Energy Transfer and Thermal Equilibrium

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Presentation transcript:

Energy Transfer and Thermal Equilibrium Unit 9 Energy Transfer and Thermal Equilibrium

Energy and Temperature Kinetic Energy Increases with temperature 𝑞=𝑚𝑐Δ𝑇

Heat (energy) is necessary to melt ice and boil water Changes of State Endothermic Process Heat (energy) is necessary to melt ice and boil water

Heat (energy) is produced when condensation or freezing occurs Changes of State Exothermic Process Heat (energy) is produced when condensation or freezing occurs

Energy and Phase Changes Fusion  Heat absorbed converting solid to liquid Solid + Heat Liquid

Energy and Phase Changes Vaporization  Heat absorbed converting liquid to gas Liquid + Heat Gas

Energy and Phase Changes q  heat absorbed or consumed c  specific heat in specified physical state m  mass DT  change in temperature DHfusion  heat of fusion(melting) DHvap  heat of vaporization (boiling)

Sample Problem Calculate how much energy it takes to convert 50 g of ice @ -45 ˚C to steam @ 170 ˚C. Cice = 2.09 J/(g ˚C) DHfus = 334 J/g Cwater = 4.18 J/(g ˚C) DHvap = 2260 J/g Csteam = 2.03 J/(g ˚C)