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Explanation:
it will flow through air like air
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Explanation:
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11.2 Heat, Specific Heat, and Heat Transfer
SECTIONS
Learning Objectives
Heat Transfer, Specific Heat, and Heat Capacity
Conduction, Convection, and Radiation
Solving Heat Transfer Problems
Practice Problems
Check Your Understanding
Learning Objectives
By the end of this section, you will be able to do the following:
Explain heat, heat capacity, and specific heat
Distinguish between conduction, convection, and radiation
Solve problems involving specific heat and heat transfer
Section Key Terms
conduction convection heat capacity
radiation specific heat
Heat Transfer, Specific Heat, and Heat Capacity
We learned in the previous section that temperature is proportional to the average kinetic energy of atoms and molecules in a substance, and that the average internal kinetic energy of a substance is higher when the substance’s temperature is higher.
If two objects at different temperatures are brought in contact with each other, energy is transferred from the hotter object (that is, the object with the greater temperature) to the colder (lower temperature) object, until both objects are at the same temperature. There is no net heat transfer once the temperatures are equal because the amount of heat transferred from one object to the other is the same as the amount of heat returned. One of the major effects of heat transfer is temperature change: Heating increases the temperature while cooling decreases it. Experiments show that the heat transferred to or from a substance depends on three factors—the change in the substance’s temperature, the mass of the substance, and certain physical properties related to the phase of the substance.
The equation for heat transfer Q is
11.7
Q = mcΔT,
where m is the mass of the substance and ΔT is the change in its temperature, in units of Celsius or Kelvin. The symbol c stands for specific heat, and depends on the material and phase. The specific heat is the amount of heat necessary to change the temperature of 1.00 kg of mass by 1.00 ºC. The specific heat c is a property of the substance; its SI unit is J/(kg⋅K) or J/(kg⋅°C). The temperature change (ΔT) is the same in units of kelvins and degrees Celsius (but not degrees Fahrenheit). Specific heat is closely related to the concept of heat capacity. Heat capacity is the amount of heat necessary to change the temperature of a substance by 1.00°C. In equation form, heat capacity C is C=mc, where m is mass and c is specific heat. Note that heat capacity is the same as specific heat, but without any dependence on mass. Consequently, two objects made up of the same material but with different masses will have different heat capacities. This is because the heat capacity is a property of an object, but specific heat is a property of any object made of the same material.
Values of specific heat must be looked up in tables, because there is no simple way to calculate them. Table 11.1 gives the values of specific heat for a few substances as a handy reference. We see from this table that the specific heat of water is five times that of glass, which means that it takes five times as much heat to raise the temperature of 1 kg of water than to raise the temperature of 1 kg of glass by the same number of degrees.
Specific Heats of Various Substances.
Substances Specific Heat (c)
Solids J/(kg⋅°C)
Aluminum 900
Asbestos 800
Concrete, granite (average) 840
Copper 387
Glass 840
Gold 129
Human body (average) 3500
Ice (average) 2090
Iron, steel 452
Lead 128
Silver 235
Wood 1700
Liquids
Benzene 1740
Ethanol 2450
Glycerin 2410
Mercury 139
Water 4186
Gases (at 1 atm constant pressure)
Air (dry) 1015
Ammonia 2190
Carbon dioxide 833
Nitrogen 1040
Oxygen 913
Steam 2020
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