Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Scott > Ch. 6 Gases & Solutions > Flashcards

Ch. 6 Gases & Solutions Flashcards

1
Q

Patm = _______

A

Atmospheric Pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

psi = ________

A

Pounds per Square Inch

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Insoluble or Soluble? / Can it Hydrogen bond?

  1. Hydrophilic =
  2. Hydrophobic =
A
  1. soluble / Yes
  2. insoluble / No
    * fyi: (**no hydrogen bonding = will dissolve)*
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Define: Gas Pressure

A

The force of collisions that take place between particles of gas and an object.

(the walls of the container that hold the gas)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What unit of measurement is used when measuring atmospheric pressure?

A

Lenght (mm Hg)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Diatomic = ______ atom(s)

A

Two

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Monoatomic = ______ atom(s)

A

One

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Water Vapor = ___________.

Vapor = ______________.

Vapor Pressure = ___________.

A

Gas

Gas from evaporation of liquid

Movement of particles from liquid to gas phase.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

The boiling point of a liquid is the temperature at which the ___________ pressure of the liquid equals the __________ pressure.

A

Vapor pressure

Atmospheric pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Liquids boil when their ________ equals the pressure of the air above them.

A

Vapor Pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Standard Temperature = _______

Standard Pressure = _________

A

Standard Temp = 0°C

Standard Pressure = 1 atm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Which elements are gases at standard temperature and pressure (0°C & 1 atm)

A

H, N, O, F, Cl, & Noble gases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Define: Sublimation

A

Solid to a gas without a liquid

fyi: (dry ice in balloon)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

At 100°C vapor pressure is 760.00 torr.

Convert 760.00 torr to mm Hg?

A
  1. 00 torr = 760 mm Hg
    * fyi: (1 atm = 760 mm Hg / 1 atm = 760.00 torr)*
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

As temp rises molecules move ________.

A

Faster

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How does an autoclave work?

A

Produces pressures greater than 1 atm, so water boils at temps above 100°C. At those temps most infections are destroyed.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Gas Laws:

All gases behave in a ______ manor.

A

Similar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Gas Laws:

What variables are used when dealing with gas laws?

<em>Hint: 4 of them</em>

A

Pressure

Temperature

Volume

amount of moles (n)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Gas Laws:

__________ says that, for a sample of gas with a constant volume, pressure and temperature are directly related.

A

Gay-Lussac’s Law

-OR-

Pressure-Temperature Law

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Gas Laws:

What does the dotted line represent?

A

Absolute zero

(- - -no data points- - -)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Gas Laws:

Pressure-Temperature/Gay-Lussac’s Law states that, for a sample of gas with a constant volume, pressure and temperature are ________ related.

As pressure increases, temperature __________.

As pressure decreases, temperature __________.

A

Directly related

Temperature Increases

Temperature Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Gas Laws:

In calculations, temperature should always be converted from °C to _____.

A

Kelvin

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Gas Laws:

Oxygen tanks get ____ when in use. The pressure inside the tank _______ as O2 exits the tank.

A

Cold

Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Gas Laws:

Volume & Temperature Law/Charles’ Law says that, for a sample of gas at a fixed pressure, volume and temperature are ________ related.

As temperature increases, volume _______.

As temperature decreases, volume _______.

A

Directly related

Increases

Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Gas Laws:

Pressure-Volume Law/Boyle’s Law says that, for a sample of gas at a fixed temperature, pressure and volume are ______ related.

As volume increases, pressure ______.

As volume decreases, pressure ______.

A

Inversely related

Decreases

Increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Gas Laws:

Respiration: inhaling and exhaling is an application of ______ Law.

A

Boyles Law

-OR-

Pressure-Volume Law

(same thing)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Gas Laws:

Which law does this scenario best fit?

Diving 10m in depth: P increases two-fold and lung volume contracts by a factor of two.

A

Boyle’s Law

-OR-

Pressure-Volume Law

(same thing)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Gas Laws:

A formula that combines Boyles, Charles’ and Gay-Lussac’s Law is called ____________ Law

A

The Combination Gas Law

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Dalton’s Law of Partial Pressure states that the total pressure of a mixture of gases is the __________________________________________.

A

Sum of the partial pressure of its components

Ptotal = P1 + P2 + P3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Daltons Law:

The partial pressure of a gas in a mixture is the pressure that the gas would exert if alone.

