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Chem test 3
| Question | Answer |
|---|---|
| conversion between mmhg and torr | they are the same value |
| conversion between celcius and kelvin | C + 273 = K |
| conversion between mmHg and atm | mmHg/760 = atm |
| ideal gas law equation | PV = nRT - this equation works under any temp and Pressure conditions -n is moles -R is the FACY PHYSICS THINGY (0.0821 ATM x L/mol x K) -T is Kelvin -V is Liters -P is ATM |
| combined gas law equation | P1V1/1T1 = P2V2/1T2 -temperature must be in K -other units must match |
| ___ mol @ standard temp and P = ___ L | 1 mol = 22.4L molar volume |
| gas stoiciometry | volume and moles (coeficients in equation) of a gas @ same T + P are = -can convert vol to vol take the L given and then multipy by a ratio (based on the balaced equation (EX 0.5 mol O2/ 1 mol SO3) |
| Graham's Law equation | m1v1² = m2v2² m = molar mass, g/mol v = velocity m/sec @equal kinetic energy |
| gas density equation | d = P (MM)/RT T = Kelvin P = atm mm = g/mol r = ideal gas constant = 0.0821 L⋅atm/mol⋅K d = g/L |
| @ STP | at standard temp and pressure 1.00 atm 0 degrees C (273 K) |
| haber process (practice writing name and pronouncing it) equation | N2(g) + 3H2(g) <---> 2NH3(g) synthesis reactions for Ammonia gas |
| haber process | goal: make more NH3 1. increase p 2. catalyst increased the rate 3. cooled the reaction to make liquid NH3 4. be able to draw the chart in notes |
| Dalton's law (def from the notes) | -in a mixture of gases, each gas exerts its own preasure called a "partial preassure" |
| partial pressure | The pressure that each gas would exert if it occupied the entire volume alone at the same temperature. |
| Boyle's law | preasure ---> (works both ways) volume have an inverse relationship as preasure increases, volume decreases Works both ways (pressure and volume) as long as the temperature is constant. |
| Charle's law | temp ----> volume have a direct relationship as temperature increases, volume increases Works both ways (volume and temperature) as long as the pressure is constant. |
| Gay-Lussac's Law | temp -----> pressure have a direct relationship as temp increases, preasure increases Works both ways (pressure and temperature) as long as the volume is constant |
| boiling point and freezing point of water | fp = 0 C or 273 K bp = 100 C or 373 K |
| If the temperature goes up x degrees celcius, then it also goes up | x degrees K |
| volume conversions | 1000 mL = 1000 cc (cubic cm = 1 cm deep, 1 cm wide, 1 cm tall) = 1L = 10^-3 m^3 (cubic meters) |
| pressure conversions | 1 atm = 7g0 torr = 760 mmHg = 14.7 psi = 101.3kPa (kilopascals) |
| law of combining volumes | if a reaction takes place at the SAME T & P, the coefficients in the equation can mean "Liters". -use stoichiometry to convert L to L |
| why was the haber process nessesary | equalibrium didn't like to go forward so Haber figured out how to produce more NH3 -prevent the procuct from shifting back to reactants |
| dalton's law formula and uses | P1 +P2 +P3 + .... = Ptotal -used when gases are purified through water, subtract partial pressure of the water vapor from total, the partical pressure of the water vapor is dependent on the T |
| behavior of an ideal gas | 1. great distance between gas particles 2. the volume of the gas is the volume of the container 3. particles in constant random motion, particles travel in straight lines 4. no attraction or repulsion between gases |
| gas mixtures | Ptot = nART/V + nBRT/V + ..... replace Pa with it's requivalent using the ideal gas law -we rearranged PV = nRT so that it is P = |
| mole fraction (X) | moles of gas A/Total moles |
| how to find the partial preassure of a specific gas in a mixture | Pa = XA Ptot mol fraction of gas TIMES the total pressure of the mixture |
| when given the total pressure of a mixture as well as the percent of each gas present, find the partical pressure of each gas | 1. Unless told otherwise, assume %s are by mass (% of the total mass the gas is) -assume 100g total 2. take off % (if by mass), convert to mol, + them for the Total mol 3. make X 4. multiply X by total P -check ans: + up answers, should = total P |
| observing the water vapor chart | assuming H2O is liquid @ 0 C the VP of H2O isn't zero -H20 Mcs can even escape from ice (though ice has a lower VP than liquids) -@ 100 C the VP of H20 is equal to the P of the atms, so it boils 0 k = O torr |
