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Chemistry (181)
CHM 113 (103)
Ron Briggs (24)
Lecture

Heat and Energy

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Department
Chemistry
Course
CHM 113
Professor
Ron Briggs
Semester
Fall

Description
Heat and Energy - Energy: Ability to do work or transfer heat st - Law of Conservation of Energy (1 law of Thermodynamics): Energy cannot be created nor destroyed, but can be changed from one form to another or transferred from one place to another o Types of Energy:  Kinetic Energy (KE) – Energy of motion 2  KE = ½ mv  Thermal energy (gases)  Translation, vibration, rotation of molecules  Potential Energy (PE) – Energy of composition of position  Gravitational PE = mgh 2  Elastic PE = ½ kx  Rest Mass Energy, E = mc 2  Electrostatic PE: interaction of charged particles el=kQ 1 /2  Chemical energy: breaking/forming chemical bonds - Heat (q): energy transfer (and increased particle motion) from a body of higher temperature to one of lower temperature when paced in thermal contact with one another o Units of heat energy: 2 2  Joule (J) – SI unit of energy (1J = 1kg m /s )  calorie (cal) – common non-SI unit (1cal = 4.184 J)  Calorie (Cal) – 1,000 cal (or 1 kcal) - Calorimetry: the measurement of heat flow. Performed with a calorimeter.  q = Csp * m * ΔT  q = quantity of heat transferred  Csp = specific heat of substance  m = mass of sample  ΔT = Temperature chang
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