Name: coffee cup calorimeter heat changes
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 3 min 2 s
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PS.Chm.7.2

Constant Pressure Calorimetry

Voor een chemische reactie die onder constante druk wordt uitgevoerd, zoals atmosferische druk, wordt de warmte die tijdens het proces wordt uitgewisseld, gemeten als de verandering in enthalpie delta H.De enthalpie-verandering voor de reactie komt tot uiting als een verandering in temperatuur, die wordt gemeten met behulp van een techniek die calorimetrie wordt genoemd. Bij calorimetrie wordt de reactie uitgevoerd in een verzegelde en gekalibreerde container, een calorimeter genaamd. De calorimeter is goed geïsoleerd en voorkomt elke warmtestroom tussen zichzelf en zijn omgeving.De warmte-uitwisseling tussen de reactanten en producten die het systeem vormen en de calorimeter die de omgeving is kan dus nauwkeurig worden berekend door de daaropvolgende veranderingen in de temperatuur in de calorimeter te volgen. Als de reactie exotherm is, stroomt er warmte uit het systeem naar de omgeving en stijgt de temperatuur. Omgekeerd, als de reactie endotherm is, stroomt er warmte uit de omgeving in het systeem, waardoor de temperatuur van de calorimeter daalt.Een eenvoudige constante druk calorimeter meet de verandering in enthalpie van een reactie die optreedt in een oplossing, onder constante drukcondities. De calorimeter bestaat uit twee koffiekopjes van piepschuim die in elkaar zijn genest en voorzien van een thermometer en een roerstaafje. De calorimeter is afgesloten met een loszittend kurkdeksel om een constante druk te handhaven die openstaat naar de atmosfeer.Stel dat 50, 0 milliliter elk van 1, 0 molair waterig zoutzuur en 1, 0 molair waterig kaliumhydroxide binnen de calorimeter reageren om de temperatuur van de oplossing met 6, 9 graden Celsius te verhogen. De warmte die wordt geabsorbeerd door de oplossing Q oplossing is gelijk aan zijn soortelijke warmte, C s, 4, 18 joules per gram graad Celsius hetzelfde als die van water vermenigvuldigd met zijn totale massa, m-100, 0 gram, en de verandering in temperatuur. De warmte van de oplossing is 2, 9 keer tien tot de macht van 3 joule of 2, 9 kilojoule.De reactiewarmte Q reactie-heeft dezelfde waarde, maar met een tegengesteld teken. Omdat de druk constant is, is de enthalpie-verandering hetzelfde als de warmte van de reactie. Om de enthalpie-verandering van de reactie per mol te vinden, wordt de enthalpie gedeeld door het aantal mol zoutzuur.De molen zoutzuur worden gevonden door het volume in liters 0, 05 L te vermenigvuldigen met de molariteit van 1 mol. Daarom geeft een negatieve 2, 9 kilojoule gedeeld door 0, 050 mol negatieve 58 kilojoule per mol.

