Chemistry 3 Flashcards
- Phase changes
- How is vapor pressure affected by temperature?
- Increased temperature increases vapor pressure.
- This makes logical sense for a few reasons.
- First, increased temperature means the molecules of the liquid have a higher average kinetic energy.
- This indicates that a larger fraction of those molecules will have the energy necessary to escape the intermolecular forces between liquid molecules to enter the gas phase.
- First, increased temperature means the molecules of the liquid have a higher average kinetic energy.
- One could also remember that liquids boil when their vapor pressure increases to the point that it equals atmospheric pressure.
- It obviously requires an increase in temperature to cause a liquid to boil, therefore increasing temperature must increase vapor pressure.
- Solution Chemistry
- Ways of measuring & describing solution []
- Compare Molarity with Molality
- How do they both change with temperature?
- Compare Molarity with Molality
- Ways of measuring & describing solution []
- Molarity, M
- =moles solute/Liter solution
- Molality, m
- =moles solute/Kg solvent
- ***
- Molarity (M) changes w/ temperature, but molality (m) DOES NOT!
- Provide a possible explanation…
- Hint: what happens to volume when temperature increases? (increases. Mass doesnt change though)
- Solution Chemistry
- Ions in Solution
- What do Na+ and Cl- look like in water?
- In specific, how are the dipoles oriented?
- Ions in Solution
RAOULT’S LAW
(Solving for vapor pressure of a solvent + impure solute)
VpTOTAL=XVp
How do you solve for the mole fraction,”X?”
Given: grams of solvent and solute
Once you find X, how do you solve for VpTOTAL?
Given: grams of solvent &solute
- Find respective # of MOLES of both
Add them together=TOTAL # of MOLES
- Divide # of INDIVIDUAL MOLES of solvent & solute
- …by TOTAL # of MOLES
THIS IS YOUR MOLE FRACTION, X
SOLVENT & SOLUTE COMBINED MUST EQUAL 1.0!!
- Now, simply multiply X’s for solvent & solute by their respective vapor pressures, Vp
ADDING THESE TOGETHER GIVES: VpTOTAL
- Solution Chemistry
- “like dissolves like” refers to?
- Describe Ksp (3 points)
- “Like dissolves like” refers to the fact that polar substances are soluble in polar solvents and non-polar substances are soluble in non-polar solvents.
- Polar and non-polar substances DO NOT form solutions.
- The Solubility Product Constant, Ksp
- Exactly the same thing as Keq, Ka, and Kb.
- Like all the other K’s, remember the following:
- Leave out pure liquids and pure solids (this will make all Ksp equations only have a numerator - if you have something in the denominator of a Ksp equation, you’ve made a mistake).
- Temperature is the ONLY THING that changes Ksp
- Ksp can ONLY be observed in a saturated solution.
- This is because saturation is the point at which the dissolution reaction has reached equilibrium.
- In other words, it’s just like all other equilibrium constants—you cannot measure them anywhere other than at equilibrium.
- Galvanic Cells
- What is used to create a Galvanic Cell?
- What will a correctly set up galvanic cell always produce?
- Describe direction of electron flow in a galvanic cell
A functioning Galvanic cell can be created using any two metals, regardless of their reduction potentials.
- If a galvanic cell is properly set up, it will always produce current.
- Electrons will automatically flow from the species with the lower reduction potential to the species with the higher reduction potential.
LO⇒HI
- Gases
- The Ideal Gas Law
- What is “STP?”
- Give the values for P,V,n,R,&T
- The Ideal Gas Law
- Standard Temperature & Pressure (STP)
- A set of standard conditions true of any ideal gas said to be “at STP.”
- For the MCAT, unless you are specifically told otherwise, assume that all gases are ideal and start out at STP.
- At STP the variables in the Ideal Gas Law are defined as follows:
- P = 1 atm
- V = 22.4 L
- n = 1 mole
- R = 0.0821 L*atm/mol*K or 8.31 J/mol*K
- T = 273 K (0°C)
- Gases
- Real Gases
- Van der Waals Equation
- What are the only 2 things you need to know about the VDWs equation?
- Real Gases
-
[P+a’(n/2V)2]*[(V/n)-b’]=RT
- a’
- is a constant that represents the actual strength of the IM attractions
- b’
- is a constant that represents the actual volme of the molecules
- a’
- Increased intermolecular attractions (a’)
- decrease pressure in real gases.
- The larger a’ is, the larger the second term will become and therefore the smaller P will be.
- Increased molecular volume (b’) increases volume in real gases.
- Solution Formation
- Describe the difference b/t a (+) and (-) ΔHsolution
NEGATIVE
exothermic and heat will be released
POSITIVE ΔHsolution=
A positive heat of solution means that energy must be ADDED to the system to make the solute dissolve.
For a solution to form, the intermolecular forces between the solute particles must first be broken;
- then any intermolecular forces between the solvent particles must be broken
- (to make room for the solute)
- Finally, new intermolecular forces are formed between the solute particles and the solvent particles.
