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Chem Exam 3
| Term | Definition |
|---|---|
| how do you get the limiting reactant | grams a ---> MM of A -----> molar ratio ----> MM of B |
| theoretical yield | the limiting reactant in the chemical reaction |
| percent yield | (actual/theoretical)*100 |
| nonelectrolytes include | alcohols (-OH), alkanes (-CH), carbohydrates (SO2,NO2etc) |
| strong electrolytes include | strong acids or bases |
| strong acids | HCl, HI, HBr, H2SO4, HClO4, HNO3 |
| Weak acids | CH3COOH (carboxylic), HNO2, HF |
| Strong bases | LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2, NH4OH |
| molarity | mols solute / liters of solution |
| dilution problems | M1V1 = M2V2 |
| Soluble compounds | group A1 cations, NH4+, Cl-,Br-,I-, NO3-, ClO4-, CH3CO2-, SO4-2 |
| exceptions to soluble Cl-, Br-, I- | Ag+, Hg2+2, Pb+2 |
| exceptions to soluble for SO4-2 | Sr+2, Ba+2, Hg2+2.Pb+2, Ca+2 |
| Insoluble Compounds | CO3-2, S2-2,PO4+3,OH- |
| what are exceptions to all insoluble compounds | group 1A cations, NH4+ |
| exceptions to sulfide (S2-2) | group 1A cations, NH4+, Ca+2, Sr+2, Ba+2 |
| exceptions to hydroxide (OH-) | group 1A cations, NH4+, Ca+2, Sr+2, Ba+2 |
| arrhenius acid | substances that produce H+ ions in water (any acid that has H+ in formula) |
| arrhenius base | substance that produce OH- |
| Bronsted-Lowry acid | H+ donor |
| Bronsted-Lowry Base | proton acceptor |
| rules for determining oxidation numbers must be in order | atoms in elemental form=0, monoatomic ions charge on ions, F=-1 when with another element, H are +1 when combined with another metal, O = -2 except in peroxides (then O=-1), Cl Br I = -1 expect when with O or F |
| atoms in elemental form | 0 |
| monatomic ions | charge on ion |
| F | -1 when combined with a metal |
| H | +1 when combined with a metal |
| O | -2 |
| what is O in peroxide | -1 |
| Cl, Br, I | -1 |
| OIL RIG | oxidation is loss of electrons, reduction is gain of electrons |
| how to balance oxidation/reduction reactions | split up into 2, balance # atoms, then add electrons (only add), multiply until each one is equal to another, add half reactions together and cancel out e- |
| oxidized species | reducing agent |
| reduced species | oxidizing agent |
| if it asked for species | use normal rule |
| what is the SI unit for pressure | Pa (pascal) |
| 1 atm = _____mmHg | 760 mmHg |
| 1 atm= _______torr | 760 mmHg=760 torr |
| 1 atm = __________Pa | 101,325 Pa |
| boyles law | P1V1=P2V2 , when volume decreases pressure increase (constant moles) |
| charles law | V1/T1=V2/T2, when temperature increases, volume increases (constant moles and pressure) |
| Avgrados law | V1/N1=V2/N2, when volume increases, moles increase (constant temp and pressure) |
| what is standard temperature and pressure for ideal gases | temp: 0 ; pressure: 1 atm (1 barr) |
| what is volume at STP | 22.4L |
| ideal gas law | Pv=NRT |
| what is R in ideal gas law | 0.08206 |
| when does ideal gas work best | low pressures and high temps |
| in a manometer | Pgas=Patm (- +) h |
| if Pgas < Patm | Patm - h |
| if Pgas > Patm | Patm + h |
| equation for molar mass with Pv=NRT | (density*RT/P) or (mass*RT/PV) |
| when does density increase | pressure increases, |
| when does density decrease | pressure decreases |
| density at low pressure can be | significant |
| density ______ when molar mass ______ | decreases, decreases |
| Ptotal | ntotal (RT/V) |
| mole fraction | moles of a / ntotal |
| when do you use mole fraction | whenever volume and pressure are the same for both gases |
| partial pressure of water vapor (vapor pressure), depends ONLY on | temperature |
| Ptotal for gas collected over water in barometric | Pgas + Pwater |
| laws for kinetic energy | volume of individual particles can be assumed negligible, particles in constant motion (collisions cause pressure), particles exert no forces on each other and do attract or repel, avg KE of gas particles are directly proportional |
| when KE increases | temperature increases |
| when temp is constant | KE doesn't depend on identity |
| Urms (KE) | sq root (3RT / M) where R is 8.314 |
| when temp is higher | higher Urms |
| higher M | lower Urms |
| as temp increases molecular velocity | increases |
| as molar mass increases | velocity decreases because molecules become heavier |
| how to read a boltzmann distribution | the lowest peak has the lowest MM and highest velocity. |
Created by:
leximohammed