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Hint

1

Boyle’s Law

P1V1 = P2V2

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2

Charles’s Law

V1/T1 = V2/T2

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3

Gay-Lussac’s Law

P1/T1 = P2/T2

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4

Combined Gas Law

P1V1/T1 = P2V2/T2

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5

Dalton’s Law of Partial Pressures

Ptotal = P1 + P2 + P3 + P4 + …

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6

STP atm

1.00

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7

STP kPa

101.325

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8

STP mmHg/torr

760

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9

STP temp (K)

273

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10

Ideal Gas Law

PV = nRT

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11

Ideal Gas Law + mass and molar mass

PVM = mRT

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12

density of a gas

m/V

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13

Avogadro’s Principle

22.4 L/ mol

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14

expands

____________ to assume the shape and volume of its container

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15

flows

readily ____________

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16

straight lines

particles only move in ____________

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17

compressible

molecules far apart but ____________

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18

few

____________ attractive forces between particles

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19

volume

space occupied by a gas sample

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20

mL, L, cm^3, dm^3

volume units

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21

1 cm^3

1 mL = ____________

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22

1dm^3

1 L = ____________

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23

temperature

a measure of the average kinetic energy of a group of particles

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24

thermometer

measurement tool for temperature

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25

kelvin (K)

temperature unit

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26

amount

number of moles of the substance

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27

mol

amount unit

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28

pressure

force per unit area caused by the collision of the gas molecules with the walls of the container

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29

manometer

measurement tool for pressure

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30

pascal (Pa), atmosphere (atm), torr, millimeter of mercury (mmHg)

pressure units

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31

kinetic molecular theory

a model that uses particle motion and interparticle forces to properties of different states of matter

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32

no volume

individual gas particles have almost ____________

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33

inter particle

gas particles have no ____________ forces

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34

constant random

gas particles are in ____________ motion

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35

elastic

collisions are ____________, no energy lost

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36

average kinetic energy

all gases have the same ____________ at a given temperature

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37

high temp and low pressure

real gases behave like ideal gases at:

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38

avogadro’s principle

equal volume of all gases measured at the same temperature and pressure contain the same number of particles

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