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Changes

Changes. Exothermic vs. Endothermic. Changes. Exothermic vs Reaction that releases heat. Endothermic-Absorbs heat. Heat versus temperature. HEAT (q) Measure of the total energy in a substance

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Changes

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  1. Changes • Exothermic vs • Endothermic

  2. Changes • Exothermic vs • Reaction that releases heat • Endothermic-Absorbs heat

  3. Heat versus temperature HEAT (q) • Measure of the total energy in a substance • Sum of energy of all particles(kinetic energy and potential energy) • Units: Joule (kgxm2/s2) kJ TEMPERATURE • Related to the Average KE of particles in a sample • Units: K or C

  4. 3 things that the quantity of heat transferred are dependent on: • Nature of the material changing temperature • Mass of the material changing temperature • Size of temperature change

  5. Specific heat • Amount of energy needed to raise the temp of 1 g of a substance 1 C (a calorie is the amount of heat required to raise the temperature of 1 g of H2 O 1 C) 1 cal=4.184 J • Helps you to determine how many joules or calories it takes a known mass of something to change from one temperature to another • Symbol: cp • Unit: J/(g.K) • Formula: cp= q/mT • q-amt of energy lost or gained • m-mass • T= temperature change

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