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IX Thermodynamics Calorimetry

IX Thermodynamics Calorimetry - Thermodynamics Calorimetry...

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Thermodynamics Calorimetry
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Heat (Q,q) Transfer of thermal energy between two bodies at different temperatures Isolated system No exchange of matter or energy with the surroundings Q = ? Q = 0 Heat flow Endothermic, Q = +, heat absorbed by the system Exothermic, Q = -, heat given off by the system
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Calorimetry Deals with the transfer of heat energy Heat Capacity - Capacity of a system to store heat - Heat needed to raise the temperature of a system by 1 o C ( 1K) = J/K q = (capacity of system)( T) Specific Heat (c) - Heat needed to raise the temperature of 1 gram of material by 1 o C (1K) = J/g K Molar Heat Capacity (C) - Heat needed to raise the temperature of 1 mole of material by 1 o C (1K) = J/ mol K q = ms T q = nC T
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Constant volume Calorimetry Bomb Calorimeter Q = E Isolated system q system = ? = 0 q system = q sample + q calorimeter q sample = - q calorimeter q sample not directly measurable q calorimeter can be measured q calorimeter = heat capacity of bomb( T) = - q sample Since reaction carried out at constant volume q sample = E
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