Name: coffee cup calorimeter heat changes
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North Carolina K-12 Science Standard Course of Study

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PS.Chm.7.2

Constant Pressure Calorimetry

Pour une réaction chimique réalisée sous pression constante, telle que la pression atmosphérique, la chaleur échangée pendant le processus est mesurée comme le changement d'enthalpie delta H.Le changement d'enthalpie pour la réaction se manifeste par un changement de température, qui est mesuré en utilisant une technique appelée calorimétrie. En calorimétrie, la réaction est exécutée dans un récipient scellé et étalonné appelé calorimètre. Le calorimètre est bien isolé et empêche tout flux de chaleur entre lui et son environnement.Ainsi, la chaleur échangée entre les réactifs et les produits-qui constituent le système-et le calorimètre qui est l'environnement-peut être calculée avec précision en surveillant les changements ultérieurs de la température dans le calorimètre. Si la réaction est exothermique, la chaleur s'écoule du système dans l'environnement et la température augmente. Inversement, si la réaction est endothermique, la chaleur s'écoule de l'environnement dans le système, provoquant la chute de la température du calorimètre.Un calorimètre de tasse de café simple mesure le changement d'enthalpie d'une réaction se produisant dans une solution, dans des conditions de pression constante. Le calorimètre se compose de deux tasses à café en mousse de polystyrène imbriquées et équipées d'un thermomètre et d'un agitateur. Le calorimètre est fermé avec un couvercle en liège lâche pour maintenir des conditions de pression constante qui est ouverte à l'atmosphère.Supposons que 50, 0 millilitres chacun d'acide chlorhydrique aqueux 1, 0 molaire et d'hydroxyde de potassium aqueux 1, 0 molaire, réagissent dans le calorimètre, pour augmenter la température de la solution de 6, 9 degrés Celsius. La chaleur absorbée par la solution solution q-est égale à sa chaleur spécifique, C s, 4, 18 joules par gramme de degré celsius-identique à celle de l'eau multipliée par sa masse totale, m-100, 0 grammes, et le changement de température. La chaleur de la solution est 2, 9 fois dix à la puissance de 3 joules ou 2, 9 kilojoules.La chaleur de la réaction réaction q a la même valeur mais avec un signe opposé. Parce que la pression est constante, le changement d'enthalpie est le même que la chaleur de la réaction. Pour trouver le changement d'enthalpie de la réaction par mole, l'enthalpie est divisée par le nombre de moles d'acide chlorhydrique.Les taupes d'acide chlorhydrique sont trouvées en multipliant le volume en litres 0, 05 L avec la molarité 1 molaire. Par conséquent, négatif 2, 9 kilojoules divisé par 0, 050 moles donne négatif 58-kilo joules par mole.

<ol>
	<li>Banna, M. Salim. « Un appareil de chauffage pour la calorimétrie à pression constante. » Journal of Chemical Education 63, n° 11 (1986) : 997.</li>
	<li>Ruekberg, Ben. « Un calorimètre étudiant économique, sûr et robuste. » Journal de l’éducation chimique 71, n° 4 (1994) : 333.</li>
	<li>Stankus, John J., et Jennifer D. Caraway. « Remplacement des calorimètres de tasse de café par des calorimètres à bécher fabriqués. » Journal of Chemical Education 88, n° 12 (2011) : 1730-1731. 
	 </li>
</ol>

calorimétrie à pression constante

La calorimétrie est une technique utilisée pour mesurer la quantité de chaleur impliquée dans un processus chimique ou physique ou pour mesurer la chaleur transférée à une substance ou à partir d'une substance. La chaleur est échangée avec un dispositif isolé et étalonné appelé calorimètre. Les expériences de calorimétrie reposent sur la supposition qu'il n'y a pas d'échange thermique entre le calorimètre isolé et l'environnement externe. Les calorimètres bien isolés empêchent le transfert de chaleur entre le calorimètre et l'environnement externe, ce qui limite effectivement “ l'environnement ” aux composants hors système à l'intérieur du calorimètre (et le calorimètre lui-même). Cela permet de déterminer avec exactitude la chaleur impliquée dans les processus chimiques, comme la teneur en énergie des aliments.  
 
 Le changement de température mesuré par le calorimètre est utilisé pour déduire la quantité de chaleur qui est transférée par le processus étudié. Dans un calorimètre, un système est défini comme la ou les substances qui subissent la transformation chimique ou physique, ou en d'autres termes, la réaction, et l'environnement est toute autre matière, y compris la solution et tous les autres composants du calorimètre qui fournissent de la chaleur au système ou absorbent la chaleur du système. 
 
 Avant de discuter de la calorimétrie des réactions chimiques, considérons un exemple plus simple qui illustre l'idée sur laquelle se base la calorimétrie. Supposons qu'un morceau de métal chaud à haute température soit placé dans une substance à basse température, telle que l'eau froide. La chaleur se propage du métal chaud vers l'eau. La température du métal diminue et la température de l'eau augmente jusqu'à ce que les deux substances aient la même température, c'est-à-dire lorsqu'elles atteignent l'équilibre thermique. Si cela se produit dans un calorimètre, toute la chaleur est transférée entre les deux substances, sans qu'aucune chaleur ne soit reçue ni perdue par son environnement externe. Dans ces circonstances idéales, la variation de chaleur nette est nulle : 
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/798/798_Equations-01.png" style="height: 40px;" />
 
 Cette relation peut être réorganisée pour montrer que la chaleur reçue par le métal est égale à la chaleur perdue par la substance l'eau : 
 
 <img alt="Eq2" src="https://www.jovecore.com/CDNSource/lessons/798/798_Equations-02.png" style="height: 40px;" />
 
 L'ampleur de la (variation de) chaleur est donc la même pour les deux substances. Le signe négatif montre simplement que qmétal et qeau sont opposés dans la direction du flux de chaleur (gain ou perte), mais il n'indique pas le signe arithmétique de l'une ou l'autre valeur de q (qui, par définition, est déterminé selon que la matière en question reçoit ou perd de la chaleur). Dans la situation spécifique décrite, qmétal est une valeur négative et qeau est une valeur positive puisque la chaleur est transférée du métal à l'eau. 
 
 Lors de l'utilisation de la calorimétrie pour déterminer la chaleur impliquée dans une réaction chimique, les mêmes principes s'appliquent. La quantité de chaleur absorbée par le calorimètre est souvent assez petite pour qu'elle soit souvent négligée, et le calorimètre minimise l'échange d'énergie avec l'environnement extérieur. Lorsqu'une réaction exothermique se produit en solution dans un calorimètre, la chaleur produite par la réaction est absorbée par la solution, ce qui augmente sa température. Lorsqu'une réaction endothermique se produit, la chaleur nécessaire est absorbée à partir de l'énergie thermique de la solution, ce qui diminue sa température. Le changement de température (ΔT), ainsi que le chaleur spécifique (csoln) et la masse de la solution (msoln), peuvent ensuite être utilisés pour calculer la quantité de chaleur (qsoln) impliquée dans les deux cas. 
 
 <img alt="Eq3" src="https://www.jovecore.com/CDNSource/lessons/798/798_Equations-03.png" style="height: 40px;" />
 
 Un  calorimètre simple, appelé calorimètre de la tasse à café, est constitué de deux tasses en polystyrène emboîtées et fermées par un couvercle lâche. Les calorimètres de la tasse à café sont utilisés pour mesurer la chaleur des réactions qui ont lieu en solution (principalement des solutions aqueuses) et n'impliquent aucun ou très peu de changement de volume. Comme l’énergie n’est ni créée ni détruite au cours d’une réaction chimique, l'addition de la chaleur produite ou consommée dans la réaction (“ le système ”), qR, plus la chaleur absorbée ou perdue par la solution (“ l'environnement ”), qsoln, doit donner zéro : 
 
 <img alt="Eq4" src="https://www.jovecore.com/CDNSource/lessons/798/798_Equations-04.png" style="height: 40px;" />
 
 Cela signifie que la quantité de chaleur produite ou consommée dans la réaction est égale à la quantité de chaleur absorbée ou perdue par la solution : 
 
 <img alt="Eq5" src="https://www.jovecore.com/CDNSource/lessons/798/798_Equations-05.png" style="height: 40px;" />
 
 Le calorimètre de la tasse à café est un calorimètre à pression constante, et la chaleur de la réaction mesurée est équivalente à la variation d'enthalpie. 
 
 <img alt="Eq6" src="https://www.jovecore.com/CDNSource/lessons/798/798_Equations-06.png" style="height: 40px;" />
 
 Ce texte est adapté de <a href="https://openstax.org/books/chemistry-2e/pages/5-2-calorimetry">Openstax, Chimie 2e, Section 5.2 : Calorimétrie</a>.

Calorimétrie à pression constante

La calorimétrie est une technique utilisée pour mesurer la quantité de chaleur impliquée dans un processus chimique ou physique ou pour mesurer la chaleur transférée vers ou depuis un ...

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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

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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...

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standard enthalpy of formation

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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...

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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.

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Coffee Cup Calorimeter Heat Changes

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