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When two systems at different temperatures are linked together, heat flows from the higher temperature to the lower temperature until their temperatures become the same. The principle of calorimetry states that heat lost by a body at higher temperature equals heat gained by a body at lower temperature, ignoring heat loss to surroundings.
- Thermodynamics Class 11 Notes CBSE Physics Chapter 11 [PDF] - Vedantu
Download Thermodynamics CBSE Class 11 Physics Chapter 11...
- Thermodynamics Class 11 Notes CBSE Physics Chapter 11 [PDF] - Vedantu
We can begin studying thermal properties of matter with definitions of temperature and heat. Temperature is a relative measure, or indication of hotness or coldness. A hot utensil is said to have a high temperature, and ice cube to have a low temperature.
Heat capacity of any body is equal to the amount of heat energy required to increase its temperature through 1°C. Heat capacity = me where c = specific heat of the substance of the body and m = mass of the body. Its SI unit is joule/kelvin (J/K). Water Equivalent
The specific heat capacity (also referred to as specific heat) of a substance is the amount of heat required to raise the temperature of a unit mass of substance through 1 °C. It is measured in cal g -1 (°C) -1 or J kg -1 K -1 .
Download Thermodynamics CBSE Class 11 Physics Chapter 11 notes PDF for free. Secure good marks by referring NCERT Class 11 Thermodynamics revision notes prepared by Vedantu experts.
Download Thermal Properties of Matter CBSE Class 11 Physics Chapter 10 notes PDF for free. Secure good marks by referring NCERT Class 11 Thermal Properties of Matter revision notes prepared by Vedantu experts.
As an application of Eq. (11.3), consider the change in internal energy for 1 g of water when we go from its liquid to vapour phase. The measured latent heat of water is 2256 J/g. i.e., for 1 g of water ∆Q = 2256 J. At atmospheric pressure, 1 g of water has a volume 1 cm3 in liquid phase and 1671 cm3 in vapour phase.
