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The capability of a substance to absorb heat energy
The high heat capacity of water has many uses. Commercial nuclear reactors release large amounts of thermal energy (heat) during radioactive decay of fission products. The heat is quickly transferred to a pool of water to cool the reactor. The water then remains hot for a long time due to its high heat capacity.
The capability for a molecule to absorb heat energy is called heat capacity, which can be calculated by the equation shown in the figure . Water's high heat capacity is a property caused by hydrogen bonding among water molecules. When heat is absorbed, hydrogen bonds are broken and water molecules can move freely. When the temperature of water decreases, the hydrogen bonds are formed and release a considerable amount of energy. Water has the highest specific heat capacity of any liquid. Specific heat is defined as the amount of heat one gram of a substance must absorb or lose to change its temperature by one degree Celsius. For water, this amount is one calorie, or 4.184 Joules. As a result, it takes water a long time to heat and a long time to cool. In fact, the specific heat capacity of water is about five times more than that of sand. This explains why the land cools faster than the sea.
The resistance to sudden temperature changes makes water an excellent habitat, allowing organisms to survive without experiencing wide temperature fluctuation. Furthermore, because many organisms are mainly composed of water, the property of high heat capacity allows highly regulated internal body temperatures. For example, the temperature of your body does not drastically drop to the same temperature as the outside temperature while you are skiing or playing in the snow. Due to its high heat capacity, water is used by warm blooded animals to more evenly disperse heat in their bodies; it acts in a similar manner to a car's cooling system, transporting heat from warm places to cool places, causing the body to maintain a more even temperature.
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“Water’s High Heat Capacity.”
Boundless, 08 Aug. 2016.
Retrieved 26 Mar. 2017 from