Ch. 6 Gases & Solutions Flashcards
(91 cards)
1
Q
Patm = _______
A
Atmospheric Pressure
2
Q
psi = ________
A
Pounds per Square Inch
3
Q
Insoluble or Soluble? / Can it Hydrogen bond?
- Hydrophilic =
- Hydrophobic =
A
- soluble / Yes
- insoluble / No
* fyi: (**no hydrogen bonding = will dissolve)*
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)
5
Q
What unit of measurement is used when measuring atmospheric pressure?
A
Lenght (mm Hg)
6
Q
Diatomic = ______ atom(s)
A
Two
7
Q
Monoatomic = ______ atom(s)
A
One
8
Q
Water Vapor = ___________.
Vapor = ______________.
Vapor Pressure = ___________.
A
Gas
Gas from evaporation of liquid
Movement of particles from liquid to gas phase.
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
10
Q
Liquids boil when their ________ equals the pressure of the air above them.
A
Vapor Pressure
11
Q
Standard Temperature = _______
Standard Pressure = _________
A
Standard Temp = 0°C
Standard Pressure = 1 atm
12
Q
Which elements are gases at standard temperature and pressure (0°C & 1 atm)
A
H, N, O, F, Cl, & Noble gases
13
Q
Define: Sublimation
A
Solid to a gas without a liquid
fyi: (dry ice in balloon)
14
Q
At 100°C vapor pressure is 760.00 torr.
Convert 760.00 torr to mm Hg?
A
- 00 torr = 760 mm Hg
* fyi: (1 atm = 760 mm Hg / 1 atm = 760.00 torr)*
15
Q
As temp rises molecules move ________.
A
Faster
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.
17
Q
Gas Laws:
All gases behave in a ______ manor.
A
Similar
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)
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
20
Q
Gas Laws:
What does the dotted line represent?
A
Absolute zero
(- - -no data points- - -)
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
22
Q
Gas Laws:
In calculations, temperature should always be converted from °C to _____.
A
Kelvin
23
Q
Gas Laws:
Oxygen tanks get ____ when in use. The pressure inside the tank _______ as O2 exits the tank.
A
Cold
Decreases
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
25
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 \_\_\_\_\_\_.
Inversely related
Decreases
Increases
26
Gas Laws:
Respiration: inhaling and exhaling is an application of ______ Law.
Boyles Law
-OR-
Pressure-Volume Law
*(same thing)*
27
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.
Boyle's Law
-OR-
Pressure-Volume Law
*(same thing)*
28
Gas Laws:
A formula that combines Boyles, Charles' and Gay-Lussac's Law is called ____________ Law
The Combination Gas Law
29
Dalton's Law of Partial Pressure states that the total pressure of a mixture of gases is the \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_.
Sum of the partial pressure of its components
Ptotal = P1 + P2 + P3
30
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.
78. 0% N2
- and-
21. 1% O2
31
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.** because lower altitude means higher O2 levels.
32
Daltons Law:
Why do climbers often carry oxygen supplies?
Is PCO2 higher in the **lungs** or the **tissue**?
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)
33
A _________ consists of just one element or compound.
Pure Substance
34
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 = \_\_\_\_\_\_\_\_\_\_\_\_\_
Two rubber balloons = **Lungs**
Y-tube = **Trachea**
Open end of the Y-tube = **Nose / Mouth**
Bell Jar = **Thorax Cavity**
Thin sheet of rubber = **Diaphragm**
35
A combination of two or more pure substances is called a \_\_\_\_\_\_\_\_.
Mixture
36
Which are elements and which are compounds?
1. Mercury
2. Silver
3. Water (H20)
4. NaCl (salt)
5. Oxygen
6. Sucrose (sugar)
1. Element
2. Element
3. Compound
4. Compound
5. Element
6. Compound
37
Heterogeneous mixtures =
Homogeneous mixtures =
Hetero = Not evenly distributed; immiscible, insoluble. *i.e: (sand + H20)*
Homo = uniformly distributed; miscible, soluble. *i.e: (sugar + H20)*
38
Solvent =
Solutes =
Solution =
Solvents = The component in solution in greatest amount. (H20)
Solutes = The component dissolved in solution.
Solution = Solute + Solvent
39
What does *"Like Dissolves Like"* mean.
_Polar_ _solute_ **will dissolve in** _polar_ _solvent_.
_Nonpolar solute_ **will dissolve in** _Nonpolar solvent_
40
The formation of solutions requires that solute particles have two important characteristics.
