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States of MatterKinetic-Molecular Theory – describes the behavior of gases
Three assumptions:
1)All gases consist of small particles
2)Constant random motion experiencing elastic collisions
3)Kinetic energy depends on mass and velocity. At a given temperature, all gases have the same kinetic energy.
K.E. = ½ mv2
m mass in kg
v velocity m/s
K. E. Proportional to temperature
Consider Nitrogen and oxygen at room temp.
Which one has higher K.E.?
Which one has faster moving molecules?
Behavior of gases
• Low density
• Compression and expansion
• Diffusion-movement of one material through another
• Effusion-gas escaping through a small hole
• Graham’s law
Gas Pressure
• Pressure – force per unit area
• Barometer – measures atm pressure
• At sea level at 0 degrees C, average air pressure is 760. mm Hg. This is the same as 1.00 atm or 760. torr or 101.3 kPa
• Be able to do conversions
• Manometer – measures gas pressure in a closed container (see page 389)
• Open manometers
Forces of AttractionIntermolecular forces
• Dispersion forces - weak forces due to a temporary induced dipole
• Exist between all particles but only significant if they are the only forces present
• Explains why Cl2 and F2 are gases but Br2 is a liquid and I2 is a solid
• Dipole-dipole• Hydrogen bonds
Liquids
• Density and compression
• Fluidity
• Viscosity – resistance to flow, decreases with temperature
• Surface tension
• Surfactants
• Capillary action
Solids
• Density
• Crystalline
• Simple cubic cell
• Body-centered cubic cell
• Face-centered cubic cell
• Molecular solids
• Covalent network solids (macromolecular)
• Ionic solids
• Metallic solids
• Amorphous solids
Phase changes
• Melting • Vaporization• Vapor pressure • Boiling – know this definition• Sublimation• Condensation• Deposition• freezing
q = mass X change in temp X specific heat
q = mass X enthalpy
For water: specific heat of steam is 2.02 J/g C
specific heat of liquid is 4.18 J/g C
specific heat of ice is 2.06 J/g C
Enthalpy of fusion is 334 J/g
Enthalpy of vaporization is 2260 J/g
Energy and change in state
• How much energy is needed to convert 10.0 g of ice at -15.0 degrees C to steam at 130.0 degrees C?
Energy and change in state
• How much energy is needed to melt 25.4 grams of iodine? The enthalpy of fusion of iodine is 61.7 J/g.
• Find the heat needed to raise the temperature of 5.58 kg of iron from 22.0 degrees C to 1000.0 degrees C.
• Find the energy change when 28.9 g of copper is cooled from it’s melting point to 25.0 degrees C. Is this energy gained or released and how can you tell?
example
• A 2.35 g sample of unknown metal at 100.0 degrees C is placed in 50.0 ml of water originally at 23.0 degrees C. The maximum temperature of the water is 23.3 degrees C. What is the specific heat of the unknown metal?