The Flow of Energy.

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Presentation transcript:

The Flow of Energy

Energy of Transformation Capacity of doing work Supplying heat Heat (q): energy that is transferred from one object to another because of temperature difference Flows from hot  cold Chemical Potential Energy Stored in chemical bonds

Thermochemistry Study of energy changes that occur during chemical reactions and change in state. System: the reaction Surroundings: everything else in the universe Law of Conservation of Energy: energy is neither created or destroyed

System and Surroundings

Types of Thermochemical Rxn. Endothermic Process: absorbs heat from the surroundings Exothermic Process: heat is released to the surroundings

Measuring Heat Calorie Joule = SI unit for energy Amount of energy needed to raise 1g of H20 1ºC 1 Calorie = 1 kilocalorie = 1000 calorie 10g sugar  41 Calories or 41,000 calories Joule = SI unit for energy 1 joule raises 1g H2O 0.2390ºC 1 joule=0.2390cal or 4.184J = 1cal

Heat Capacity Heat Capacity: amount of heat needed to raise the temperature of any object 1ºC aka Specific Heat Depends on mass and chemical composition greater mass  greater the heat capacity On a sunny day, a piece of steel would be too hot to touch while a puddle would be cool

Calculating Specific Heat The temperature of a 95.4g piece of copper increases from 25.0ºC to 48.0ºC when the copper absorbs 849J of heat. What is the specific heat of copper? mCu = 95.4g CCu= ? J/(g·ºC) ΔT= (48.0-25.0)=23.0ºC q = 849J

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