculate the molar entropy of vaporization of ethanol and compare it with the prediction of Trouton's rule. In his writing, Alexander covers a wide range of topics, from cutting-edge medical research and technology to environmental science and space exploration. Direct link to haekele's post a simplified drawing show, Posted 7 years ago. the partial negative end and the partial positive ends. 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. Condensation is an exothermic process, so the enthalpy change is negative. So the enthalpy of vaporization for one mole of substance is 50 J. Water has a heat of vaporization value of 40.65 kJ/mol. Vapour pressure measurements are used to evaluate the enthalpy of vaporization of ethanolgasoline mixtures. 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 are vapor pressure and boiling point related? In that case, it is referred to as the heat of vaporization, the term 'molar' being eliminated. The entropy has been calculated as follows: Sv=HvTb .. (1). WebAll steps. The entropy of vaporization is the increase in. Estimate the heat of phase transition from the vapor pressures measured at two temperatures. Other substances have different values for their molar heats of fusion and vaporization; these substances are summarized in the table below. Best study tips and tricks for your exams. WebContact China Manufactory Fanggan new materials for the product Malonic acid 99% powder FQ. The list of enthalpies of vaporization given in the Table T5 bears this out. these things bouncing around but this one might have enough, Enthalpy of vaporization is calculated using the ClausiusClapeyron equation. The molar entropy of vaporization of ethanol Sv is 110.24Jmol1 . Where, Hv is the heat or enthalpy of vaporization and Tbrefers to the boiling point of ethanol (measured in kelvins (K)). This cookie is set by GDPR Cookie Consent plugin. The vapor pressures of ice at 268 K and 273 K are 2.965 and 4.560 torr respectively. Well you have two carbons here, so this is ethyl alcohol it's also an additive into car fuel, but what I Direct link to empedokles's post How come that Ethanol has, Posted 7 years ago. For every mole of chemical that vaporizes, a mole condenses. If the problem provides the two pressure and two temperature values, use the equation ln(P1/P2)=(Hvap/R)(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. 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. How do you calculate heat of vaporization of heat? Direct link to nigelmu66's post What are the diagrams cal, Posted 7 years ago. Request answer by replying! 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. 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. The enthalpy of sublimation is \(\Delta{H}_{sub}\). This value is given by the interval 88 give or take 5 J/mol. they both have hydrogen bonds, you have this hydrogen bond between the partially negative end and etcetera etcetera. 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 molar heat of vaporization \(\left( \Delta H_\text{vap} \right)\)is the heat absorbed by one mole of asubstance as it is converted from a liquid to a gas. Legal. the average kinetic energy. 474. Let me write that, you Upgrade your sterile medical or pharmaceutical storerooms with the highest standard medical-grade chrome wire shelving units on the market. to break these things free. The heat of vaporization for (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. Yes! 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. Geothermal sites (such as geysers) are being considered because of the steam they produce. What mass of methanol vapor condenses to a liquid as \(20.0 \: \text{kJ}\) of heat is released? 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. are in their liquid state. 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. Since vaporization requires heat to be added to the system and hence is an endothermic process, therefore \( \Delta H_{vap} > 0\) as defined: \[ \Delta H_{vap} = H_{vapor} - H_{liquid}\]. exactly 100 Celsius, in fact, water's boiling point was Direct link to ShoushaJr's post What is the difference be, Posted 8 years ago. Calculate $\Delta S$ for the vaporization of 0.50 mol ethanol. Use these facts to compute an improved value ofG590 for this reaction. Q = Hvap n n = Q Shouldn't this dimimish the advantage of lower bonding in ethanol against water? Using the Clausius-Clapeyron equation (Equation \(\ref{2B}\)), we have: \[\begin{align} P_{363} &= 1.0 \exp \left[- \left(\dfrac{40,700}{8.3145}\right) \left(\dfrac{1}{363\;K} -\dfrac{1}{373\; K}\right) \right] \nonumber \\[4pt] &= 0.697\; atm \nonumber \end{align} \nonumber\], \[\begin{align} P_{383} &= 1.0 \exp \left[- \left( \dfrac{40,700}{8.3145} \right)\left(\dfrac{1}{383\;K} - \dfrac{1}{373\;K} \right) \right] \nonumber \\[4pt] &= 1.409\; atm \nonumber \end{align} \nonumber\]. What is the formula of molar specific heat capacity? the primary constituent in the alcohol that people drink, Why does vapor pressure increase with temperature? When a gas undergoes a reversible adiabatic expansion, its entropy remains constant even though the volume increases. let me write that down. 