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| 6365473850 | Electrolyte | Substance that dissociates into ions when dissolved in water (strong - completely, weak - partially) - ions in water conduct electricity if covalent (delocalized electrons, moving charged particles) | 0 | |
| 6365475467 | Nonelectrolyte | May dissolve in water, but it does not dissociate into ions when it does so | 1 | |
| 6365521986 | Precipitate | when 2 solutions containing soluble salts are mixed, sometimes insoluble salt will be produced. | 2 | |
| 6365531183 | Acids | Proton donor (Lowry). Strong acids completely dissociate, weak acids partially= HCl, HNO3, H2SO4, HClO4, HI, HClO3, HBr | 3 | |
| 6365547924 | Bases | Proton acceptors (Lowry). strong bases dissociate to metal cations and hydroxide anions in water; weak bases only partially react to produce hydroxide anions. | 4 | |
| 6365555858 | Neutralization Rxn | Ron between an acid and a base | 5 | |
| 6365563365 | Single Displacement Rxns | ions oxidize an element. elements higher on the activity series are more reactive (active). | 6 | |
| 6365587334 | Characteristics of Gases | - nonmetallic elements -expand to fill containers -highly compressible -low density -2 or more form a homogenous mixture (can change it by moving due to non chemically bonded components) | 7 | |
| 6365595718 | Properties of a Gas | 1. Temperature (measure of kinetic energy) 2. Pressure 3. Volume (fill up container) 4. Amount of gas, number of moles | 8 | |
| 6365602146 | Pressure | amount of force applied to an area standard atmospheric pressure - 1.00 atm | 9 | |
| 6365606963 | Ideal-gas equation | V-T: volume of gas is directly proportional to temperature (increase v, increase t). V-N: volume and moles directly proportional (more particles, the more space they take up). PV=nRT | 10 | |
| 6365616110 | Density | d = MP/RT can find M = mRT/PV | 11 | |
| 6365626360 | Partial Pressures (dalton) | if 2 gases that don't react are combined, they act as if they are alone. Ptotal = p1+p2... | 12 | |
| 6365636352 | Mole Fraction | Ratio of moles of a substance to total moles x1 = moles of compound 1/total moles = n1/n1 p1 = (n1/n1)(Ptotal) = X1*Ptotal | 13 | |
| 6365646715 | Kinetic Molecular Theory (motion, volume, forces, energy, avg kinetic energy). | 1. gases consist of large numbers of molecules - continuous, random motion 2. Combined volume of all molecules of the game is negligible relative to the total volume in which the gas is contained (molecules/volume all together is so small compared to the total volume) 3. Attractive and repulsive forces between gas molecules are negligible. 4. Energy can be transferred bw molecules during collision (perfectly elastic, no loss of energy). 5. average kinetic energy of molecules is proportional to the temperature (K) | 14 | |
| 6365672483 | Molecular speed graph | are underneath graph is proportionality of how much gaseous molecules there are. Low temperature --> higher peak, molecules have less distributed range of speeds Higher temperature--> peak lowers, distribution increases because sample is heated and needs to overcome intermolecular forces at a faster rate due to temperature change |  | 15 |
| 6365690829 | gas molecular speed | individual molecules can have different speeds of motion temp related to average kinetic Urms = root mean sure speed, associated with avg kinetic energy | 16 | |
| 6365736290 | urms | at a given temp, average kinetic energy of molecules is the same. 1/2 m(urms)^2 is the same for 2 gases at the same temp if gas has a low mass, speed will be greater than for a heavier molecule. urms = sqrt root of 3RT/molar mass higher molar mass, smaller urms expression | 17 | |
| 6365759579 | Effusion | escape of gas molecules through a tiny hole into an evacuated space - if molecules have a high speed, hit area with a greater frequency, so greater probability of finding the hole - rate of effusion increases when molecules are fast and lighter - greater mass with less frequency, decrease rate of effusion | 18 | |
| 6365761029 | Diffusion | the spread of one substance throughout a space or a second substance | 19 | |
| 6365768911 | Graham's Law | lighter gas always has faster rate of speed - relative speed of two gases molar mass ratio is dependent on this r1/r2 = sort of molar mass 2/molar mass1 | 20 | |
| 6365775760 | Deviations from Ideal behavior | 1. Gas molecules occupy a small fraction of the total volume. it is a negligible volume 2. gas molecules occupy a larger fraction of the total volume --> significant proportion *non-ideal situation with high pressure* With high temperature, lesser chance to hold on to molecules as it is fast moving gaseous condition IMF --> rel. weak (short distance) --> at high pressure/low temp: attractive forces come into play | 21 | |
| 6365798362 | Van der Waals equation (p+n2a/v2)(V-nb)=nRT | used for corrected-ideal gas equation (a and b are constants that are always positive values) n2a/v2 --> accounts for attractive forces. pressure is adjusted upwards since attractive forces result in fewer collisions. nb --> accounts for small but definite volume of molecules; subtracted to just volume down to give a more accurate representation of the actual volume available. | 22 |
