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States of matter

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Unit 2 of Physics and Chemistry for 3rd year of ESO

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States of matter

1. 1. THE STATES OF MATTER
2. 2. Remembering magnitudes and units In this unit well use these units, you must learn them by heart MAGNITUDE UNIT SI Remember Kg MASS 1 Kg = 1000 g (kilograme) 1 m3 = 1000 L VOLUME m3 1 L = 1000 mL (cubic meter) 1 L = d m3 1 cm3= 1 mL Pascal 1 atm = 101300 Pa PRESSURE (Pa = N/m2) 1 atm = 760 mm Hg KTEMPERATURE T( K ) = T (º C) + 273 (Kelvin)
3. 3. Properties of matter● Matter has two kinds of properties: – General properties: they are common to all kinds of matter: ● mass, volume, temperature,... – Specific properties: they are different for every kind of matter: ● Melting temperature, boiling temperature, density, electric conductivity,...
4. 4. Macroscopic behaviour Macroscopic properties of solids, liquids and gasses. SOLID LIQUID GASIt has its own shape It adapts to the shape of its container It is not easily compressible It is easily compressible. It doesnt flow It flows It flows It tends to fill all aviable spaceIt has its own volume It has its own volume Any two gasses are mixed easily
5. 5. Kinetic Theory● The kinetic theory explains the behaviour of solids, liquids and gasses.● Its based on three ideas: – Matter is made of particles – The particles are in continuous motion: ● Temperature is a measurement of the average kinetic energy of the particles. ● If the system is hotter, its particles move faster – All particles attract each other with a force.
6. 6. Kinetic Theory MICROSCOPIC BEHAVIOR OF THE DIFFERENT STATES SOLID LIQUID GAS The only possible Every particle can Every particle has a Particles motion movement is slide over its uniform rectilinear vibration neighbours motion Every particle is in Every particle is in The distance is muchDistance between contact with its contact with its bigger than particles particules neighbours neighbours size There are almost no Atractive force Very strong forces Weak forces forces betweenbetween particules particles
7. 7. Kinetic Theory
8. 8. Kinetic Theory and solids● These questions about solids can be answered using the kinetic theory: – Why do solids keep their own shape? – Why do solids increase their volume when they are heated? – Why do solids became liquids when their temperature increase enough? – Why cant solids be compressed?
9. 9. Kinetic Theory and liquids● These questions about liquids can be answered using the kinetic theory. – Why can they flow? – Why cant they be compressed? – Why do liquids increase their volume when they are heated?
10. 10. Kinetic Theory and gasses● The temperature is related to the average kinetic energy of the particles of a system. – If the temperature raises, the particles move faster.● Gasses exert pressure on the container walls: – Pressure is a consequence of the collision of particles with the container walls.
11. 11. Kinetic Theory and gasses● A few questions that we can answer with the kinetic theory (I): – Any two gasses can be mixed together. Why? – Why can gasses be compressed easily? – Why can gasses flow? – ...
12. 12. Kinetic Theory and gasses● A few questions that we can answer with the kinetic theory (II): – ... – Does pressure change when a gasses is heated? How? Why? – Does pressure change when we reduce the volume of the container of a gas? How? Why? – Why do gasses tend to fill all available space?
13. 13. Gasses Laws● Charles Law: describes how gasses expand when heated.● At a constant pressure, the volume of a gas increases or decreases proportionally to its absolute temperature. – Dont forget: T(K) = t(ºC) + 273 V = constante T V1 V2 = T1 T2
14. 14. Gasses Laws● Charles Law ● Use the Internet for more information: ● Practise doing numeric exercises about this law: http://www.educaplus.org/gases/e ● A simple experiment about Charles Law http://youtu.be/ATje2S5YZNo ● An interactive on-line software about Charles Law http://www.educaplus.org/gases/fl
15. 15. Gasses Laws● Gay-Lussacs Law: describes the relationship between pressure and temperature in gasses contained in rigid containers (V = constant)● At a constant volume, the pressure of a gas increases or decreases proportionally to its absolute temperature. Dont forget: T(K) = t(ºC) + 273 p = constant T p1 p2 = T1 T2
16. 16. Gasses Laws● Gay-Lussacs Law ● Use the internet for more information: ● Practise doing numeric exercises about this law: http://www.educaplus.org/gases/e ● A simple experiment about Gay-Lussacs law: http://youtu.be/VNU6YpKmLtM
17. 17. Gasses Laws● Boyle-Mariotes Law: describes how gasses are compressed.● At a constant temperature, the pressure and the volume of a gas are inversely proportional. p · V = constant p1 · V 1 = p 2 · V 2