1. \_\_\_\_\_\_\_\_\_\_\_\_\_\_...
2. \_\_\_\_\_\_\_\_\_\_\_\_\_\_...
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
\_\_\_\_\_\_\_\_\_ refers to the amount of solute that will dissolve in a given amount of solvent at a given temperature.
Temperature can affect \_\_\_\_\_\_\_\_\_*(directly related)*.
Solubility
Solubility
42
Most liquid and solid solutes become more soluble in water as temperature increases, why?
Because temperature affects the rate at which molecules are bouncing off one another.
*i.e: (high temp = more soluble)*
43
Electrolytes =
Compounds that dissolve in water to form ions.
44
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.
Transmission of nerve impulses ***(spasms)***
Muscle contraction and blood clotting ***(cramping)***
45
Solubility of a gas and temperature:
For all gaseous solutes (02, C02, etc.), an ________ in temperature leads to a _________ in solubility.
Why?
Increase
Decrease
The solubility of gaseous solute and temperature are inversely related. Temp increase causes molecules to move quicker and become more soluble.
46
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.
Pressure
47
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 \_\_\_\_\_\_\_\_.
Reduced
Bubbles
48
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.)*
Increases
***P.S. Henry is directly related***
49
Solubility of gas and temperature:
Give two applications that use Henry's Law.
1. \_\_\_\_\_\_\_\_\_\_...
2. \_\_\_\_\_\_\_\_\_\_...
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
Solubility of gas and temperature:
How does a Hyperbaric chamber work?
High levels of 02. Bacteria cannot survive in high levels of 02.
51
Solubility of Organic Compounds:
Pentane + Hexan =
Hydrophobic **or** Hydrophilic
Why?
Hydrophobic
Like dissolves like*(polar & polar)*.
*fyi: pentane & hexane cannot bond together.*
52
Solubility of Organic Compounds:
Alcohol + H20 =
Hydrophilic **or** Hydrophobic
Why?
Hydrophilic
Like dissolves like*(polar & polar),*
*fyi: alcohol & water can bond.*
53
Which compound is **more** soluble in water?
Why?
Ethanol: CH3CH2OH
-OR-
1-Octanol: CH3CH2CH2CH2CH2CH2CH2CH2OH
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
Which compound is **more** soluble in water?
Why?
Alcohol: CH3CH2CH2OH
-OR-
Thiol: CH3CH2CH2SH
Alchohol
Because its polar and Thiol is not.
* (like dissolves like)*
* fyi**: Thiol has a* *bad* *smell.. Skunky*
55
Which is more soluble?
Why?
B.
Because there is more EN. It has 2 Oxygens and the other only has 1 Oxygen.
56
Bitter tasting = \_\_\_\_\_\_\_\_\_
Soluble
57
\_\_\_\_\_\_, inactive compounds that are converted to fully active drugs in the body.
Prodrugs
*fyi**: hydrolysis of esters*
58
Concentration of Solutions:
The term _______ is used to refer to the amount of solute that is dissolved in a solvent.
Concentration
59
Biochemical Hydrophilic Compounds-simple sugars:
Since like dissolves like, to be hydrophilic a molecule must resemble \_\_\_\_\_\_\_.
Water
*fyi: (alcohol functional groups are polar. they are able to form hydrogen bonds with water.)*
60
Biochemical Hydrophilic Compounds-amino acids:
How can you determine that a compound is an amino acid?
If an NH2 is present then it's an amino acid.
*fyi: NH2 = Amine*
61
Biochemical Hydrophobic Compounds-fatty acids:
How can you determine that a compound is a fatty acid?
A carboxylic Acid is present.
&
A large non-polar tail is present.
62
Amphipathic Compounds:
Compounds having both ________ and _________ parts are considered **Amphipathic cooumpounds**.
*i.e: soap*
Hydrophilic
&
Hydrophobic
63
Amphipathic Compounds:
How is soap considered hydrophilic and hydrophobic?
Prior to double displacement the molecule is hydrophilic.
After double displacement the molecule becomes hydrophobic.
*i.e: soap needs to be somewhat soluble.*
64
Which is more polar?
Carboxylate Ion
-OR-
Carboxylic Acid
Carboxylate Ion
65
Pressure-Temperature Law is also called the ______________ Law.
Pressure _______ as Temp \_\_\_\_\_\_\_\_
Gay-Lussac's Law = Pressure-Temperature Law
Pressure _increases_, as Temp _increases_
66
Volume & Temperature Law is also called the \_\_\_\_\_\_\_\_\_\_.
