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Compared to water, most metals have low specific heats. True or false?
Weegy: Specific Heat The specific heat is the amount of heat per unit mass required to raise the temperature by one degree Celsius. [ The relationship between heat and temperature change is usually expressed in the form shown below where c is the specific heat. The relationship does not apply if a phase change is encountered, because the heat added or removed during a phase change does not change the temperature. Q= CM(delta T) Q= heat added C= specific heat M= mass delta T= the change in temp. The specific heat of water is 1 calorie/gram °C = 4.186 joule/gram °C which is higher than any other common substance. As a result, water plays a very important role in temperature regulation. The specific heat per gram for water is much higher than that for a metal, as described in the water-metal example. For most purposes, it is more meaningful to compare the molar specific heats of substances. The molar specific heats of most solids at room temperature and above are nearly constant, in agreement with the Law of Dulong and Petit. At lower temperatures the specific heats drop as quantum processes become significant. The low temperature behaviour is described by the Einstein-Debye model of specific heat. Source(s): ] (More)
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