##### Physical Characteristics of Gases 2
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#### Complete list of Terms and Definitions for Physical Characteristics of Gases 2

Terms Definitions
Fluids Liquids and gases
Boyle's Law P₁V₁ = P₂V₂
mm Hg now called a torr
Gas Laws Simple mathematical relationships between the volume, temperature, pressure, and amount of a gas
diffusion such spontaneous mixing of the particles of two substances caused by their random motion.
none the forces of attraction between the particles except near the temperature at which the gas condenses
volume amount of space that an object occupies
Precipitate A solid produced in a chemical reaction
Decomposition Reactions Formula AX ---> A + X
absolute zero The temperature -273.15 C; given a value of zero in the Kelvin scale
newton N, force that will increase the speed of a 1 kg mass by 1 meter per second each second it is applied
Activity Series A list of elements organized according to the ease with which the elements undergo certain chemical reactions
Partial Pressure Pressure of each gas in a mixture
Ideal gas an imaginary gas whose particles are infinitely small and do not interact with each other
Standard Temperature and Pressure 1 atm pressure and 0 Celsius
torr equivalent to 1 mm Hg, named in honor of Torricelli for his invention of the barometer
number of moles and pressure the constants in Charles's law
Word Equation An equation in which the reactants and products in a chemical reaction are represented by words
What are elastic collisions Collisions between gas particles and between particles and container walls
Kinetic-molecular theory based on the idea that particles of matter are always in motion
units of pressure 1. millimeters of mercury = mm Hg 2. torr 3. atmosphere of pressure = atm 4. pascal = Pa
2KI + Pb(NO₃)2 ---> PbI₂ + 2NO₃ Double Replacement Reactions Example
elastic collisions one in which there is no net loss of KE
How many atm are there to torr 1 atm = 760 torr
Dalton's Law of Partial Pressure States that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
What happens when gases are together They spread out and mix with one another because of the random and continuous motion of the molecules
Why is it that gas is 1/1000 dense than its liquid/solid state The particles are so much father apart