| what do water vapor pressure charts show | based on the T, how much P is the H20 vapor contributing hotter = more H2O vaporizing = higher P |
| how does prassure work | vapor/gas molecules coming up from the water pushes up against the downward push of the atmosphere below 100 C, the Atm P is higher than the VP @ 100 C, the atm = the VP above 100C the VP > atm |
| given a balanced equation given the the P and the T of a reactant find how many liters of the reactants are required to react completely with ___ g of the other reactant | 1. convert g into moles and then moles to moles of the other reactant 2. plug into PV - nRT |
| when given equation given the density of of reactant B, the volume of product A, the P, the T | 1. PV = n RT to find the moles of A 2. convert moles of A into gram of B 3. if B is H2O, then the d = 1 (1 g per 1 mL) so g = ml. otherwise, use density equation to find ml of B |
| given balanced equation given moles of reatant A, moles of reactant B, total P find the partial pressure of all the gases present NOTE: "the above reaction proceeds to completions" mean that it is not equalibrium | use an Ice chart find the End pressures of each compound add up the end pressures for the total preasure make mole fraction usual the total P we found multiply X by the acctual total pressure BOOM |
| when to use an ice chart? | whenever a rxn occurs and gives you the beggining and ending measurements -if things are changing |
| intermolecular forces | forces between molecules -opposites attract = "electrostatic attraction" = coulomb's law |
| London Dispersion forces | -a momentary dipole -just by chance, the e- in a mc might end up more on one side of the mc than the other. this often induces a temporary diople in a nearby mc |
| LDF strength | -ranges from weak to strong -the more polarizable an electron cloud is, the stronger LDF -more surface area (atomic radius) in an atom --> more e- interact --> more LDF |
| polarizability | how easily the e- cloud of an atom or mc can be distorted by nearby charges -the more easily the e-s move, the more polarizable -small atoms --> nucleus has strong hold ---> hard to polarize -big atoms -->more e- --> more polarizable |
| compare LDF to other IMF | -indivisually they are much weaker than other LDF, but the net LDF between large mcs is often the strongest force -large mcs have many e-s and large surfaces, so there are many places for temporary dipoles to interact |
| which bonds have a greater effect on LDF | pi bonds -form temporary dipoles more easily they are more spread out and looser than sigma (e- are easier to move around) -e- are above and below the nuclei, not directly between them (look up photo) |
| dipole dipole | -permanent dipole -medium strength -between a polar mc and another polar mc -stronger than LDF |
| hydrogen bonding | -between H atom and unshared e- in a different molecule -mcs need to have h bonded to N or O or F (they must be connected by a shared pair/line in it's structure) -a specifal form of dipole-dipole -strong |
| why in HB does an H have to be paired specifically with F O or N | F O and N are so electrongegative that they "hog" all the electrons and make the H+ more positive |
| real gas law | -there are problems w/ the ideal gas law cause real gases occupy space and have IMF |
| how do real gases deviate from the ideal gas law about V | volume of the container is not equal to the volume of the gas -V = the amount of space the gas particles have to move around in -the gas particles themselves take up some of this space so the volume os the gas is slightly less from the container |
| how do real gases deviate from teh ideal gas law about IMF | -the IMF causes the gas particles to hit the wall with less frecuencey -P observed is lass than P ideal |
| what make the differences between real and ideal gases to become more drastic | low T and high P -the gas is closer to liquid state T: whent eh particles move slower, they have more time to intereact when they pass eachother (IMF have stronger effect) P: the gas is compressed and the V available for movement is less |
| ideal gas law ammendment | Van der Waal's equation (P + n²a/V²)(V - nb) = nRT a = correction for attraction (HB, DD, LDF) (CONSTANT) b = correction for volume (bigger mc = bigger b) (CONSTANT) units: atm, L, mol, K |