calorimetrie met constante druk

Calorimetrie is een techniek die wordt gebruikt om de hoeveelheid warmte te meten die betrokken is bij een chemisch of fysisch proces of om de warmte te meten die naar of van een stof wordt overgedragen. De warmte wordt uitgewisseld met een gekalibreerd en geïsoleerd apparaat, de calorimeter. Calorimetrie-experimenten zijn gebaseerd op de veronderstelling dat er geen warmte-uitwisseling plaatsvindt tussen de geïsoleerde calorimeter en de externe omgeving. De goed geïsoleerde calorimeters voorkomen de overdracht van warmte tussen de calorimeter en de externe omgeving, waardoor de “omgeving” effectief wordt beperkt tot de niet-systeemcomponenten binnen de calorimeter (en de calorimeter zelf). Hierdoor is het mogelijk om nauwkeurig de warmte te bepalen die betrokken is bij chemische processen, zoals de energie-inhoud van voedingsmiddelen. De door de calorimeter gemeten temperatuurverandering wordt gebruikt om de hoeveelheid warmte af te leiden die door het onderzochte proces wordt overgedragen. In een calorimeter wordt een systeem gedefinieerd als de stof of stoffen die de chemische of fysische verandering ondergaan, of met andere woorden, de reactie, en de omgeving bestaat uit alle andere materie, inclusief de oplossing en alle andere componenten in de calorimeter die ofwel warmte leveren aan het systeem of absorberen uit het systeem. Voordat we de calorimetrie van chemische reacties bespreken, moeten we eerst een eenvoudiger voorbeeld overwegen dat het kernidee achter calorimetrie illustreert. Stel dat een heet stuk metaal met een hoge temperatuur in een stof met een lage temperatuur wordt geplaatst, zoals koud water. Warmte zal van het hete metaal naar het water stromen. De temperatuur van het metaal zal afnemen en de temperatuur van het water zal stijgen totdat de twee stoffen dezelfde temperatuur hebben – dat is wanneer ze thermisch evenwicht bereiken. Als dit in een calorimeter gebeurt, wordt alle warmte tussen de twee stoffen overgedragen, zonder dat er warmte wordt gewonnen of verloren door de externe omgeving. Onder deze ideale omstandigheden is de netto warmteverandering nul: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-01.png" style="height: 40px;"> Deze relatie kan worden herschikt om aan te tonen dat de warmte die door het metaal wordt gewonnen gelijk is aan de warmte die verloren gaat door de substantie water: <img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-02.png" style="height: 40px;"> De grootte van de warmte(verandering) is dus voor beide stoffen gelijk. Het negatieve teken geeft alleen aan dat qmetaal en qwater tegengesteld zijn in de richting van de warmtestroom (winst of verlies), maar het geeft niet het rekenkundige teken aan van een van de q-waarden (dat wordt bepaald door de vraag of de materie in kwestie warmte wint of verliest, per definitie). In de specifieke beschreven situatie is qmetaal een negatieve waarde en qwater een positieve waarde, omdat warmte wordt overgedragen van het metaal naar het water. Bij het gebruik van calorimetrie om de warmte te bepalen die betrokken is bij een chemische reactie, zijn dezelfde principes van toepassing. De hoeveelheid warmte die door de calorimeter wordt geabsorbeerd, is vaak zo klein dat deze meestal kan worden verwaarloosd, en de calorimeter minimaliseert de energie-uitwisseling met de buitenomgeving. Wanneer een exotherme reactie plaatsvindt in oplossing in een calorimeter, wordt de door de reactie geproduceerde warmte geabsorbeerd door de oplossing, waardoor de temperatuur stijgt. Wanneer er een endotherme reactie plaatsvindt, wordt de benodigde warmte geabsorbeerd uit de thermische energie van de oplossing, waardoor de temperatuur daalt. De temperatuurverandering (ΔT), samen met de soortelijke warmte (csoln) en de massa van de oplossing (msoln), kan vervolgens worden gebruikt om de hoeveelheid warmte (qsoln) te berekenen die in beide gevallen betrokken is. <img alt="Eq3" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-03.png" style="height: 40px;"> Een eenvoudige calorimeter, de koffiekopcalorimeter genoemd, is opgebouwd uit twee geneste polystyreenbekers, afgesloten met een loszittend deksel. Koffiekopcalorimeters worden gebruikt om de warmte te meten van reacties die plaatsvinden in oplossingen (meestal waterige oplossingen) en die geen of zeer weinig volumeverandering met zich meebrengen. Omdat energie niet wordt gecreëerd of vernietigd tijdens een chemische reactie, moeten de warmte die wordt geproduceerd of verbruikt tijdens de reactie (het “systeem”), qrxn, plus de warmte die wordt geabsorbeerd of verloren door de oplossing (de “omgeving”), qsoln, optellen. naar nul: <img alt="Eq4" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-04.png" style="height: 40px;"> Dit betekent dat de hoeveelheid warmte die tijdens de reactie wordt geproduceerd of verbruikt, gelijk is aan de hoeveelheid warmte die door de oplossing wordt geabsorbeerd of verloren: <img alt="Eq5" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-05.png" style="height: 40px;"> De koffiekopcalorimeter is een calorimeter met constante druk en de gemeten reactiewarmte is gelijk aan de verandering in enthalpie. <img alt="Eq6" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-06.png" style="height: 40px;"> Deze tekst is aangepast van <a href="https://openstax.org/books/chemistry-2e/pages/5-2-calorimetry">Openstax, Chemistry 2e, Sectie 5.2: Calorimetrie</a>.

Calorimetrie met constante druk

Calorimetry is a technique used to measure the amount of heat involved in a chemical or physical process or to measure the heat transferred to or from a ...

