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DCE Chem Unit 7

DCE Chemistry Unit 7 Vocabulary

TermDefinition
fluid a material in which the particles have enough energy to slide past one another (flow). Gases and liquids are fluids.
pressure force per unit area caused by collisions between gas particles and the container (can be measured in atm, mmHg, kPa, etc.)
compressibility a measure of how much the volume of matter decreases when pressure is applied
STP standard temperature and pressure: zero degrees Celsius (273 K) and 101.3 kPa (1 atm or 760 mm Hg)
Kinetic Molecular Theory a theory explaining the states of matter based on the concept that matter consists of tiny particles that are in constant motion
Avagadro's Law equal volumes of gases at the same temperature and pressure contain equal numbers of gas particles (at STP all gases have a volume of 22.4 L)
Dalton's Law of Partial Pressures the total pressure of a mixture of gases is equal to the sum of all the partial pressures for each gas
partial pressure in a mixture of gases, the contribution that each gas makes towards the overall pressure
Ideal Gas Law PV = nRT
Kelvin A temperature scale used for measuring temperature of gases (Kelvin = Celsius plus 273)
R ideal gas constant (8.31 or 0.0821 or 62.4 depending upon units used)
diffusion the tendency for molecules to move from areas of higher concentration to areas of lower concentration until the concentration is uniform throughout
Boyle's Law P1V1 = P2V2
Charles's Law V1T2 = V2T1
Guy-Lussac's Law P1T2 = P2T1
Combined Gas Law P1V1T2 = P2V2T1
effusion the process by which gas escapes through a tiny hole
Avagadro's Principle V1n2 = V2n1
Archimedes Principle actual mass = apparent mass + mass of displaced fluid
Created by: dcechem
 

 



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