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Thermochemistry

Explore how energy flows in chemical reactions, the concepts of exothermic and endothermic processes, and units for measuring heat flow. Learn how substances heat up or cool down based on their composition.

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Thermochemistry

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  1. Thermochemistry Chapter 17 Chemistry

  2. Section 1 - The Flow of Energy — Heat and Work Introduction • The temperature of lava from a volcano ranges from 550°C to 1400°C. • As lava flows, it loses heat and begins to cool. • You will learn about heat flow and why some substances cool down or heat up more quickly than others.

  3. 17.1 1. Energy Transformations • Energy is the capacity to do work or supply heat. • Energy has neither mass nor volume. • Thermochemistry is the study of energy changes that occur during chemical reactions and changes in state. • The energy stored in the chemical bonds of a substance is called chemical potential energy. • The kinds of atoms and their arrangement in the substance determine the amount of energy stored. • Heat, represented by q, is energy that transfers from one object to another because of a temperature difference between them. • Heat always flows from a warmer object to a cooler object. When fuel is burned in a car engine, chemical potential energy is released and is used to do work.

  4. 2. Exothermic and Endothermic Processes • In studying energy changes, you can define a system as the part of the universe on which you focus your attention. • The surroundings include everything else in the universe. • Together the system and its surroundings make up the universe. • The law of conservation of energystates that in any chemical or physical process, energy is neither created nor destroyed.

  5. Exothermic and Endothermic Processes (cont.) • An endothermic processis one that absorbs heat from the surroundings. • In an endothermic process, the system gains heat as the surroundings cool down. • q has a positive value because heat is flowing into the system. • An exothermic processis one that releases heat to its surroundings. • In an exothermic process, the system loses heat as the surroundings heat up. • q has a negative value because heat is flowing out of the system.

  6. 17.1 3. Units for Measuring Heat Flow • Heat flow is measured in two common units, the calorie and the joule. • A calorie (cal) is defined as the quantity of heat needed to raise the temperature of 1g of pure water by 1⁰C. • The word calorie is written with a small c except when referring to the energy contained in food. • The energy in food is usually expressed in Calories. • The joule is the SI unit of energy • One joule of heat raises the temperature of 1g of pure water by 0.2390⁰C 1 J = 0.2390 cal 4.184 J = 1 cal

  7. 4. Heat Capacity and Specific Heat • The heat capacity of an object depends on both its mass and its chemical composition. • The greater the mass the greater the heat capacity. • The amount of heat needed to increase the temperature of an object exactly 1°C is the heat capacity of that object. • The specific heat capacity, or simply the specific heat, of a substance is the amount of heat it takes to raise the temperature of 1 g of the substance 1°C.

  8. Heat Capacity and Specific Heat (cont.) • Example: • Step 1: • Step 2:

  9. END OF SECTION 1

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