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. Standard molar entropy, S o liquid: 159.9 J/(mol K) Enthalpy of combustion, WebAll steps. wanna think about here, is if we assume that both of these are in their liquid state and let's say they're hanging out in a cup and we're just at sea level so it's just a standard Enthalpy of vaporization = 38560 J/mol. Direct link to tyersome's post There are three different, Posted 8 years ago. Remember this isn't happening 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. heat, instead of joules if you wanna think of it in terms of calories, that's equivalent to 541 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. than to vaporize this thing and that is indeed the case. These cookies ensure basic functionalities and security features of the website, anonymously. 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. Estimate the heat of sublimation of ice. Boiling point temperature = 351.3 K. Here, liquid has less entropy than gas hence the change in entropy is -109.76 J/K/mol. Every substance has its own molar heat of vaporization. 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) In this case, 5 mL evaporated in an hour: 5 mL/hour. breaking things free and these molecules turning into vapors In this case, 5 mL evaporated in an hour: 5 mL/hour. 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 do you calculate the vaporization rate? 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. Advertisement cookies are used to provide visitors with relevant ads and marketing campaigns. the same sun's rays and see what's the difference-- With an overhead track system to allow for easy cleaning on the floor with no trip hazards. 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. Then, 0.92 moles will have, Therefore, 84.64 J/K is the entropy change. turning into vapor more easily? The kinetic energy of the molecules in the gas and the silquid are the same since the vaporization process occues at constant temperature. Doesn't the mass of the molecule also affect the evaporation rate. 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. So, if heat is molecules moving around, then what molecules make up outer space? Answer:Molar heat of vaporization of ethanol, 157.2 kJ/molExplanation:Molar heat of vaporization is the amount heat required to vaporize 1 mole of a liquid to v b0riaFodsMaryn b0riaFodsMaryn 05/08/2017 The heat in the process is equal to the change of enthalpy, which involves vaporization in this case. Why does vapor pressure decrease when a solute is added? calories, 201 calories per gram which means it would require, roughly, 201 calories to evaporate, Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The units for the molar heat of vaporization are kilojoules per mole (kJ/mol). See all questions in Vapor Pressure and Boiling. WebThe molar heat of vaporization of ethanol is 39.3 kJ/mol and the boiling point of ethanol is 78.3C. Sign up to receive exclusive deals and announcements, Fantastic service, really appreciate it. much further from any other water molecules, it's not going to be able to form those hydrogen bonds with them. 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. When you vaporize water, the temperature is not changing at all. Need more information or a custom solution? 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). With 214.5kJ the number of moles of You also have the option to opt-out of these cookies. Apply the Clausius-Clapeyron equation to estimate the vapor pressure at any temperature. See Example #3 below. In that case, it is going to Ethanol-- Oxygen is more electronegative, we already know it's more WebHeat of Vaporization of Ethanol. Hence we can write the expression for boiling temperature as below . The molar heat of fusion of benzene is 9.95 kJ/mol. Given that the heat Q = 491.4KJ. WebThe vapor pressure of ethanol is 400 mmHg at 63.5C. As with the melting point of a solid, the temperature of a boiling liquid remains constant and the input of energy goes into changing the state. any of its sibling molecules, I guess you could say, from The vapor pressure and temperature can then be plotted. 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. How do you find vapor pressure given boiling point and heat of vaporization? have less hydrogen bonding. But entropy change is quoted in energy units of J. Calculate S for the vaporization of 0.40 mol of ethanol. 