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Understanding Density: Concepts, Demonstrations, and Applications

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ranee
30 diapositives · 543 Views · Jul 13, 2014

This guide explores the concept of density—defined as mass per unit volume—and its significance across various substances, including solids, liquids, and gases. Key principles related to density, such as how temperature and pressure affect it, are illustrated through demonstrations, including the comparison of densities in different materials and real-life applications. From buoyancy in fish to the density of water at various temperatures, readers will gain a comprehensive understanding of density and how to determine it in both regular and irregular shapes.

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  1. DENSITY Introduction

  2. What is density? Density is a comparison of how much matter there is in a certain amount of space.

  3. Which one is more dense? Demonstration: People in a square How about this: Which square is more dense?

  4. Which one is more dense? Now which one is more dense?

  5. What is density? Density = mass OR mass ÷ volume. volume Units for density: g . cm3 Why are these the units for density? ALWAYS REMEMBER UNITS!

  6. DENSITY • Depends on: • Mass • Volume D = m/v (g/cm3) Mass usually expressed in grams Volume usually expressed in cm3 or liters, etc.

  7. What would take up more space??? A kilogram of feathers…..or a kilogram of steel?? OR

  8. The proximity of like atoms or molecules More than just the “heaviness” of a substance, density includes how much space an object takes up!! All substances have density including liquids, solids, and gases Density is the measure of the “compactness” of a material

  9. “Compactness”

  10. Gases • How much kinetic energy do the molecules have?? • The greater the kinetic energy • ……the greater the volume • …… and the less dense that gas is!! • Therefore, cold air is more dense than warm air

  11. Gases • Real life application….. • Low pressure weather system means warmer air tends to rise, • High pressure systems indicate a colder more dense air mass that will……. • SINK!!!

  12. Balloon and liquid nitrogen • http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/balloon.html#c1 • http://paer.rutgers.edu/pt3/movies/TVrhoandFb.mov www.dkimages.com

  13. LIQUIDS • The more dissolved solids in a solution, the more dense (such as ocean water) • Cold water in lakes tend to sink (this creates a constant mixing of water, nutrients, and other substances) • Kinetic energy again!! Denser layers to less dense layers…..

  14. What would happen???? • Mercury density = 13600kg/m3 • Lead density = 11340kg/m3

  15. Lead floats on liquid mercury!

  16. Solids Ice vs. water…..

  17. SOLIDS • Ice is less dense than water (which is why lakes and ponds have a thin layer of ice covering in winter, with water underneath) • Various rocks, woods, metals have a characteristic density specific to that substance Wouldn’t you like to have a bunch of THIS dense material?

  18. Archimedes and the Kings Crown

  19. Factors affecting Density • Temperature • Pressure

  20. Factors affecting Density • Dissolved solids – in liquids • Concentration and kind of substances

  21. FACTORS AFFECTING DENSITY • ATomS!!!!

  22. Relative Density • The density of a material or substance, relative to another substance • Expressed in a ratio: water = 1g/cc • Water is the substance to which we generally compare other substances • ALSO known as SPECIFIC GRAVITY

  23. How are Submarines like fish…. • The swim bladder in bony fish control their relative density in order to rise or dive in the water….buoyancy • When air is added to the swim bladder, by diffusion through the blood vessels in the bladder walls, the fish becomes less dense overall • when air is removed fish become more dense • By changing the volume of air in the bladder, the fish’s density can be made equal to that of the surrounding water at a given depth.

  24. Absolute DENSITY • The density of a material in its closest “packed form” • For water: Absolute Density = 1000kg/m3 at 40C and 1 atm(pressure) in other words, the greatest density of water is at 40C

  25. DETERMINING DENSITY • Regular Shapes – mass, then determine the volume by formula EX: cubes, cylinders, spheres, cones, etc. • Irregular shapes – mass, then measure displacement of a liquid (usually water) by that irregularly shaped object

  26. Liquid Layers Check out this picture from your book. Which layer has the highest density? Which layer has the lowest density? Imagine that the liquids have the following densities: 10g/cm3. 3g/cm3. 6g/cm3. 5g/cm3. Which number would go with which layer?

  27. Liquid Layers – Try with your neighbor Which liquid has the highest density? Which liquid has the lowest density? Which liquid has the middle density?

  28. Liquid Layers – Try on your own! Imagine that the liquids on the right have the following densities: 15g/cm3 10g/cm3 3g/cm3 9g/cm3 7g/cm3 12g/cm3 Match the colors to the correct densities. 3g/cm3 7g/cm3 9g/cm3 10g/cm3 12g/cm3 15g/cm3

  29. Review What is the formula for density? What happens if you pour together liquids that have different densities? Will the liquid on the top have the highest or lowest density? Will the liquid on the bottom have the highest or lowest density?

  30. Super Scientist Question of the Day Jake has a book, a ruler, and a balance. How can Jake find the density of the book with the tools he has?