sci

• gases expand when heated
• they compressed when cooled
• they They expand and uniformly fills any container, with no fixed volume
• They can be compressed easily.
• They mixed completely with other gases.
• They exert pressure.
• expansion- gases do NOT have a definite shape or volume.
• Fluidity- gas particles glide past one another, called fluid just like a liquid.
• Compressibility – can be compressed because gases take up mostly empty space.
• Diffusion - gases spread out and mix without stirring and without a current. Gases mix completely unless they react with each other.
• Volume - refers to the space matter (gas) occupies.
• Pressure (P)- the number of times particles collide with each other and the walls of the container
• Pressure is measured with a device called a barometer.
• Temperature (T) – as temperature increases gas particles move faster, as temperature decreases gas particles move slower.
• measured with a thermometer in Celsius.
• Number of Moles - tells you how much of a certain gas you have 1 mole = number of grams of the compound or element (molar mass) 6.02 x 1023 molecules per mole of the gas.
• STP - "standard temperature and pressure".
• BOYLE'S LAW states that if the pressure of a gas is increased, the volume of the gas is decreased.
• CHARLES' LAW- states that the volume of a fixed amount of gas is directly proportional to the temperature at constant pressure.
• GAY LUSSAC'S LAW - states that the pressure of the gas is directly proportional to its temperature.
• COMBINED GAS LAW- states that “for a given mass of gas, the volume is inversely proportional to the pressure and directly proportional to its absolute temperature.
• AVOGADRO'S LAW - states that the volume of gas is directly proportional to the number of moles of gas.
• IDEAL GAS LAW - interrelates, volume, temperature, pressure and number of moles of gas
• The word KINETIC refers to motion
• Kinetic energy= energy an object has because of its motion
• The average kinetic energy of gas particles depends on the temperature of the gas.
• Collisions between particles of a gas and the container wall are elastic.
• Total Kinetic energy remains constant.
• Gases consist of a large number of tiny particles (molecules or atoms) ; these particles are very far apart, therefore gas is mostly empty space.
• Particles of a gas are in constant, straight-line motion, until they collide.
• Particles of matter (any type) are in constant motion!