Volume _______ as Temp \_\_\_\_\_\_\_.
Charles' Law = Volume & Temperature Law
Volume _increases_ as Temp _increases_
67
Pressure-Volume Law is also called the __________ Law.
Volume _______ as Pressure \_\_\_\_\_\_\_.
Boyle's Law = Pressure-Volume Law
Volume _increases_ as Pressure _decreases_
68
Commonly Encountered Concentration Units:
%(w/v) = \_\_\_\_\_\_\_\_
ppt = \_\_\_\_\_\_\_\_\_\_
ppm = \_\_\_\_\_\_\_\_\_
ppb = \_\_\_\_\_\_\_\_\_
(M) = \_\_\_\_\_\_\_\_\_\_
meq/L = \_\_\_\_\_\_\_\_
%(w/v) = **Weight/Volume percent**
ppt = **Parts per thousand**
ppm = **Parts per million**
ppb = **Parts per billion**
(M) = **Molarity**
meq/L = **milliequivalents/litre**
69
Concentration:
Weight/volume percent =
**g of solute / mL of solution x 100** = Weight/volume %
70
Concentration of Solutions:
Ppt formula = \_\_\_\_\_\_\_
ppm formula = \_\_\_\_\_\_\_
ppb formula = \_\_\_\_\_\_\_
(M) Molarity = \_\_\_\_\_\_\_\_
meq/L = \_\_\_\_\_\_\_\_\_\_\_\_
**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
What does the term concentration refer to?
Amount of solute that dissolved in a solvent.
*fyi**: (solvent is typically water)*
72
What is an equivalent (Eq)?
The # of moles of charges that one mole of a solute contributes to a solution.
*fyi**: (applied to ions)*
73
# 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+
1
2
3
74
Solutes move from areas of **higher solute concentration to those of lower solute concentration** in a process called \_\_\_\_\_\_\_\_\_\_.
Diffusion
75
Solvent(water) moves across a membrane from a solution of **lower solute concentration to one of higher solute concentration** in a process called \_\_\_\_\_\_\_\_.
Osmosis
*fyi**: (semi-permeable membrane)*
76
How long does concentration occur?
Until both sides are equal
*fyi: (equal ratio of concentrations.. 1:2 & 1:2)*
77
Cell membranes are semipermeable and hence affected by \_\_\_\_\_\_\_.
Osmosis
78
Isotonic solution = \_\_\_\_\_\_% glucose solution & \_\_\_\_\_\_\_% NaCl solution
5. 5% glucose solution
0. 95% NaCl solution
79
Hypotonic solution =
Less than 5.5% glucose & 0.95% NaCl
*fyi**: (solution is less concentrated compared to* *isotonic* *solution.)*
80
Hypertonic solution =
Greater than 5.5% glucose & 0.95% NaCl.
fyi: (greater concentration compared to isotonic.)
81
Crenation =
Hemolysis =
Hypertonic
Hypotonic
82
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.
Lungs = Boyles Law
Bends = Henrys Law
83
02 tank questions:
02 storage: Pressure _______ as temp \_\_\_\_\_\_\_\_\_.
02 used at hospital: Pressure _______ as temp \_\_\_\_\_\_\_.
Pressure decreases as temp decreases,
pressure increases as temp increases.
*fyi**: (careful storing 02 tanks in warm places, bang!)*
84
Hypotonic, Hypertonic, or Isotonic?
**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
What is dilution?
Give a useful equation for dilution.
When a solvent is added to a solution
V1 x C1 = V2 x C2
***fyi******: (dilutions important in health care******because******dilution of drugs.)***
86
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. Solubility of CO2 increases
b. Solubility of CO2 decrease
(solubility of a gas)
87
How does a Hyperbaric Chamber work?
High Patm = less gas solubility, which means more O2
High levels of O2 kill bacteria
88
Explain the effects of **Bends** with divers.
_Bends_
On resurfacing, divers experience lower Patm so SN2 decreases.
N2 seeps out damaging arteries.
89
Diffusion VS. Osmosis
Diffusion = High to Low
Osmosis = Low to High *(w/ semi-permeable membrane)*
90
Explain how dialysis works.
*_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
Reverse Osmosis-**Desalination** of sea water:
Desalination = \_\_\_\_\_\_\_\_\_
Desalination = Removal of salt water through osmosis