This applies to air which is a mixture of 78.0% _____, 21.1% _____, and 0.9% other gases like water vapor, Ar, He, H 2, CO2, CH4, etc.

A
  1. 0% N2
    - and-
  2. 1% O2
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Daltons Law:

In which town does dry air contain highest partial pressure of O2?

a. Hot Coffee, Mississippi (altitude 279 ft)
b. Pie Town, New Mexico (altitude 7,778 ft)

A

A. because lower altitude means higher O2 levels.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Daltons Law:

Why do climbers often carry oxygen supplies?

Is PCO2 higher in the lungs or the tissue?

A

Daltons Law:

Because the partial pressure of 02 (P02) is low at high altitudes

Daltons Law: As pressure increases, gas solubility decreases

PC02 (tissue) is greater than P02 (lungs)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

A _________ consists of just one element or compound.

A

Pure Substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What parts of the human body are best represented by the following pieces of the lung demonstration model:

Two rubber balloons = __________

Y-tube = ________

Open end of the Y-tube = ____________

Bell Jar = __________

Thin sheet of rubber = _____________

A

Two rubber balloons = Lungs

Y-tube = Trachea

Open end of the Y-tube = Nose / Mouth

Bell Jar = Thorax Cavity

Thin sheet of rubber = Diaphragm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

A combination of two or more pure substances is called a ________.

A

Mixture

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Which are elements and which are compounds?

  1. Mercury
  2. Silver
  3. Water (H20)
  4. NaCl (salt)
  5. Oxygen
  6. Sucrose (sugar)
A
  1. Element
  2. Element
  3. Compound
  4. Compound
  5. Element
  6. Compound
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Heterogeneous mixtures =

Homogeneous mixtures =

A

Hetero = Not evenly distributed; immiscible, insoluble. i.e: (sand + H20)

Homo = uniformly distributed; miscible, soluble. i.e: (sugar + H20)

38
Q

Solvent =

Solutes =

Solution =

A

Solvents = The component in solution in greatest amount. (H20)

Solutes = The component dissolved in solution.

Solution = Solute + Solvent

39
Q

What does “Like Dissolves Like” mean.

A

Polar solute will dissolve in polar solvent.

Nonpolar solute will dissolve in Nonpolar solvent

40
Q

The formation of solutions requires that solute particles have two important characteristics.

  1. ______________…
  2. ______________…
A
  1. The must be about the same size as the solvent molecules.
    - AND-
  2. They must be able to interact with the solvent molecules through IMF (H-bond, D-D int, L-forces).
41
Q

_________ refers to the amount of solute that will dissolve in a given amount of solvent at a given temperature.

Temperature can affect _________(directly related).

A

Solubility

Solubility

42
Q

Most liquid and solid solutes become more soluble in water as temperature increases, why?

A

Because temperature affects the rate at which molecules are bouncing off one another.

i.e: (high temp = more soluble)

43
Q

Electrolytes =

A

Compounds that dissolve in water to form ions.

44
Q

Electrolytes:

The consequences of having too much or too little of a particular electrolyte can have profound effects on your health.

Give two examples of the consequences of taking too much or too little of a particular electrolyte.

A

Transmission of nerve impulses (spasms)

Muscle contraction and blood clotting (cramping)

45
Q

Solubility of a gas and temperature:

For all gaseous solutes (02, C02, etc.), an ________ in temperature leads to a _________ in solubility.

Why?

A

Increase

Decrease

The solubility of gaseous solute and temperature are inversely related. Temp increase causes molecules to move quicker and become more soluble.

46
Q

Solubility of a gas and pressure:

Henry’s Law states that the solubility of gas in a liquid is proportional to the ________ of the gas over the liquid.

A

Pressure

47
Q

Solubility of gas and temperature:

Henry’s Law

When a bottle of carbonated water is opened, the pressure of C02 over the liquid is ________ to that of the surrounding Patm. C02 has a lower solubility at this reduced pressure and it rapidly leaves the solution as ________.

A

Reduced

Bubbles

48
Q

Solubility of gas and temperature:

Henry’s law predicts that increasing the pressure of gas __________ its solubility by the same proportion.

(doubling the pressure doubles the solubility and so on.)

A

Increases

P.S. Henry is directly related

49
Q

Solubility of gas and temperature:

Give two applications that use Henry’s Law.

