chapter 7; Changes of State and the gas Laws

Question 1

kinetic molecular view

Answer 1

describes behavior of gases at the molecular level

Question 2

gaseous atoms and molecules are in constant motion, moving at […] speeds

Answer 2

high

Question 3

greater speeds =

Answer 3

greater kinetic energy

Question 4

gaseous atoms or molecules move in […] lines in […] directions, […] with walls of their container, and fill entire container

Answer 4

straight
random
collide

Question 5

greater speeds = greater kinetic energy =

Answer 5

higher temperatures

Question 6

gaseous atoms or molecules are […] apart from one another and have […] intermolecular forces of attraction

Answer 6

far
negligible

Question 7

gases are […] giving them unique properties that are different from […] and […]

Answer 7

compressible
gases
liquids

Question 8

gas particles collide with the walls of the container, creating […]

Answer 8

pressure

Question 9

Pressure (P) =

Answer 9

force / area

Question 10

1 atmosphere (atm) =

Answer 10

760 millimeters of mercury (mmHg) used in medicine
760 torr
14.70 pounds per square inch (psi) English unit for pressure
101,325 pascals (Pa)

Question 11

at sea level, atmospheric pressure is how many atm

Answer 11

1 atm

Question 12

higher altitudes =

Answer 12

Lower atmospheric pressure
- fewer molecules pressing down
- less oxygen per breath

Question 13

why do people who climb mount Everest usually carry cylinders of oxygen with them

Answer 13

the decreased atmospheric pressure at high altitude means that less oxygen is inhaled with every breath. Cylinders of oxygen provide supplemental oxygen and at a higher pressure

Question 14

what are the four variables that describe the macroscopic properties of a gas

Answer 14

pressure (P)
volume (V)
temperature (T) and
moles (n)

Question 15

what is the pressure volume relationship (Boyle’s law)

Answer 15

pressure and volume are inversely proportional when n and T are constant

Question 16

what is the volume temperature relationship (Charles’s law)

Answer 16

volume and temperature are directly proportional when n and P are constant

Question 17

what is the pressure temperature relationship (Gay Lussac’s law)

Answer 17

pressure and temperature are directly proportional when n and V are constant, and T is given in kelvins

Question 18

in a graph how is the Boyle’s law shown

Answer 18

(constant temperature)
- as volume increases pressure decreases
pressure vs 1/V
if inversely it is straight line with pressure increasing as 1/V

Question 19

in a graph how is Charles’s law shown

Answer 19

(constant pressure)
- increase temperature so does the volume
proportional

Question 20

in a graph how is Gay-Lussac’s law

Answer 20

(constant volume)
- as temperature increases there is increase in pressure

Question 21

what is the equation of Boyle’s law

Answer 21

PiVi = PfVf

Question 22

what is the equation of Charles’s Law

Answer 22

Vi/Ti = Vf/Tf
volume and temperature are directly proportional
tmp is given in kelvins

Question 23

convert celcius to kelvin

Answer 23

kelvin = celcius + 273

Question 24

what is the equation of gay-lussac’s law

Answer 24

Pi/Ti = Pf/Tf
pressure and temperature are directly proportional
T is in kelvins

Question 25

what is the combined gas law: pressure, volume, and temperature

Answer 25

PiVi/Ti = PfVf/Tf

Question 26

when is the combined gas law used

Answer 26

when there is a fixed amount of gas, n, and the variables P, V, and T are changing

Question 27

what is the volume mole relationship (Avogadro's law)

Answer 27

moles of gas, n, is directly proportional to volume, V, of the gas (constant T and P)

Question 28

what is the equation of the volume-mole relationship (avogrado's law) equation

Answer 28

Vi/ni= Vf/nf constant pressure and temperature

Question 29

what is standard temperature and pressure (STP)

Answer 29

0 degrees Celsius (273.15 K) and 1 atm of pressure

Question 30

what is molar volume of a gas at STP

Answer 30

22.4 L

Question 31

one mole of any gas at [...] degrees celsius and [...] atm occupies a volume of [...] L, known as the molar volume of a gas

Answer 31

0 1 22.4

Question 32

what is 1 mole = in L at STP

Answer 32

22.4L 1 mole = 22.4 L

Question 33

what is the density of a gas at STP equation

Answer 33

density = molar mass / molar volume (22.4 L/mol)

Question 34

example of density of helium

Answer 34

density (helium) = (4.00 g/mol) / (22.4 L/mol) = 0.179 g/L *less dense then air*

Question 35

what is the molar mass of air

Answer 35

28.8 g/mol if divided by STP 28.8 g/mol / 22.4 L/mol = 1.29 g/L

Question 36

when something is less dense than air does it float or sink

Answer 36

sink

Question 37

how many gases do gas mixtures contain

Answer 37

two or more

Question 38

what is daltons law of partial pressures

Answer 38

- each gas in a mixture exerts a pressure independent of other gases, behaving as if it alone occupied the total volume - Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressure of each gas in the mixture

Question 39

what Daltons Law of partial pressure equation

Answer 39

Ptotal = P1 +P2 + P3 + ... Pn P1, P2, P3 ..., Pn are partial pressures of the gases in the mixture

Question 40

what is the percentage oxygen in the atmosphere

Answer 40

20.95%

Question 41

e.g. at sea level (760 mmHg), the partial pressure of oxygen is) + on Mount Everest (400 mmHg) the partial pressure of oxygen

Answer 41

0.2096 x 760 mmHg = 159 mmHg 0.2096 is 20.95% of oxygen in the atmosphere divided by 100 + 0.2095 x 400 mmHg) the partial pressure of oxygen is 84 mmHg

Question 42

what does Henry's law state

Answer 42

that the number of moles of gas, n, dissolved in a liquid is directly proportional to the partial pressure, P, of the gas

Question 43

what dissolved gases does blood serum contain

Answer 43

oxygen nitrogen, and carbon dioxide

Question 44

what is Henry laws equation

Answer 44

P = K subscript H C P=KHC (t is constant)

Question 45

what do the letters stand for in Henrys Law equation P = K subscript H C

Answer 45

P = the partial pressure of the gas K subscript H = Henry's constant which is unique for each gas C = the concentration of the dissolved gas (mol/L)

Question 46

how to solve for concentration of the dissolved gas from Henry's law P = K subscript H C

Answer 46

P/K subscript H = C

Question 47

Henry's law shows that the moles of gas dissolved in solution are [...] to the partial [...] of the gas

Answer 47

proportional pressure

Question 48

Is volume and temperature proportional

Answer 48

Yes, as temperature increases volume.