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Energy and the Measurement of Heat

It is more difficult to measure energy than it is to measure length, mass, volume, or temperature. But when measured, energy is quantitatively given in the SI unit of the Joule (J) or in the calorie (cal), an older unit used for measuring heat energy. By definition  [Pg.30]

If larger units of energy are needed, the kilojoule (kj) and the kilocalorie (kcal) can be used. [Pg.30]

The amount of heat needed to raise the temperature of 1 gram of a substance 1 °C is called the specific heat (S.H.) of that substance. It requires 4.184 Joules (or 1 calorie) of heat to raise the temperature of 1 gram of water 1°C. It follows, then, that the specific heat of water is 4.184 J/g°C. If you know the amount of heat needed to raise the temperature of 1 g of water 1°C, you can calculate the amount of heat (symbolized, q) needed to raise the temperature of 10 g of water 10°C. The formula for doing just this is  [Pg.31]

how many Joules of heat energy are required to raise the temperature of 10.0 g of water [Pg.31]

Notice that the units of gram and °C cancel, leaving Joule, the unit of energy. This equation can be rewritten in a general way that applies to all substances. AT symbolizes a change in temperature. [Pg.31]


If you answered incorrectly, review Energy and the Measurement of Heat, page 30. [Pg.419]


See other pages where Energy and the Measurement of Heat is mentioned: [Pg.8]    [Pg.30]   


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