Name: heat transfer and specific heat
Uploaded: 2025-06-17T07:55:58.000Z
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K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Energy

PS.Chm.7.2

Quantifying Heat

A energia interna é definida pela interconversão de calor e trabalho. Mas como é medido o calor. Todas as substâncias possuem energia térmica.Quando um sistema experimenta uma diferença de temperatura com o seu meio ambiente, a energia térmica flui da matéria com a temperatura mais elevada para a matéria com a temperatura mais baixa. Esta transferência da energia térmica da energia térmica é também chamada de transferência de calor e é medida em Joules. A temperatura, por outro lado, descreve uma propriedade da energia térmica e é medida em Celsius ou Kelvin.Assim, a temperatura é independente da substância, ao contrário do calor, que depende do número e do tipo de moléculas num sistema. O calor pode ser medido por uma técnica chamada de calorimetria, que utiliza a relação entre o calor e uma alteração na temperatura de um sistema. Quando um pedaço de ferro a 114 graus Celsius é colocado em água à temperatura ambiente, o calor flui do ferro para a água até que estejam à mesma temperatura.Uma vez que não há fluxo líquido de calor, estão em equilíbrio térmico. Num sistema isolado, a água ganha exatamente o mesmo calor que o ferro perde. Mas a temperatura final é de apenas um grau acima da temperatura inicial da água, enquanto o ferro arrefeceu 93 graus Celsius.A quantidade de calor transferida é proporcional à alteração de temperatura delta T.A constante de proporcionalidade C ou a capacidade calorífica"é a quantidade de calor necessária para aumentar uma temperatura do sistema por um kelvin, ou um grau Celsius. A capacidade calorífica depende do tipo da substância:um sistema com uma grande capacidade térmica como a água precisa de absorver mais calor para aumentar a sua temperatura do que um sistema com uma capacidade térmica menor, como o ferro. A capacidade calorífica também depende da massa da substância.Capacidade calorífica específica, Cs, ou capacidade calorífica molar, Cm, descreve a quantidade de calor necessária para aumentar a temperatura de 1 grama, ou 1 mol de uma substância por 1 grau Celsius. Assim a unidade é dada em Joules por grama de grau Celsius, ou em Joules por mol de grau Celsius. Assim, se as capacidades específicas de calor e de temperatura são conhecidas as alterações de um sistema, o valor do calor pode ser calculado a partir do seu produto.

quantificação do calor

<h4>Energia Térmica </h4>

Microscopicamente, a energia térmica é a energia cinética associada ao movimento aleatório de átomos e moléculas. A temperatura é uma medida quantitativa de “quente” ou “frio”, que depende da quantidade de energia térmica. Quando os átomos e moléculas em um objeto se movem ou vibram rapidamente, eles têm uma energia cinética média (KE) mais alta (ou energia térmica mais alta), e o objeto é percebido como “quente”, ou é descrito como estando a uma temperatura mais alta. Quando os átomos e moléculas se movem lentamente, eles têm KE média mais baixa (ou energia térmica mais baixa), e o objeto é percebido como “frio”, ou é descrito como estando a uma temperatura mais baixa. 

Partindo do princípio de que não ocorre qualquer reação química ou mudança de fase (como fusão ou vaporização), aumentar a quantidade de energia térmica em uma amostra de matéria fará com que a sua temperatura aumente, enquanto que diminuir a quantidade de energia térmica em uma amostra de matéria fará com que a sua temperatura diminua.

<h4>Calor</h4>

O calor (q) é a transferência de energia térmica entre dois corpos a temperaturas diferentes. O fluxo de calor aumenta a energia térmica de um corpo e diminui a energia térmica do outro. O calor flui espontaneamente do quente para o frio (ou seja, apenas uma direção) e continua até que as duas substâncias estejam à mesma temperatura. As alterações no calor são medidas através de alterações na temperatura. 