  1. __________…
  2. __________…
A
  1. Hyperbaric Chamber: Used to treat C0 poisoning, gangrene, and tetanus.
  2. Bends: On resurfacing, divers experience lower Patm so SN2 in serum decreases, N2 seeps out of damaging arteries.
50
Q

Solubility of gas and temperature:

How does a Hyperbaric chamber work?

A

High levels of 02. Bacteria cannot survive in high levels of 02.

51
Q

Solubility of Organic Compounds:

Pentane + Hexan =

Hydrophobic or Hydrophilic

Why?

A

Hydrophobic

Like dissolves like(polar & polar).

fyi: pentane & hexane cannot bond together.

52
Q

Solubility of Organic Compounds:

Alcohol + H20 =

Hydrophilic or Hydrophobic

Why?

A

Hydrophilic

Like dissolves like(polar & polar),

fyi: alcohol & water can bond.

53
Q

Which compound is more soluble in water?

Why?

Ethanol: CH3CH2OH

-OR-

1-Octanol: CH3CH2CH2CH2CH2CH2CH2CH2OH

A

Ethanol,

because it has a smaller non-polar tail. Meaning Londons Forces is weak.

1-Octanol has larger surface area. Strong London forces, less soluble.

54
Q

Which compound is more soluble in water?

Why?

Alcohol: CH3CH2CH2OH

-OR-

Thiol: CH3CH2CH2SH

A

Alchohol

Because its polar and Thiol is not.

  • (like dissolves like)*
  • fyi**: Thiol has a* bad smell.. Skunky
55
Q

Which is more soluble?

Why?

A

B.

Because there is more EN. It has 2 Oxygens and the other only has 1 Oxygen.

56
Q

Bitter tasting = _________

A

Soluble

57
Q

______, inactive compounds that are converted to fully active drugs in the body.

A

Prodrugs

fyi**: hydrolysis of esters

58
Q

Concentration of Solutions:

The term _______ is used to refer to the amount of solute that is dissolved in a solvent.

A

Concentration

59
Q

Biochemical Hydrophilic Compounds-simple sugars:

Since like dissolves like, to be hydrophilic a molecule must resemble _______.

A

Water

fyi: (alcohol functional groups are polar. they are able to form hydrogen bonds with water.)

60
Q

Biochemical Hydrophilic Compounds-amino acids:

How can you determine that a compound is an amino acid?

A

If an NH2 is present then it’s an amino acid.

fyi: NH2 = Amine

61
Q

Biochemical Hydrophobic Compounds-fatty acids:

How can you determine that a compound is a fatty acid?

A

A carboxylic Acid is present.

&

A large non-polar tail is present.

62
Q

Amphipathic Compounds:

Compounds having both ________ and _________ parts are considered Amphipathic cooumpounds.

i.e: soap

A

Hydrophilic

&

Hydrophobic

63
Q

Amphipathic Compounds:

How is soap considered hydrophilic and hydrophobic?

A

Prior to double displacement the molecule is hydrophilic.

After double displacement the molecule becomes hydrophobic.

i.e: soap needs to be somewhat soluble.

64
Q

Which is more polar?

Carboxylate Ion

-OR-

Carboxylic Acid

A

Carboxylate Ion

65
Q

Pressure-Temperature Law is also called the ______________ Law.

Pressure _______ as Temp ________

A

Gay-Lussac’s Law = Pressure-Temperature Law

Pressure increases, as Temp increases

66
Q

Volume & Temperature Law is also called the __________.

Volume _______ as Temp _______.

A

Charles’ Law = Volume & Temperature Law

Volume increases as Temp increases

67
Q

Pressure-Volume Law is also called the __________ Law.

Volume _______ as Pressure _______.

A

Boyle’s Law = Pressure-Volume Law

Volume increases as Pressure decreases

68
Q

Commonly Encountered Concentration Units:

%(w/v) = ________

ppt = __________

ppm = _________

ppb = _________

(M) = __________

meq/L = ________

A

%(w/v) = Weight/Volume percent

ppt = Parts per thousand

ppm = Parts per million

ppb = Parts per billion

(M) = Molarity

meq/L = milliequivalents/litre

69
Q

Concentration:

Weight/volume percent =

A

g of solute / mL of solution x 100 = Weight/volume %

70
Q

Concentration of Solutions:

Ppt formula = _______

ppm formula = _______

ppb formula = _______

(M) Molarity = ________

meq/L = ____________

A

ppt = g of solute / mL of solution x 103

ppm = g of solute / mL of solution x 106

ppb = g of solute / mL of solution x 109

M = Moles of solute / L of solution

meq/L = # of moles of charges that 1 mole of a solute contributes to a solution.

fyi: (meq/L applies to ions, Na+, Br-, Ca2+, SO42-, etc.)