| kinetic molecular theory | -relates the macroscopic properties of gases to motions of the particles in the gas (how the microscopic motions of particles (speed, collisions, energy) connect to the macroscopic properties we measure (pressure, temperature, volume) |
| kinetic moleular theory explain that | -all particles are in continuous random motion -the average kinetic energy of a particle is related to its average velocity (KE = 1/2mv²) -the average kinetic E of gases is directly proportional to K temp |
| effusion | flow of gas through a hole -gas particles bounce around until one finally escape trhough the hole of the container -effusion = how fast particles do this lighter (lower molar mass) gases move faster, so they effuse more quickly. |
| In an effusion expierement they give the amount of time it takes each gas to pass through a membrane. The T is the same for both gases. You're given only one molar mass. Find the other molar mass | -assume 1 event or 1 membrane per unit time (time does not have to be over distance) so one over the amount of time given is the velocity |
| what does 0 K mean | -no KE -no movement |
| what is not ideal about the ideal gas law | P and V |
| when given two molecules/atoms, which has a bigger a value and which a bigger b value | bigger a --> more IMF bigger b --> bigger atom/mc |
| proportionas of the velocities of two gases and the molar masses of two gases | v₁/v₂ = √(M₂/M₁) |
| when given two compounds, determine which is most ideal | more ideal = smaller & least IMF |
| how to make a gas more ideal | increase T and decrease P |
| translational energy | the kinetic energy a particle has because of its motion from place to place The energy they have just because they are moving from place to place is called translational energy. |
| what determines the translational energy | Depends only on temperature The hotter the gas, the faster the particles move, so the more translational energy they have. (speed is different from energy) same temperature → they all have the same average translational energy. |
| how the amount (moles) of gas being effused affects the rate of effusion | the effusion rate doesn't change based on the moles, lighter gases, no matter how much you have, will alawys effuse faster than heavier gases the more particles you have, the more particles leave per second |
| is vapor pressure affected by volume or surface area | NO |
| covalent molecular | -indivisual atoms -covalent compounds -when they react, nobel gases are covalent (cause it's harder to completly lose or gain e- from a full shell) - - |
| covalent molecular properties | LOWEST mp and bp of all solids -mcs held together by IMF - |
| the strength of LDF is based on | the number of e- |
| the strength of dipole-dipole based on | the strength of polarity (differences of electronegativity) |
| ionic | -indivisual atoms -formula units - |
| ionic properties | -form crystal lattice structures -DO'"T conduct electricity in solid form but DO in molten form or aq form (because of mobile charged particles - ions) -Coulomb's explains strength of interactions between cations & anions |
| crystal lattice | 3D repeating arrangement of atoms, ions, or mcs in a solid |
| why do ionic structures only conduct electricity in certain forms | the ions in solids are held in a lattice. Thay can't move freely so no eletric current can flow -heat or H2O breaks the lattice, so ions are free to move electric current: moving ions carrying a charge |
| why might one ionic compound have a stronger ionic bond than another | the stronger compound is smaller meaning that their nuclei are closer together -look at their shells |
| covalent network | -atoms connected by covalent bonds in a continuous #D swtructure -AKA macromolecules -one extremely large, interconnected entity (you can't isolate one molecule) |
| covalent network properties | highest melting points of all solids |
| allotropes | different forms of the same element in the same physical state w/ different structures and properties |
| allotropes of carbon | diamond graphite buckeyballs |
| diamond | so hard becuase it's strong in all 3 dimensions |
| graphite | has a weak demention -when you write you rip these sheets apart |
| buckeyballs | forms an acctual ball shape -the classic version has 60 carbons -they can be streched out into nanotubes |
| metallic | group of atoms lose their val e- to become more stable. The delocalized e-s form "sea of e-" & [the attraction between e-s and the newly formed cations - metallic bond] glues the structure. The cations form a crystal lattus & sea of e- acts as glue. |
| metallic properties | conducts electricity in all forms uses valance electrons for bonding the greated the # of val e- the stronger the bond |
| why do metallic bonds conduct electricity so well? | When an electric field is applied, these free-moving electrons can easily carry an electric charge throughout the material |
| metal alloys | -def: a mixture of elements with metallic properties -type of metallic bond - |
| substitutional alloys | -form between atoms of comparable radius where one atom substitutes for the other (some of the atoms in the metal lattice are replaced by atoms of a different metal) |
| interstitial alloy | form between atoms of different radii, where the smaller atoms fill the intersitial spaces between the larger atoms -the atomic radii must be diferent sies or else one won't fit in the other |
| interstices | spaces |
| properties of liquids | Evaporation - in an open container, fast moving mcs near the surface of a Liquid escape & diffuse into air 2. VP -pressure is constant no matter the container size -increase temp = higher VP -every liquid has a VP |
| vapor pressure | the preasure exerted by the vapor over a liquid |
| why increasing the temp causes the VP to become higher beacuse | 1. more vapor molecules 2. vapor molecuels move more quickly |
| volatile liquid | has a high VP -evaporates easily at normal temps becuase it has weak IMF |
| vapor equalibrium | dynamic equ - rate of vaporization EQUALS the rate of condenstation -the amount of gas and liquid remains constant -equalibrium is shifted with temperature change |
| boiling point | the point at which the vapor pressure of the liquid equals the pressure above its surface (Boiling = equalibrium) (rate of evaporations = rate of condenstation) -the lower the atmosphereic preassure, the lower the bp is |
| boiling points of liquids are based on | the types of forces between the particles -if only LDF, go by the number of electrons -"normal" boiling point = 1 atm pressure |
| when given: grams of liquid temperature of liquid the volume of the flask the liquid is introduced to the vapor preassure of the water at that temp How much liquid will remain when equalibrium is established? | 1. find the moles of the liquid using ideal gas law 2. convert into grams --> this is the amount of liquid that will vaporize under the conditions of the new container 3. subtract this from the origininal mass of liquid 4. BOOM |
| name the only covalent networks we will be dealing with | pure carbon and SiO2 -everything else that is covalent is covalent molecular |
| phase diagram | a graph of pressure (y-axis) VS temperature (X-axis) -depicting 3 phases of a substance |
| triple point | -at a certain T and P, all 3 phases exsist -be able to label on phase diagram |
| deposition point | gas --> solid |
| sublimation point | solid --> gas |
| critical temperatue | the temperature above which gases cannot liquefy -the preassure doesn't matter -highest temperature where a gas can exsist as a liquid |
| as you increase preassure and keep T constant | you favor the more dense phase of the substnace |
| lines on the phase diagram are | equalibrium systems - molecuels are constantly moving between the two phases, but the amount of each phase stays the same |
| -if a gas is put under very high P | ,it will liquefy |
| critical preassure | the minimum preassure required to liquidfy a gas at it's critical temperature |
| how is the line between the solid and liquid phases on the phase diagram differnt for water | normally: the sold to liquid line has a positive slope (-increasing the P makes it solid) h2O: negitive slope -water: a higher P makes it liquid -when H2O freezes it expands (ice is less dense than liquid --> HB creates an open hexagonal structure) |
| order the different bonds from strongest to weakest | covalent network, ionic, metallic, interstitial alloys, substitutional alloys, covalent molecular |
Created by:
Blessed Rectangle 10