A unidade SI de calor, trabalho, e energia é o joule. Um joule (J) é definido como a quantidade de energia utilizada quando uma força de 1 newton move um objecto 1 metro. Tem o seu nome em honra do físico Inglês James Prescott Joule. Um joule equivale a 1 kg m2/s2, que também é chamado de 1 newton–metro. Um quilojoule (kJ) são 1000 joules. Para padronizar a sua definição, uma caloria foi definida como sendo igual a 4,184 joules.

<h4>Transferência de Energia Térmica</h4>

A capacidade térmica (C) de um corpo de matéria é a quantidade de calor (q) que ele absorve ou liberta quando sofre uma mudança de temperatura (ΔT) de 1 grau C (ou equivalentemente, 1 kelvin):

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-01.png" style="height: 40px;" />

A capacidade térmica é determinada tanto pelo tipo como pela quantidade de substância que absorve ou liberta calor. Portanto, a capacidade térmica é uma propriedade extensa — o seu valor é proporcional à quantidade da substância. Por exemplo, considere as capacidades de calor de duas frigideiras de ferro fundido. A capacidade térmica da frigideira grande é cinco vezes maior do que a da frigideira pequena porque, embora ambas sejam feitas do mesmo material, a massa da frigideira grande é cinco vezes maior do que a massa da frigideira pequena. Mais massa significa que mais átomos estão presentes na frigideira maior, por isso é preciso mais energia para fazer todos esses átomos vibrarem mais rapidamente. A capacidade térmica da frigideira de ferro fundido pequena é encontrada ao observar que são necessários 18.140 J de energia (q) para aumentar a temperatura da frigideira em 50,0 °C (ΔT):

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-02.png" style="height: 40px;" />

A frigideira de ferro fundido maior, feita com a mesma substância, requer 90.700 J de energia (q) para aumentar a sua temperatura em 50,0 °C (ΔT). A frigideira maior tem uma capacidade térmica (proporcionalmente) maior porque a maior quantidade de material requer uma quantidade (proporcionalmente) maior de energia para produzir a mesma alteração de temperatura:

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-03.png" style="height: 40px;" />

A capacidade térmica específica (c) de uma substância, geralmente designada por “calor específico”, é a quantidade de calor necessária para aumentar a temperatura de 1 grama de uma substância em 1 grau Celsius (ou 1 kelvin): 

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-04.png" style="height: 40px;" />

A capacidade térmica específica depende apenas do tipo de substância que absorve ou liberta calor. É uma propriedade intensiva—por isso não depende da quantidade da substância. Por exemplo, a frigideira de ferro fundido pequena tem uma massa de 808 g. O calor específico do ferro (o material utilizado para preparar o recipiente) é, por conseguinte:

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-05.png" style="height: 40px;" />

A frigideira grande tem uma massa de 4040 g. Utilizando os dados para esta frigideira, também podemos calcular o calor específico do ferro: 

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-06.png" style="height: 40px;" />

Embora a frigideira grande seja mais maciça do que a frigideira pequena, uma vez que ambas são feitas do mesmo material, ambas produzem o mesmo valor de calor específico (para o material de construção, ferro). Observe que o calor específico é medido em unidades de energia por temperatura por massa e é uma propriedade intensiva, sendo derivado de uma relação de duas propriedades extensivas (calor e massa). A capacidade térmica molar, também uma propriedade intensiva, é a capacidade térmica por mole de uma determinada substância e tem unidades de J/mol⋅°C.

A água tem um calor específico relativamente elevado (cerca de 4,2 J/g⋅°C para o líquido e 2,09 J/g⋅°C para o sólido); a maioria dos metais tem um calor específico muito mais baixo (geralmente menos de 1 J/g⋅°C). Sabendo a massa (m) de uma substância e o seu calor específico (c), pode-se determinar a quantidade de calor, q, que entra ou sai da substância, medindo a variação de temperatura (ΔT) antes e depois de o calor ser ganho ou perdido: 

<img alt="Eq7" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-07v3.png" style="height: 20px;" />

<img alt="Eq8" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-08v4.png" style="height: 20px;" />

Se uma substância ganhar energia térmica, a sua temperatura aumenta, a sua temperatura final é superior à temperatura inicial, Tfinal − Tinicial tem um valor positivo, e o valor de q é positivo. Se uma substância perder energia térmica, a sua temperatura diminui, a temperatura final é inferior à temperatura inicial, Tfinal − Tinicial tem um valor negativo, e o valor de q é negativo.

