Solids

 high degree of internal order, atoms or molecules are limited to back and forth motion about a central position, maintain their shape bc their atoms are kept in place by strong mutual attractive forces

1. have weaker mutual attraction forces than in solids and liquid molecules can move about freely, liquids are dense and cannot be easily compressed (just like solids arent that way)

1. Gases- molecular attractive forces are very weak, gas molecules exhibit rapid, random motion w/ frequent collisions,  have no inherent boundaries and are easily compressed and expanded,

All matter has energy and its called internal energy

two types (potential and kinetic)

  temp at which there is no kinetic energy

No one can actually achieve this, purely conceptual

In Celsius units, kinetic molecular energy stops at

-273 degrees Celsius

So 0 ° K = -273° C and 0°= 273°K

To convert degrees celsius to degrees kelvin,

°K= °C + 273

-460°F

To convert degrees fahrenheit to degrees celsius use

°C = (5/9) (°F-32)

To convert degrees celsius to degress fahrenheit, simple reverse formula

1. Weak forces of attraction, most internal energy is kinetic energy
2. Gas molecules travel about randomly at high speeds and w/ frequent collisions
3. Velocity of gas molecules is directly proportional to its temperature

Avogadro's law

-states that the 1 g atomic weight of any substance contains exactly the same no of atoms, molecules or ions.

- states that equal volumes of gases under the same conditions must contain the same no of molecules. Therefore, 1 mole of gas, at a constant temp and pressure, should occupy same volume as 1 mole of any other gas.

 Ideal volume is called molar volume

This no, 6.023 x 10^23 is Avogardro's constant. In SI units, quantity of matter equals 1 mole.

At standard temp and pressure, dry (STPD), the ideal molar volume of any gas is