(i.e. 1mmol Na+ = 1 mEq Br- & 2mmolCa2+ =2mEqSO42-)

71
Q

What does the term concentration refer to?

A

Amount of solute that dissolved in a solvent.

fyi**: (solvent is typically water)

72
Q

What is an equivalent (Eq)?

A

The # of moles of charges that one mole of a solute contributes to a solution.

fyi**: (applied to ions)

73
Q

Fill in the blanks:

1 mol of K+ = ______ Eq of K+

1 mol of Mg2+ = _____ Eq of Mg2+

1 mol of Al3+ = ______ Eq of Al3+

A

1

2

3

74
Q

Solutes move from areas of higher solute concentration to those of lower solute concentration in a process called __________.

A

Diffusion

75
Q

Solvent(water) moves across a membrane from a solution of lower solute concentration to one of higher solute concentration in a process called ________.

A

Osmosis

fyi**: (semi-permeable membrane)

76
Q

How long does concentration occur?

A

Until both sides are equal

fyi: (equal ratio of concentrations.. 1:2 & 1:2)

77
Q

Cell membranes are semipermeable and hence affected by _______.

A

Osmosis

78
Q

Isotonic solution = ______% glucose solution & _______% NaCl solution

A
  1. 5% glucose solution
  2. 95% NaCl solution
79
Q

Hypotonic solution =

A

Less than 5.5% glucose & 0.95% NaCl

fyi**: (solution is less concentrated compared to isotonic solution.)

80
Q

Hypertonic solution =

A

Greater than 5.5% glucose & 0.95% NaCl.

fyi: (greater concentration compared to isotonic.)

81
Q

Crenation =

Hemolysis =

A

Hypertonic

Hypotonic

82
Q

Scuba Diver Questions:

If the question mentions pressure in lungs it’s referring to _________ Law.

If the question mentions bends it’s referring to ___________ Law.

A

Lungs = Boyles Law

Bends = Henrys Law

83
Q

02 tank questions:

02 storage: Pressure _______ as temp _________.

02 used at hospital: Pressure _______ as temp _______.

A

Pressure decreases as temp decreases,

pressure increases as temp increases.

fyi**: (careful storing 02 tanks in warm places, bang!)

84
Q

Hypotonic, Hypertonic, or Isotonic?

A

Isotonic fyi:(5.5%glucose, 0.95%NaCl)

Hypertonic fyi:(less than 5.5%glucose, 0.95%NaCl)

Hypotonic fyi:(more than 5.5%glucose, 0.95%NaCl)

85
Q

What is dilution?

Give a useful equation for dilution.

A

When a solvent is added to a solution

V1 x C1 = V2 x C2

fyi: (dilutions important in health carebecausedilution of drugs.)

86
Q

What happens to the solubility of CO2 in water in each of the following conditions:

a. The pressure of CO2 over the solution is increased.
b. The temperature is increased.

A

a. Solubility of CO2 increases
b. Solubility of CO2 decrease

(solubility of a gas)

87
Q

How does a Hyperbaric Chamber work?

A

High Patm = less gas solubility, which means more O2

High levels of O2 kill bacteria

88
Q

Explain the effects of Bends with divers.

A

Bends

On resurfacing, divers experience lower Patm so SN2 decreases.

N2 seeps out damaging arteries.

89
Q

Diffusion VS. Osmosis

A

Diffusion = High to Low

Osmosis = Low to High (w/ semi-permeable membrane)

90
Q

Explain how dialysis works.

A

Dialysis is used to cleanse the blood of patients whose kidneys malfunction.

Blood is diverted from the body, pumped through a long semipermeable dialysis tube and suspended into an isotonic solution.

Small waste materials such as urea pass through the dialysis membrane.

Protein molecules are too large to pass through the membrane.

91
Q

Reverse Osmosis-Desalination of sea water:

Desalination = _________

A

Desalination = Removal of salt water through osmosis

Scott (26 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions