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

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Chemistry

Energy

PS.Chm.7.2

Constant Pressure Calorimetry

Para uma reação química realizada sob pressão constante, tal como a pressão atmosférica, o calor trocado durante o processo é medido como a alteração na entalpia delta H.A alteração da entalpia para a reação manifesta-se como uma alteração na temperatura, que é medida utilizando uma técnica chamada de calorimetria. Na calorimetria, a reação é executada num recipiente selado e calibrado chamado de calorímetro. O calorímetro está bem isolado e impede qualquer fluxo de calor entre si e o seu ambiente.Assim, o calor trocado entre os reagentes e os produtos-que constituem o sistema e o calorímetro que é o meio ambiente pode ser calculado com precisão através da monitorização das posteriores alterações na temperatura no calorímetro. Se a reação for exotérmica, o calor flui do sistema para o meio ambiente e a temperatura sobe. Inversamente, se a reação for endotérmica, o calor flui do meio ambiente para o sistema, provocando a queda da temperatura no calorímetro.Um simples calorímetro de chávena de café mede a alteração na entalpia de uma reação que ocorre numa solução, em condições de pressão constante. O calorímetro consiste em dois copos de cafés de esferovite juntos e equipados com um termômetro e um agitador. O calorímetro é fechado com uma tampa de cortiça larga de forma a manter as condições de pressão constante que está aberto ao ar.Suponhamos 50, 0 mililitros em cada um de 1, 0 mol de ácido clorídrico aquoso e 1, 0 mol de hidróxido de potássio aquoso, reagem no calorímetro, para aumentar a temperatura da solução em 6, 9 graus Celsius. O calor absorvido pela solução solução q é igual ao seu calor específico, C s, 4, 18 joules por grama de grau celsius igual à da água multiplicada pela sua massa total, m-100, 0 gramas, e a alteração na temperatura. O calor da solução é 2, 9 vezes dez à potência de 3 joules ou 2, 9 kilojoules.O calor da reação reação q tem o mesmo valor mas com um sinal oposto. Porque a pressão é constante, a alteração da entalpia é a mesma que o calor da reação. Para encontrar a alteração da entalpia da reação por mol, a entalpia é dividida pelo número de mols do ácido clorídrico.Os mols do ácido clorídrico são encontrados multiplicando o volume em litros 0, 05 L com a molaridade de 1 mol. Portanto, 2, 9 kilojoules negativos divididos por 0, 050 mols dão 58-kilojoules negativos por mol.

<ol>
	<li>Banna, M. Salim. "Um aquecedor para calorimetria de pressão constante." Jornal de Educação Química 63, nº 11 (1986): 997.</li>
	<li>"Um calorímetro estudantil econômico, seguro e robusto." Jornal de Educação Química 71, nº 4 (1994): 333.</li>
	<li>Stankus, John J. e Jennifer D. Caraway. "Substituição de calorímetros de xícara de café por calorímetros de béquer fabricados." Journal of Chemical Education 88, nº 12 (2011): 1730-1731. 
	 </li>
</ol>

calorimetria de pressão constante

A calorimetria é uma técnica utilizada para medir a quantidade de calor envolvida em um processo químico ou físico ou para medir o calor transferido de ou para uma substância. O calor é trocado através de um aparelho calibrado e isolado chamado calorímetro. As experiências de calorimetria baseiam-se no pressuposto de que não existe troca térmica entre o calorímetro isolado e o ambiente externo. Os calorímetros bem isolados evitam a transferência de calor entre o calorímetro e o seu ambiente externo, o que limita efetivamente as “imediações” aos componentes não-sistema dentro do calorímetro (e o próprio calorímetro). Isto permite a determinação precisa do calor envolvido em processos químicos, como o teor energético dos alimentos. 

A alteração da temperatura medida pelo calorímetro é utilizada para derivar a quantidade de calor transferida pelo processo em estudo. Em um calorímetro, um sistema é definido como a substância ou substâncias sujeitas a alterações químicas ou físicas ou, por outras palavras, a reação, e as imediações são toda a outra matéria, incluindo a solução e quaisquer outros componentes no calorímetro que fornecem calor ao sistema ou absorvem calor do sistema.

Antes de discutir a calorimetria das reações químicas, considere um exemplo mais simples que ilustra a idéia central por trás da calorimetria. Suponha que um pedaço de metal quente a uma temperatura elevada é colocado em uma substância a baixa temperatura, como água fria. O calor fluirá do metal quente para a água. A temperatura do metal diminuirá e a temperatura da água aumentará até que as duas substâncias tenham a mesma temperatura, ou seja, quando atingirem o equilíbrio térmico. Se isto ocorrer em um calorímetro, todo o calor é transferido entre as duas substâncias, sem que o calor seja obtido ou perdido pelo seu ambiente externo. Nestas circunstâncias ideais, a alteração líquida de calor é zero:

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-01.png" style="height: 40px;" />

Esta relação pode ser reorganizada para mostrar que o calor ganho pelo metal é igual ao calor perdido pela substância água:

<img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-02.png" style="height: 40px;" />

A magnitude do calor (alteração) é, portanto, a mesma para ambas as substâncias. O sinal negativo mostra apenas que qmetal e qágua são opostos na direção do fluxo de calor (ganho ou perda), mas não indica o sinal aritmético de nenhum dos valores de q (que é determinado se a matéria em questão ganha ou perde calor, por definição). Na situação específica descrita, qmetal é um valor negativo e qágua é um valor positivo, uma vez que o calor é transferido do metal para a água.

Ao utilizar a calorimetria para determinar o calor envolvido em uma reação química, aplicam-se os mesmos princípios. A quantidade de calor absorvida pelo calorímetro é muitas vezes suficientemente pequena para que possa ser geralmente negligenciada, e o calorímetro minimiza a troca de energia com o ambiente externo. Quando ocorre uma reação exotérmica em solução em um calorímetro, o calor produzido pela reação é absorvido pela solução, o que aumenta a sua temperatura. Quando ocorre uma reação endotérmica, o calor necessário é absorvido da energia térmica da solução, o que diminui a sua temperatura. A mudança de temperatura (ΔT), juntamente com o calor específico (em>csoln) e a massa (msoln) da solução, pode então ser utilizada para calcular a quantidade de calor (qsoln) envolvida em qualquer dos casos.

<img alt="Eq3" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-03.png" style="height: 40px;" />

Um  calorímetro simples — chamado de calorímetro de xícara de café — é construído a partir de duas xícaras de poliestireno aninhadas fechadas com uma tampa solta. Os calorímetros de xícara de café são utilizados para medir o calor das reações que ocorrem em soluções (na sua maioria soluções aquosas) e não implicam uma alteração de volume ou têm uma alteração de volume muito reduzida. Uma vez que a energia não é criada nem destruída durante uma reação química, o calor produzido ou consumido na reação (o “sistema”), qrxn, mais o calor absorvido ou perdido pela solução (as “imediações”), qsoln, deve ser zero:

<img alt="Eq4" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-04.png" style="height: 40px;" />

Isto significa que a quantidade de calor produzida ou consumida na reação é igual à quantidade de calor absorvida ou perdida pela solução:

<img alt="Eq5" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-05.png" style="height: 40px;" />

O calorímetro de xícara de café é um calorímetro de pressão constante, e o calor medido da reação é equivalente à alteração da entalpia.

<img alt="Eq6" src="https://www.jove.com/files/core/CDNSource/lessons/798/798_Equations-06.png" style="height: 40px;" />

Este texto é adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/5-2-calorimetry">Openstax, Chemistry 2e, Section 5.2: Calorimetry</a>.

Calorimetria de Pressão Constante

A calorimetria é uma técnica usada para medir a quantidade de calor envolvida em um processo químico ou físico ou para medir o calor transferido de ou para um ...

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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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Coffee Cup Calorimeter Heat Changes | JoVE K12

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Coffee Cup Calorimeter Heat Changes

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