- If the new intermolecular forces formed are greater (i.e., stronger, more stable) than the sum of the intermolecular forces that had to be broken, net energy is released and the solution is said to have a negative Heat of Solution (ΔHsolution
- This means that the dissolution process is exothermic and heat will be evolved.
- If the new intermolecular forces are not more stable than the old ones, the solution has a positive ΔHsolution.
- A positive heat of solution means that energy must be added to the system to make the solute dissolve
- Gases
- The Ideal Gas Law=?
-
PV = nRT
- R = 0.0821 L*atm/mol*K or 8.314 J/mol*K
- Phase changes
- Heating Curves
- Describe them
- Heating Curves
- A graph of temperature (T) in Kelvin or Celsius vs. heat (q) in Joules.
- Occasionally, time is graphed on the x-axis instead of heat
- (if heat is added at a constant rate the temperature vs. heat graph and the temperature vs. time graph look approximately the same).
Phase Changes
- Describe Osmotic Pressure
- What side RECEIVES water?
- More___=More OSMOTIC PRESSURE
- A measure of the tendency of water to move from one solution to another across a semi-permeable membrane
- Usually represented by the capital Greek letter pi, Π.
- It is the side that will receive the water via osmosis that has the higher osmotic pressure.
- In other words, more solute means more osmotic pressure.
Π= iMRT
- i = # of ions formed in solution
- M is the solute molarity
- R is the gas constant
- T is the absolute temperature
The Ideal Gas Law
- STP
Define Absolute Temperature
-
What is it measure relative to?
- What’s happening on a molecular level at the point Abs. Temp. is relative to?
An absolute temperature is any temperature measured relative to absolute zero
- The Kelvin scale is measured relative to absolute zero
- where absolute zero is defined as 0 degrees Kelvin
- ∴ all Kelvin temperatures are absolute
- where absolute zero is defined as 0 degrees Kelvin
- Absolute zero is a theoretical temperature limit where all molecular motions cease
- Solution Formation
- What happens to entropy when a solution forms from a solute?
- The dissolution of a solute into a solution is accompanied by a very large, positive change in entropy.
- A solid or crystal is highly ordered and the break-up and solvation of that solid into individual molecules represents a significant increase in disorder
- Gases
- The Ideal Gas Law
- The Kinetic Theory of Gases
- Describe it in general
- The Kinetic Theory of Gases
- The Ideal Gas Law
- Theoretical model used by scientists to study and predict the “ideal” behavior of gases.
- Phase Changes
- Define a phase change
- In common use, the term “phase” is used to distinguish between the solid, liquid, and gas forms of a substance.
- Solid, liquid and gas are more correctly called “states” (a.k.a., “states of matter”).
- *
- Gases
- Dalton’s Law of Partial Pressures
- Ptotal=P1+P2+P3….
- This seems pretty straightforward; the sum of the partial pressures equals the total pressure.
- However, if you gloss over this you will miss a very important point.
- If we add more of Gas 1 (P1) to an existing mixture of three gases, we have increased the partial pressure of Gas 1 and the total pressure, but have had zero effect on the partial pressure of the other gases.
- Partial pressure is NOT similar to mole fraction or mass percent.
- By adding more of Gas 1 we did decrease the mole fraction and the mass fraction of Gases 2 and 3, but we did NOT decrease their partial pressures.
Phase Changes
- Vapor Pressure
Raoult’s Law
- What does Raoult’s Law solve for?
- Give the formula for vapor pressure w/ a NON-Volatile solute
SOLVES FOR VAPOR PRESSURE OF A SOLVENT THAT HAS A SOLUTE ADDED TO IT
VpTotal = XVp°
Vapor Pressure w/ a Non-Volatile Solute =
(mole fraction of the pure solvent, X)
X
(Vp of the pure solvent, Vp°)
- Phase Changes
- Draw a phase diagram. Label:
- axes
- solid, liquid, gas regions
- critical point
- triple point
- Describe what’s going on at the critical & triple points wrt phases
- Draw a phase diagram. Label:
- The triple point
- the precise temperature and pressure at which all three phases (i.e., states) exist simultaneously in equilibrium with each other.
- The critical point
- the precise temperature and pressure above which liquid and gas phases become indistinguishable.
- At this point liquid and gas phases cease to exist, merging into a single phase called a supercritical fluid.
- This supercritical fluid cannot be compressed back into the liquid phase by increasing pressure, nor can it be turned into a gas by increasing temperature.
- At this point liquid and gas phases cease to exist, merging into a single phase called a supercritical fluid.
- the precise temperature and pressure above which liquid and gas phases become indistinguishable.
- The critical temperature and the critical pressure are simply the temperature and pressure at the critical point.
- At the triple point all three phases are present.
- At the critical point none of the original three phases are present, only the new “supercritical fluid” phase.
- Phase Changes
- Heating Curves
- What do horizontal portions of the graph represent?
- What does the slope of the various non-horizontal sections of the graph represent?
- Heating Curves
- The horizontal sections of the graph represent phase changes.
- The first flat section will represent the phase change between solid and liquid and the second will represent the phase change between liquid and gas.
- If heat is on the x-axis then the length of the first horizontal section represents the heat of fusion and the length of the second horizontal section represents the heat of vaporization.
- The slope of the lines between these horizontal sections represents the inverse (∆T/Q) of heat capacity (Q/∆T) for that particular phase of the substance.
- One should observe, therefore, that different phases of the same substance usually have different heat capacities—as indicated by the differing slopes of those sections of the following graph:
- Solution Chemistry
- Ions in solution
- Define:
- Solvation
- Hydration
- Hydration Number
- Hydrate
- Anhydrous
- Aqueous
- Define:
- Ions in solution
-
Solvation
- a general term for the process wherein solvent molecules surround a dissolved ion or other solute particle creating a shell.
-
Hydration
- a specific kind of solvation wherein water is the participating solvent.
- Water molecules, being polar, can surround both negatively and positively charged solutes by directing either their partially-negative oxygen, or partially positive hydrogen, moieties toward the ion.
- a specific kind of solvation wherein water is the participating solvent.
-
The hydration number
- is the number of water molecules an ion can bind via this solvation process, effectively removing them from the solvent and causing them to behave more like an extension of the solute.
-
A hydrate
- an inorganic compound in which water molecules are permanently bound into the crystalline structure.
- The nomenclature of a hydrate is altered to reflect the presence of water molecules.
- For example, anhydrous cobalt(II)chloride contains no water, but cobalt(II)chloride hexahydrate [CoCl2∙6H2O] contains six water molecules complexed with each cobalt.
- As we see in these two names, the term anhydrous is often applied to a compound that can form complexes with water to differentiate molecules that do not contain water from those that do.
- an inorganic compound in which water molecules are permanently bound into the crystalline structure.
-
Aqueous
- efers to any solution for which water is the solvent.
Phase Changes
- Freezing Point Depression
- Freezing point of a liquid is depressed when a ____ _____ is added according to WHAT FORMULA?
- The freezing point of a liquid is depressed when a non-volatile solute is added according to:
∆T = kfmi
- kf is a constant (different than kb)
- Electrochemical cells
- Concentration cells
- Nernst Equation
- For a concentration cell, Eo will always be…?
- Concentration cells
- E=Eº-(.06/n)*log [lower]/[higher]
- n=moles of electrons transferred
- ex: Ag+(aq)⇒Ag(s)
- 1 electron transferred
- ex: Ag+(aq)⇒Ag(s)
- n=moles of electrons transferred
- Eo will always be ZERO
- Phase changes
- How does the addition of a non-volatile solute affect vapor pressure?
- What about a volatile solute?
BOTH DECREASE Vp
Non-volatile solute
Addition of a non-volatile solute DECREASES vapor pressure.
- The non-volatile solutes in solution occupy a portion of the limited surface area available for vaporization.
- Liquid molecules must be at the surface of the liquid in order to escape into the gas phase
Volatile solute
- When a volatile solute is added to a solvent it usually decreases vapor pressure for the same reason that a non-volatile solute decreases vapor pressure.
-
As long as the vapor pressure of the solute is LESS THAN the vapor pressure of pure solvent:
- addition of the volatile solute will decrease vapor pressure.
- However, if a solute is added that has a vapor pressure greater than that of the pure solvent:*
- then the vapor pressure of the solution will actually be higher than that of the pure solvent*
- Gases
- Solving Ideal Gas Law Problems
- Describe the 2 methods for approaching these problems
- Solving Ideal Gas Law Problems
- Manipulating Equations:
- Compare the variables for any system to the variables outlined above for STP.
- For any variation found, estimate the factor by which that variable has changed and use the manipulating equations skills to predict the effect that change will have on the unknown variable
-
P1V1/T1 = P2V2/T2
- (a.k.a., The Combined Gas Law)
- Because PV/T = nR and R is a constant, for the same number of moles of gas the ratio of PV/T must remain constant regardless of the changes made to the system.
- You can choose the first set of data as being STP, or as any other point where P, V and T are known.
- The second set of data will be different, but the ratio will always be the same.
- Plug in the data and solve for the unknown.
- Conceptually, you’re probably better off if you understand and can apply the first method.
- The first method is also much faster!
- The ratio given by PV/nRT tells us which of two assumptions is the major cause of the deviation from Ideal Gas Law behavior
- What are the 2 assumptions?
- Hint: If PV/nRT is > or
- If PV/nRT > 1 it is due mostly to the molecular volume assumption
- If PV/nRT it is due mostly to the intermolecular forces assumption
- Redox Rns
- Define Oxidation State
- Is the apparent charge that an atom takes while in a molecule
- The sum of oxidation states for all the atoms in a molecule must equal the charge of that molecule
- or equal zero if the molecule is neutral