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## Physics / Calorimetry

### Physics / Calorimetry

You wrap up in blankets in the winter, hold your hands out to feel the warmth of a fire, and jump when touch any hot object. Why does this happen? What is this thing which you call as heat? You all know that heat is form of energy but how this energy is generated? Each substance is made up of molecules. The molecules in a substance are in a state of random motion. This kinetic energy due to random motion of the molecules of a substance is known as its heat energy. Thus each body possesses heat energy in form of its internal kinetic energy.
Understand the concepts of heat capacity, specific heat capacity and their difference.
When a hot body is mixed (or comes in contact ) with a cold body, heat energy passes from hot body to cold body, till both the bodies attain the same temperature. Example: To cool a glass containing hot milk, place it in cold water. What is this phenomenon known as ? Heat flows from hot milk to cold water until both their temperature are equalized. This process in which Heat energy lost by hot body = heat energy gained by the cold body is known as calorimetry. The study of the heat gained or lost during physical processes and chemical reactions is called calorimetry. It is based on the law of conservation of energy. Learn about calorimeter and understands how the principle of calorimetry is used in your daily life.
Find out the following concepts - Hot water bottles are used for fermentation, In cold countries water is used as heat reservoir for wine and juice bottles to avoid their freezing, the base of cooking pan is made thick.

Exercises
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Exercises
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• ### Calorimetry - SmartTest

A SmartTest on Calorimetry

• Accessed by: 365 Students
• Average Time: 00:06:01
• Average Score: 65.18
• Questions: 46
• Introduction to calorimetry
• Concept of heat and temperature
• Heat ( or thermal capacity)
• Specific heat capacity
• Calorimeter and its principle
• Consequences of high specific heat capacity of water
• Consequences of high and low thermal capacity of water
• Change of phase - melting or fusion, Vaporisation or boiling
• Latent heat and specific latent heat
• Calorimetry review