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Chapter 10: Problem 13

What is heat capacity? Explain the difference between heat capacity and specific heat capacity.

Short Answer

Expert verified
Heat capacity is the total heat energy required to raise the temperature of an object by one degree, while specific heat capacity is the heat energy required to raise the temperature of one kilogram of a substance by one degree. The latter is a material-specific intensive property, unlike heat capacity, which is an extensive property dependent on mass.

Step by step solution

01

Understanding Heat Capacity

Heat capacity is defined as the amount of heat energy required to raise the temperature of an object by one degree Celsius (or one Kelvin). It is dependent on the mass and the type of material of the object. Heat capacity is an extensive property, which means it is dependent on the amount of the substance.
02

Understanding Specific Heat Capacity

Specific heat capacity is defined as the amount of heat energy required to raise the temperature of one kilogram of a substance by one degree Celsius (or one Kelvin). This is an intensive property, meaning it is independent of the mass of the substance and is a characteristic of the material itself.
03

Comparing Heat Capacity and Specific Heat Capacity

The difference between heat capacity and specific heat capacity is that heat capacity is an extensive property and is dependent on the mass of the substance, whereas specific heat capacity is an intensive property and is independent of the mass. To get the heat capacity from the specific heat capacity, one needs to multiply the specific heat capacity by the mass of the substance.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Specific Heat Capacity
Imagine you have a cup of hot tea and a swimming pool, both at the same temperature. If you wanted to increase their temperatures by the same amount, intuitively, you'd need a lot more energy for the pool. This is where the concept of specific heat capacity comes into play. It's a measure of how much energy is needed to raise the temperature of a unit mass of a substance by one degree Celsius (or one Kelvin).

Different materials absorb heat differently 鈥� for instance, it takes less energy to heat up a kilogram of copper than it does for a kilogram of water. This unique characteristic is vital in numerous applications, from designing heating systems to understanding climate dynamics.
Extensive Property
An extensive property is a physical quantity that changes when the size of the sample changes. In simpler terms, the bigger the size, the higher the value. Let's consider an example: If you have a large pizza, it has more calories than a smaller one because of its size. Similarly, heat capacity is an extensive property and thus depends on the mass of the substance you're considering.

Understanding extensive properties is crucial because it allows us to predict how a system will behave when its size is altered. It also helps differentiate between intrinsic qualities of materials and those dependent on quantity.
Intensive Property
Now, think about the color of the pizza, regardless of whether you have one slice or ten, the color remains the same. This is what an intensive property is like 鈥� it doesn't depend on the amount of the substance present. Specific heat capacity is an intensive property, so no matter how much of the substance you have, the amount of heat needed to raise its temperature by one degree per unit mass remains constant.

This makes intensive properties particularly useful for identifying substances and comparing their intrinsic qualities, as they provide a standard measure unaffected by the sample's size.
Temperature Change
Dealing with temperature change is another way to assess how substances interact with thermal energy. When energy is transferred to an object, its temperature typically rises. However, the rate at which this happens differs depending on the material. What we measure as temperature is actually a representation of the average kinetic energy of the particles within a substance.

The relevance of temperature change is far-reaching, impacting everything from meteorology to the design of thermal insulation in buildings. By understanding how different substances respond to energy, we can develop more efficient ways to manage thermal processes.
Thermal Energy
At the root of these concepts is thermal energy, the total kinetic energy of the particles in a substance due to their motion. It's what you feel as heat. This energy can be transferred from one object to another, resulting in temperature changes. For example, when you heat a pot of water, the stove transfers thermal energy to the pot, then the pot to the water, which eventually gets hot.

Comprehension of thermal energy is pivotal because it's the driving force behind the physical changes we observe in temperature. From powering engines to cooking food, mastering the flow and conversion of thermal energy is essential for technological advancement and everyday life.

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Most popular questions from this chapter

Is the change in enthalpy for a reaction an extensive property? Explain the relationship between \(\Delta H\) for a reaction and the amounts of reactants and products that undergo reaction.

Which statement is true of the internal energy of the system and its surroundings following a process in which \(\Delta E_{\mathrm{sys}}\) \(=+65 \mathrm{kJ} ?\) Explain. \begin{equation} \begin{array}{l}{\text { a. The system and the surroundings both lose } 65 \text { kJ of energy. }} \\ {\text { b. The system and the surroundings both gain } 65 \text { kJ of energy. }} \\ {\text { c. The system loses } 65 \text { kJ of energy, and the surroundings gain } 65 \text { kJ of }} \\ {\text { d. The system gains } 65 \text { kJ of energy, and the surroundings lose } 65 \text { kJ of }} \\ {\text { energy. }}\end{array}\end{equation}

What is the law of conservation of energy? How does it relate to energy exchanges between a thermodynamic system and its surroundings?

Explain the difference between an exothermic and an endothermic reaction. Give the sign of \(\Delta H\) for each type of reaction.

Consider the generic reaction: $$\mathrm{A}+2 \mathrm{B} \longrightarrow \mathrm{C}+3 \mathrm{D} \quad \Delta H=155 \mathrm{kJ}$$ Determine the value of \(\Delta H\) for each related reaction: \begin{equation} \begin{array}{l}{\text { a. } 3 \mathrm{A}+6 \mathrm{B} \longrightarrow 3 \mathrm{C}+9 \mathrm{D}} \\ {\text { b. } \mathrm{C}+3 \mathrm{D} \rightarrow \mathrm{A}+2 \mathrm{B}} \\ {\text { c. } \frac{1}{2} \mathrm{C}+\frac{3}{2} \mathrm{D} \longrightarrow \frac{1}{2} \mathrm{A}+\mathrm{B}}\end{array} \end{equation}
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