1. Chapter Seventeen Page 504

2. Assess prior knowledge… What does a thermometer measure? Can a thermometer measure heat?

3. Energy Transformations Energy is the capacity for doing work or supplying heat. Energy is not matter – it is detected because of its effects Thermochemistry is the study of energy changes that occur during chemical changes or changes in state. All matter has a certain amount of energy stored within it. This is referred to as chemical potential energy. It is based on the substance's atomic structure.

4. Energy Transformations (cont'd) Can you think of substances we purchase that house significant chemical potential energy? Energy changes occur as work, heat or a combination of both. Heat (q), is energy that transfers from one object to the next because of temperature differences between the two. Adding heat (energy) causes a rise in the temperature.

5. Heat HEAT ALWAYS FLOWS FROM A WARMER OBJECT TO A COOLER OBJECT. THE BOLD BLACK LETTERS MEANS THE STATEMENT IS REALLY, REALLY IMPORTANT. Does the heat transfer continue indefinitely?

6. Heat Transfer When it comes to heat transfer, the terms system and surroundings are often used The system is the object or part of the universe you focus your attention on The surroundings is everything else (when it comes to heat transfer, it is typically the 'immediate surroundings'). Thermochemistry is concerned with the heat flow between the system and its surroundings. If we rely on the law of conservation of energy, when the system loses energy, the surroundings must gain energy and vice versa.

7. Endothermic Processes The system absorbs heat and the surroundings cool down. Heat is defined as positive (+q). To help you remember, endo- means "within". Exothermic Processes The system releases heat and the surroundings warm up. The heat is defined as negative (-q). The prefix exo- means "outside of" Page 507, Q. 1 - 2

8. Units for Measuring Heat Flow Heat flow is measured in two common units, the calorie (cal) and the joule (J). The joule is the SI unit for energy. One joule of heat raises the temperature of 1g of water 0.2390°C 1 J = 0.2390 cal4.184 J = 1 cal

9. Heat Capacity and Specific Heat The amount of heat needed to raise the temperature of an object by 1°C is called its heat capacity. It depends on its mass and chemical composition. The greater the mass, the greater its heat capacity. Why does the parking lot at Walmart heat up faster than a swimming pool? Specific heat is merely an extension of heat capacity It is the amount of heat it required for 1g of substance to raise its temperature by 1°C. Table 17.1, page 508

10. To calculate specific heat (C): heat (joules or calories) mass (g) x change in temperature (°C) the units of specific heat are then… J/g·°Corcal/g·°C Questions 3-4, 9-11, pg. 510