Name: how specific heat affects temperature
Uploaded: 2019-03-11T09:21:01.000Z
Duration: 1 min 16 s
Channel: JoVE

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Specific Heat

Specific heat capacity is the amount of heat absorbed by one gram of a substance to raise its temperature by one degree Celsius.
Equal masses of different substances absorb different amounts of heat and have distinct specific heat capacities.
Water has a high specific heat of 1 calorie per gram-degree Celsius and absorbs more energy to increase its temperature than most other substances.&#160;
Heat absorbed by a substance increases the kinetic energy of the molecules and makes them vibrate.
Some of the heat absorbed by water is spent on breaking the hydrogen bonds that connect the water molecules, allowing them to move around. The rest of the absorbed heat increases the kinetic energy of the molecules and raises the water temperature.
When the temperature drops, the hydrogen bonds are formed again and a large quantity of energy is released.
Thus, water absorbs and releases heat without immediate temperature change and takes longer to warm up or cool down.
These properties of water enable it to withstand temperature changes, supporting aquatic life.

specific heat

The specific heat capacity of a substance refers to the energy required to increase the temperature of one gram of that substance by one degree Celcius. Specific heat capacity is often represented in calories (cal), grams (g), and degrees Celsius (oC), but can also be expressed in joules (J), kilograms (kg), and Kelvin (K), among other units.
For example, increasing the temperature of one gram of water by 1&#176;C requires one calorie of heat energy and can be written as 1 cal/g-&#176;C, or 4186 J/kg/K. Water has a high specific heat capacity. It absorbs a large amount of heat to increase its temperature and similarly releases a lot of heat when it cools down. Therefore, it takes significant time for water to heat or cool down.
On the other hand, metals have a low heat capacity and thus heat up quickly and cool down quickly. For example, solid gold has a specific heat capacity of ~0.03 cal/g/&#176;C or 129 J/kg/K, which is much less than water.
<h4>Water has a high specific heat</h4>
When water is boiled, a high amount of energy is absorbed to break the hydrogen bonds between the water molecules. This results in the random movement of water molecules. Similarly, when the water cools down, hydrogen bonds start forming between the water molecules when the water cools down, bringing them closer. An enormous amount of heat is released in this process.&#160;&#160;
<h4>Moderation of environmental temperatures</h4>
The high heat capacity of water helps modulate extreme environmental temperatures. Towns near large bodies of water have more minor temperature changes daily and seasonally. During the day, the nearby water absorbs heat energy, cooling the surrounding land. The water releases its heat energy at night, keeping the area warmer. Towns away from large bodies of water can experience large swings in daily and seasonal temperatures. Since sand and rocks have lower heat capacities, they heat up quickly during the day and rapidly release heat at night.

The specific heat capacity of a substance refers to the energy required to increase the temperature of one gram of that substance by one degree Celcius. ...

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how specific heat affects temperature

Specific heat capacity describes how much energy a substance needs to rise by 1 degree Celsius for each gram. It is often written with calories, grams, and degrees Celsius, but it can also be shown in joules, kilograms, and Kelvin. For water, 1 gram needs 1 calorie to increase by 1°C, which is also written as 1 cal/g-°C or 4186 J/kg/K.

Water has a high specific heat capacity, so it takes in a large amount of heat before its temperature changes much. It also gives off a lot of heat when it cools. That is why water heats up and cools down slowly. Metals have a much lower heat capacity, so they warm up quickly and also lose heat quickly. Solid gold is one example, with a specific heat capacity of about 0.03 cal/g/°C or 129 J/kg/K.

Water’s high specific heat is linked to hydrogen bonds between water molecules. When water is boiled, it absorbs a large amount of energy to break these bonds, which lets the molecules move more freely. When water cools, hydrogen bonds form again and pull the molecules closer together. A large amount of heat is released during this process.

This property also helps control environmental temperatures. Areas near large bodies of water usually have smaller daily and seasonal temperature changes. During the day, the water absorbs heat and cools the nearby land. At night, the water gives off stored heat and keeps the area warmer.

Places far from large bodies of water can have much bigger swings in temperature. Sand and rocks have lower heat capacities, so they heat up quickly in the day. They also release heat quickly at night. This is why water helps moderate climate more than dry land does.

How Specific Heat Affects Temperature

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Specific heat capacity describes how much energy a substance needs to rise by 1 degree Celsius for each gram. It is often written with calories, grams, and degrees Celsius, but it can also be shown in joules, kilograms, and Kelvin. For water, 1 gram needs 1 calorie to increase by 1°C, which is also written as 1 cal/g-°C or 4186 J/kg/K. Water has a high specific heat capacity, so it takes in a large amount of heat before its temperature changes much. It also gives off a lot of heat when it...

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Learn how specific heat capacity controls heating and cooling, why water changes temperature slowly, and how it helps moderate climate near oceans and lakes.

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How Specific Heat Affects Temperature

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