Presentation on theme: "Intro Energy. Explain that physical and chemical changes in matter involve transfers of energy. Apply the law of conservation of energy to analyze changes."— Presentation transcript:
Explain that physical and chemical changes in matter involve transfers of energy. Apply the law of conservation of energy to analyze changes in matter. Distinguish between heat and temperature. Convert between the Celsius and Kelvin temperature scales.
Work in small groups to brainstorm ideas relating to energy. List different types of energy, list why energy is important, and when energy is released or absorbed. After brainstorming for five minutes, examine your lists and write your own definition for energy.
What is the energy? Energy is the capacity to do some kind of work, such as moving an object, forming a new compound, transferring heat or generating light.
Energy is always involved when there is a change in matter. All physical and chemical changes involve energy Energy may affect matter: (raise its temperature, eventually change a state)
Exothermic Any change in matter in which energy is absorbed from the surroundings is an endothermic process. Endothermic Any change in matter in which energy is released is an exothermic process. Energy is released Energy is absorbed
Energy can be absorbed by the surroundings or released to the surroundings, but it cannot be created or destroyed. The law of conservation of energy states that during any physical or chemical change, the total quantity of energy remains constant. Energy can be transfer one form to another form.
A system consists of all the components that are being studied at any given time. The surroundings include everything outside the system. system surrounding
chemical mechanical light heat electrical sound
Heat is the energy transferred between objects that are at different temperatures. Heat energy is always transferred from a warmer object to a cooler object.
Temperature indicates how hot or cold something is. Temperature as a measurement of the average kinetic energy of the random motion of particles in a substance. The transfer of energy as heat can be measured by calculating changes in temperature.
Temperature can be measured in a variety of units. Celsius, Kelvin, Fahrenheit The zero point on the Celsius scale is designated as the freezing point of water. The zero point on the Kelvin scale is designated as absolute zero, the temperature at which the minimum average kinetic energies of all particles occur.
Use the following equations in such conversions: T (Kelvin) = t (Celsius) t = T – Assignments Page 45 #1-13 Worksheet Temperature
The transfer of energy as heat does not always result in a change of temperature. The temperature of the mixture remains at 0°C until all of the ice has melted. Once all the ice has melted, the temperature of the water will start to increase until it reaches 100°C. As the water boils, the temperature remains at 100°C until all the water has turned into a gas.
If you transfer the same quantity of heat to similar masses of different substances, they do not show the same increase in temperature. This relationship between energy transferred as heat to a substance and the substances temperature change is called the specific heat. The specific heat of a substance is the quantity of energy as heat that must be transferred to raise the temperature of 1 g of a substance 1 K.
Calorie (cal) Energy (heat) required to raise temperature of one gram of water by one Celsius degree. Joule (J) The SI unit for energy is the joule (J). 1 cal = J Specific heat is expressed in joules per gram kelvin (J/gK).
5.Use the concept of specific heat to analyze the following observation: two pieces of metal with exactly the same mass are placed on a surface in bright sunlight. The temperature of the first block increases by 3°C while the temperature of the second increases by 8°C. Answer: Because the temperatures of the objects differ under the same conditions, they must have different specific heats, so they are made of different metals. Standardized Test Preparation Understanding Concepts Chapter 2