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