Presentation on theme: "Energy Processes in Earth Science Earth Science Mr. Clark Bethpage High School."— Presentation transcript:
Energy Processes in Earth Science Earth Science Mr. Clark Bethpage High School
Energy Transfer of Energy Conduction Convection Radiation Electromagnetic Energy’s Interactions with Matter
Energy Terrestrial Radiation The Greenhouse Effect First Law of Thermodynamics Second Law of Thermodynamics Kinetic energy Potential energy Heat and Temperature
Energy Energy is the ability to do work. Energy is measured in units called Joules. Energy is also measured in calories.
Transfer of Energy Energy can be transferred in three ways: Conduction Conduction Convection Convection Radiation Radiation
Transfer of Energy Conduction is the transfer of heat energy through molecular collisions. Convection is the transfer of heat energy through currents formed due to density differences. Radiation is the transfer of electromagnetic energy through space. Radiation requires no medium. (matter)
Conduction Conduction can occur with solids, liquids, or gases. Contact must be made to conduct heat.
Convection Convection is due to density differences, it creates currents. Convection is the driving force behind global winds, ocean currents, and plate tectonics. A convection box can be used to show convection.
Radiation Electromagnetic radiation radiates through space. Electromagnetic radiation travels at the speed of light. Light is part of the visible spectrum of the electromagnetic spectrum.
Insolation Insolation (incoming solar radiation) can be absorbed by the Earth. Absorption by Earth materials –Color and texture affect absorption. –Dark colors and rough surfaces absorb the best.
Terrestrial Radiation Terrestrial radiation is the radiation given off by the Earth when it heats up after absorbing insolation. When energy is absorbed it is always reradiated at a longer wavelength because longer wavelengths contain less energy.
Radiation rule Rule: A good absorber is a good radiator.
Terrestrial Radiation Specific Heat: The lower the specific heat the better the absorption. Granite and Basalt have low specific heats and therefore heat up quickly and cool down quickly. Water has the highest specific heat of Earth materials so it is the poorest absorber and therefore heats up and cools down the slowest.
The Greenhouse Effect Certain materials (glass) allow the shorter wavelength (visible light) to pass through them (transparent) but do not allow longer wavelengths (infrared) to pass through (opaque) and therefore trap longer wavelength (infrared) radiation and cause the temperatures inside the glass to rise.
The Greenhouse Effect Certain gases in the Earth’s atmosphere are greenhouse gases, among them are carbon dioxide, methane, and water vapor. If concentrations of these gases get too high, global warming could ensue. Global Warming would have drastic effects upon the Earth's climate. The planet Venus has these conditions.
First Law of Thermodynamics Conservation of Energy Energy is neither created nor destroyed but is always conserved and transformed from one kind to another. Energy only changes form. You cannot get something from nothing. Energy in = energy out
Second Law of Thermodynamics Energy always goes from a more usable form (high quality) to a less usable form (low quality). Heat always travels from hot to cold. All systems proceed to maximum entropy (randomness).
Kinetic Energy Kinetic energy is the energy of motion. KE = ½ mv 2 where m is mass and v is velocity.
Potential Energy Potential energy is stored energy. PE = m x g x h where m is mass, g is the acceleration due to gravity, and h is height.
Heat and Temperature They are not the same. Temperature is average kinetic energy of the molecules in a sample of matter. Heat is the total internal energy of a sample of matter.
Temperature There are three temperature scales: Fahrenheit Celsius Kelvin To convert use the Earth Science Reference Tables or use a formula.
Sample Heat Problem How many calories are absorbed when 50.0 g of water are heated from 30 o C to 60 o C? Solution: Q = m c p DT Q = (50.0 g) (4.18 J/g o C)(30 o C) Q = 6270 J or 6.270 kcal
Changes of Phase Solid to liquid = melting Liquid to solid = solidification Liquid to gas = vaporization (evaporation) Gas to liquid = condensation Solid to gas = sublimation There is no change in temperature during a phase change. Only latent heat may be added or released.
Latent Heat of Fusion The heat needed to convert a mass from solid to liquid is the latent heat of fusion. Heat of fusion for water is 334 J/g. (ESRT)
Latent Heat of Fusion Problem Sample problem: How many calories are required to melt a 255g ice cube at 0 o C? Q = mass X heat of fusion Q = (255g) (334 J/g) = 85170 J
Latent Heat of Vaporization The heat needed to convert a mass from a liquid to a gas is the latent heat of vaporization. Heat of vaporization for water is 2260 J/g. (ESRT)
Latent Heat of vaporization Problem Sample problem How many calories are required to vaporize a 423g of water at 100 o C and 1 atmosphere of pressure? Q = mass X heat of vaporization Q = (423g) (2260 J/g) = 955980 J
The heating of a solid results in a liquid. The heating of a liquid results in a gas. The flat part of the curve represents a phase change. Phase changes during are not accompanied by temperature changes. Reading the curve in reverse is a cooling curve.