Observe que a relação entre calor, calor específico, massa, e mudança de temperatura pode ser usada para determinar qualquer uma dessas quantidades (não apenas calor) se as outras três forem conhecidas ou puderem ser deduzidas.

Este texto é adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/5-1-energy-basics">OpenStax Chemistry 2e, Section 5.1: Energy Basics</a> e <a href="https://openstax.org/books/chemistry-2e/pages/5-3-enthalpy">OpenStax Chemistry 2e, Section 5.3: Enthalpy</a>.

Quantificação do Calor

Calor 

Microscopicamente, a energia térmica é a energia cinética associada ao movimento aleatório de átomos e moléculas. A temperatura é um ...

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heat transfer and specific heat

Heat transfer and specific heat explain how thermal energy moves and how materials respond to it. Thermal energy is the kinetic energy linked to the random motion of atoms and molecules. Temperature is a measure of how hot or cold a substance is, and it depends on how much thermal energy those particles have.

When atoms and molecules move or vibrate faster, their average kinetic energy is higher. That means the object has more thermal energy and a higher temperature. When they move more slowly, the thermal energy is lower and the temperature drops. If no chemical reaction or phase change, such as melting or vaporizing, occurs, adding thermal energy raises temperature and removing it lowers temperature.

Heat, written as q, is the transfer of thermal energy between two bodies at different temperatures. Heat flow increases the thermal energy of one body and decreases the thermal energy of the other. It moves spontaneously from hot to cold and continues until both substances reach the same temperature. Changes in heat are tracked by changes in temperature.

The SI unit for heat, work, and energy is the joule. One joule is the energy used when a force of 1 newton moves an object 1 meter. It is also equal to 1 kg m^2/s^2, or 1 newton-meter. A kilojoule is 1000 joules, and one calorie is defined as 4.184 joules.

Heat capacity, C, tells how much heat a body absorbs or releases when its temperature changes by 1 degree C, or 1 kelvin. It depends on both the type of substance and the amount present, so it is an extensive property. A large cast iron frying pan has a heat capacity five times greater than a small one because it has five times more mass. More mass means more atoms, so more energy is needed to make all of them vibrate faster.

The small cast iron frying pan in the example takes 18,140 J of energy to rise by 50.0 °C. The larger pan needs 90,700 J to rise by the same amount. Even though both pans are made of the same material, the larger one needs proportionally more energy because it contains more matter.

Specific heat capacity, often called specific heat, is the heat needed to raise 1 gram of a substance by 1 degree Celsius, or 1 kelvin. It depends only on the kind of substance, so it is an intensive property. Using the mass and temperature change of the small pan, the specific heat of iron can be calculated. The large pan gives the same result, even though its mass is greater.

Specific heat is measured in units of energy per temperature per mass. Because it is a ratio of heat and mass, it is intensive even though those two quantities are extensive. The molar heat capacity is another intensive property. It is the heat capacity per mole of a substance and has units of J/mol·°C.

Water has a relatively high specific heat, about 4.2 J/g·°C for liquid water and 2.09 J/g·°C for solid water. Most metals have much lower specific heats, usually less than 1 J/g·°C. If the mass of a substance, its specific heat, and its temperature change are known, the amount of heat entering or leaving it can be found. A positive q means thermal energy is gained and temperature rises. A negative q means thermal energy is lost and temperature falls.

Heat Transfer and Specific Heat

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Heat Transfer and Specific Heat

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