When two bodies (one being solid and other liquid or both being liquid) at different temperatures are related, heat will be gone from body at higher temperature to body at lower temperature till both acquire similar temperature. The object at higher temperature releases heat while body at lower temperature takes it, so that:

            Heat lost = Heat gained,

i.e. principle of calorimetric represents the law of conservation of heat energy.

While, using this principle always keep in mind that:

(a) Temperature of mixture (T) is always ≥ lower temperature (T_L) and ≤ higher temperature (T_H), i.e., T_L ≤ T ≤ Th i.e. the temperature of mixture can never be lesser than lower temperatures (as a body cannot be cooled below the temperature of cooling body) and greater than higher temperature (as a body cannot be heated above the temperature of heating  body when there is no chemical reaction).

(b) When temperature of an object modifies, the body releases heat if its temperature falls and absorbs heat when its temperature arise. The heat absorbed or released by a body of mass m is given by:

                        Q = mc ΔT

(c)  When state of an object changes, change of state takes place at constant temperature and heat absorbed or released is given by

                                    Q = mL

            Heat is absorbed if solid converts into liquid (at m.pt.) or liquid converts into vapors (at b.pt.) and is free if liquid transferred into solid or a vapor converts into liquid.

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