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coffee cup calorimeter heat changes

Coffee cup calorimetry measures heat changes in reactions and physical changes using an insulated calorimeter. The calorimeter is calibrated and designed to limit heat exchange with the outside environment. That makes it possible to measure the heat taken in or released by a substance more accurately, including the energy content of foods.

In calorimetry, the system is the substance or substances undergoing change. The surroundings are everything else inside the calorimeter, including the solution and any other components that can give heat to the system or absorb heat from it. The measured temperature change is then used to calculate the heat transferred in the process under study.

A simple example helps show the idea. If a hot piece of metal is placed in cool water, heat flows from the metal to the water until both reach thermal equilibrium, or the same temperature. In an ideal calorimeter, no heat is gained or lost by the external environment, so the heat lost by the metal equals the heat gained by the water. The two heat values have the same magnitude, but they point in opposite directions of heat flow.

The same rules apply when a chemical reaction happens in solution. For an exothermic reaction, the reaction gives off heat, and the solution absorbs it, so the solution temperature rises. For an endothermic reaction, the reaction absorbs heat from the solution, so the solution temperature falls. The temperature change, along with the solution mass and specific heat, can be used to find the heat involved.

A coffee cup calorimeter is a simple constant-pressure calorimeter made from two nested polystyrene cups with a loose-fitting lid. It is used for reactions in solution, mostly aqueous solutions, when there is little or no volume change. In this setup, the heat of the reaction, q rxn, and the heat of the solution, q soln, add up to zero. That means the heat released or absorbed by the reaction matches the heat gained or lost by the solution. Because the pressure stays constant, the measured heat change is the enthalpy change.

Coffee Cup Calorimeter Heat Changes

energy basics

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Heat changes in chemical equations show how much energy a reaction releases or absorbs. At constant pressure, the enthalpy of reaction, or ΔHrxn, is equal to the heat exchanged with the surroundings, qp. Because this value depends on how much reactant takes part, it is an extensive property. The size and sign of ΔHrxn also depend on the reaction itself and on the physical states of the substances involved. An exothermic reaction has a negative ΔHrxn value, while an endothermic reaction has a...

constant pressure calorimetry

Coffee cup calorimetry measures heat changes in reactions and physical changes using an insulated calorimeter. The calorimeter is calibrated and designed to limit heat exchange with the outside environment. That makes it possible to measure the heat taken in or released by a substance more accurately, including the energy content of foods. In calorimetry, the system is the substance or substances undergoing change. The surroundings are everything else inside the calorimeter, including the...

constant volume calorimetry

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Bomb calorimetry measures the heat released by reactions that produce a lot of energy, especially combustion reactions. A coffee cup calorimeter works at constant pressure and is useful for reactions in solution. A bomb calorimeter works at constant volume and is used for reactions that make large amounts of heat and gaseous products. The word "bomb" refers to the strong, explosive force some reactions can have. In a bomb calorimeter, the volume does not change, so 94V = 0. That means the...

hess's law

Calculating Reaction Heat with Hess's Law

Calculating reaction heat with Hess's law lets chemists find enthalpy changes without measuring every reaction directly. Some reactions are hard or impossible to test in the lab. Even when a reaction can be measured, it is often easier to calculate the heat change from other known enthalpy values. Hess's law says that if a process can be written as the sum of several stepwise processes, the enthalpy change for the total process equals the sum of the enthalpy changes for the steps. This works...

standard enthalpy of formation

Using Standard Enthalpy Values in Chemistry

Enthalpy changes are often listed for reactions that start and end under the same conditions. Chemists use a standard state as a reference set of conditions for comparing properties. In IUPAC terms, the standard state means 1 bar of pressure and 1 M solutions, but it does not set a temperature. Many thermochemical tables still use 1 atm as the reference pressure. Because the difference between 1 bar and 1 atm is very small, enthalpy change usually stays almost the same. A superscripted o in...

enthalpies of reaction

Calculating reaction heat with Hess's law uses standard enthalpies of formation to find the enthalpy change of a reaction. When the formation values for the reactants and products are known, the overall reaction can be broken into simpler stepwise reactions. This approach helps show how the heat change for the full reaction is built from smaller parts. First, the reactants are thought of as being decomposed into their component elements. The enthalpy change for this step is proportional to the...

key terms and concepts

Explore how a coffee cup calorimeter measures heat changes in solutions, from thermal equilibrium to exothermic and endothermic reactions at constant pressure.

Coffee Cup Calorimeter Heat Changes | JoVE K12

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Coffee Cup Calorimeter Heat Changes

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