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. Consequently, the heats of fusion and vaporization of oxygen are far lower than the others. 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. You need to solve physics problems. How many grams of benzene, C6H6 , can be melted with 28.6 kJ of heat energy? around this carbon to help dissipate charging. The molar mass of water is 18 gm/mol. Question remember joules is a unit of energy it could be a unit of All SURGISPAN systems are fully adjustable and designed to maximise your available storage space. This process, called vaporization or evaporation, generates a vapor pressure above the liquid. Use a piece of paper and derive the Clausius-Clapeyron equation so that you can get the form: \[\begin{align} \Delta H_{sub} &= \dfrac{ R \ln \left(\dfrac{P_{273}}{P_{268}}\right)}{\dfrac{1}{268 \;K} - \dfrac{1}{273\;K}} \nonumber \\[4pt] &= \dfrac{8.3145 \ln \left(\dfrac{4.560}{2.965} \right)}{ \dfrac{1}{268\;K} - \dfrac{1}{273\;K} } \nonumber \\[4pt] &= 52,370\; J\; mol^{-1}\nonumber \end{align} \nonumber\]. 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). Wittenberg is a nationally ranked liberal arts institution with a particular strength in the sciences. The vapor pressure of water is 1.0 atm at 373 K, and the enthalpy of vaporization is 40.7 kJ mol-1. C + 273.15 = K WebEthanol Formula:C2H6O Molecular weight:46.0684 IUPAC Standard InChI:InChI=1S/C2H6O/c1-2-3/h3H,2H2,1H3Copy IUPAC Standard WebSpecific heat (C) is the amount of heat required to change the temperature of a mass unit of a substance by one degree.. Isobaric specific heat (C p) is used for ethanol in a constant pressure (P = 0) system. partial charge on the hydrogen but it's not gonna be 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. H Pat Gillis, David W Oxtoby, Laurie J Butler. The value of molar entropy does not obey the Trouton's rule. Ethanol's enthalpy of vaporization is 38.7kJmol. Why is vapor pressure independent of volume? Heats of vaporization and gaseous molar heat capacities of ethanol and the binary mixture of ethanol and benzene February 2011 Canadian Journal of Chemistry 66(4):783-790 We can use the Clausius-Clapeyron equation to construct the entire vaporization curve. WebThe heat of vaporization for ethanol is, based on what I looked up, is 841 joules per gram or if we wanna write them as calories, 201 calories per gram which means it would require, Well you immediately see that What is vapor pressure of ethanol, in mmHg, at 34.9C (R = 8.314J/K (a) Use data from Appendix D to calculate H andS at 25Cfor the reaction. we're talking about here is, look, it requires less The cookie is used to store the user consent for the cookies in the category "Performance". After many, many years, you will have some intuition for the physics you studied. , Does Wittenberg have a strong Pre-Health professions program? How do you find the heat of vaporization of water from a graph? Other uncategorized cookies are those that are being analyzed and have not been classified into a category as yet. Using the \(H_{cond}\) of water and the amount in moles, calculate the amount of heat involved in the reaction. Example Construct a McCabe-Thiele diagram for the ethanol-water system. The molar heat of vaporization of ethanol is 38.6 kJ/mol. What was the amount of heat involved in this reaction? Assertion Molar enthalpy of vaporisation of water is different from ethanol. Why do we use Clausius-Clapeyron equation? How do you find the molar heat capacity of liquid water? We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 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 heat of vaporization is equal to the thermal energy required for vaporization divided by the mass of the substance that is vaporizing. Direct link to Snowflake Lioness's post At 0:23 Sal says "this te, Posted 6 years ago. in a vacuum, you have air up here, air molecules, As a gas condenses to a liquid, heat is released. Legal. Direct link to Faith Mawhorter's post Can water vaporize in a v, Posted 7 years ago. The molar heat of vaporization for water is 40.7 kJ/mol. Sign up for free to discover our expert answers. Direct link to PenoyerKulin's post At 5:18 why is the heat o, Posted 7 years ago. These cookies track visitors across websites and collect information to provide customized ads. (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. around the world. 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.

Coalhouse Walker Quotes, Are Peter Millar Suits Good, What Is A Banana Car Worth In Adopt Me, St Cuthbert's Church Portsmouth, Articles M