A principle is a fundamental truth or law that serves as the foundation for a system of belief or behavior. In science, it refers to a basic rule that explains how natural phenomena occur. Principles guide understanding and application in fields like physics mathematics and engineering.
Chapter 10 of Class 11 Physics focuses on the thermal properties of matter including heat temperature and the behavior of substances under thermal expansion. It explores concepts like specific heat capacity thermal conductivity and the principles of calorimetry. The chapter also discusses practical applications like thermometers and real-life examples of heat transfer.
Calorimetry is the science and technique of measuring heat transfer in chemical reactions and changes of state or heat capacity in substances. Calorimetry is the process used in quantifying the heat absorbed or released in a reaction or phase change – typically using an apparatus known as a calorimeter.
Calorimetry Principle:
The principle of calorimetry is based on the law of conservation of energy, which states that energy cannot be created or destroyed, only transformed from one form to another. In calorimetry, the heat lost or gained by the system is equal to the heat gained or lost by the surroundings (if isolated), and this heat change is measured.
Mathematically, it can be expressed as:
Qₗₒₛₜ = Q₉ₐᵢₙₑₔ
Where:
– Qₗₒₛₜ is the heat energy lost by the hot object (or substance),
– Q₉ₐᵢₙₑₔ is the heat energy gained by the cold object (or surroundings).
In calorimetry, the amount of energy change or heat flow is usually determined from the degree of temperature change in a measured mass of the substance, using the formula:
Q = mcΔT
Where:
– Q = Heat energy absorbed or released (in joules, J),
– m = Mass of the substance (in kilograms or grams),
– c = Specific heat capacity of the substance (in J/kg·°C or J/g·°C),
– ΔT = Change in temperature (in °C or K).
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