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| 7626903443 | Gases in terms of density | Low density because the few particles are spread out in a large volume | 0 | |
| 7626908244 | Gases in terms of compressibility | Easy to compress because the particles are spread out in a lot of empty space | 1 | |
| 7626910467 | Gases in terms of Fluidity | Very Fluid because particles are in constant motion and aren't attracted to each other so they can move easily around each other | 2 | |
| 7626910468 | Gases in terms of diffusion | Diffuse easily because particles are in constant motion, so they can mix freely with other types of gases. Two or more gases from a homogeneous mixture regardless of reactivity or identity | 3 | |
| 7626914016 | Gases in terms of Effusion | Easily effuse through tiny openings because they have no shape or permanent volume. | 4 | |
| 7626914940 | Kinetic Molecular Theory | 1. Gases consist of large numbers of molecules that are in continuous random motion 2. The combined volume of all the molecules of the gas is negligible relative to the total volume in which the gas contained 3. Attractive and repulsive forces between gas molecules are insignificant 4. Energy can be transferred between molecules during collisions that are perfectly elastic but as long as the temperature stays constant, the average kinetic energy of the molecules don't change with time 5. The average kinetic energy of the molecules is proportional to the absolute temperature 6. Gases consist of tiny particles in empty space | 5 | |
| 7626917745 | Ideal Gas | ideal gases are always gases regardless of temperature or pressure ideal gases cannot be liquified or solidified no attractive forces exist between the particles (atoms or molecules) the particles have no volume real gases behave "ideally" when the right conditions exist more ideal conditions: high temperature, high volume, low pressure, low moles | 6 | |
| 7626917746 | Real Gas | Have volume Have attractive forces between the particles Behave ideally when high temperatures and low pressures Can be liquified or solidified | 7 | |
| 7626919621 | Pressure | Pressure is a force exerted by the substance per unit area on another substance. P=F/A | 8 | |
| 7626919622 | Barometer | an instrument measuring atmospheric pressure, used especially in forecasting the weather and determining altitude. | 9 | |
| 7626920930 | Manometer | an instrument for measuring the pressure acting on a column of fluid, especially one with a U-shaped tube of liquid in which a difference in the pressures acting in the two arms of the tube causes the liquid to reach different heights in the two arms. | 10 | |
| 7627134407 | How do you find pressure of a gas in a manometer? | P(gas)= p(atm)+p(height) in mmHg | 11 | |
| 7626921080 | atm to mmHg | multiply by 760 | 12 | |
| 7626923745 | mmHg to Pa | multiply by 1.01325e5/760 | 13 | |
| 7626923746 | atm to Pa | multiply by 1.01325e5 | 14 | |
| 7626923747 | atm to kPa | multiply by 101.325 | 15 | |
| 7626927462 | mmHg to kPa | multiply by 101.325/760 | 16 | |
| 7626929215 | Celsius to Kelvin | Add 273 | 17 | |
| 7626931396 | Kelvin to Celsius | Subtract 273 | 18 | |
| 7626933264 | Boyle's law | The volume of a fixed quantity of gas maintained at a constant pressure is inversely proportional to the pressure. P1V1=P2V2. |  | 19 |
| 7626936473 | Charles's Law | The volume of a fixed amount of gas maintained at a constant pressure is directly proportional to its absolute value. V1/T1=V2/T2 |  | 20 |
| 7626936474 | Gay Lussac's Law | The pressure of a gas is directly proportional to its Kelvin temperature. P1/T1=P2/T2 |  | 21 |
| 7626940430 | Avogadro's Law | Equal volumes of gases at the same temperature and pressure contain equal numbers of moles. V1/n1=V2/n2 |  | 22 |
| 7626942586 | Combined Gas Law | P1V1/T1=P2V2/T2 comes from ideal gas law | 23 | |
| 7626944267 | Ideal gas law | PV=nRT Assumes that the molecules don't interact and the combined volume of the molecules id much smaller than the one the gas occupies | 24 | |
| 7626946057 | R | Universal Gas Constant | 25 | |
| 7626946058 | R in atm | 0.08206 | 26 | |
| 7626946238 | R in mmHg | 62.4 | 27 | |
| 7626949547 | R in kPa and Pa | 8.31447 | 28 | |
| 7626951386 | Graham's Law | The rate of effusion of a gas is inversely proportional to the square root of its mass. r1/r2= the square root of MM2/MM1 | 29 | |
| 7626953483 | Absolute Zero | The temperature where all motion stops | 30 | |
| 7626955473 | Dalton's Law | The total pressure of a mixture of gases equals the sum of the pressures that each would exert if it were present alone. P(total)=P1+P2+P3... | 31 | |
| 7627382313 | Partial Pressure | the hypothetical pressure of that gas if it alone occupied the volume of the mixture at the same temperature. | 32 | |
| 7626957632 | Conditions of STP | Pressure= 1atm Temperature= 273 or 0C Volume occupied by 1 mole at STP= 22.4 (molar volume) | 33 | |
| 7626964305 | Kinetic Energy | Kinetic energy is the energy an object possesses due to its motion. KE=1/2mv^2 or KE=3/2RT |  | 34 |
| 7626964306 | Root Mean Square Velocity | v= the square root of 3(R)(T)/MM in kg/mol |  | 35 |
| 7626967630 | Conditions for most ideal gases | High Temperature Low Pressure Low moles | 36 | |
| 7626970352 | Van der Waals Equation | mathematically deals with the non-ideality of real gases. (P + n^2a/V^2)(V-nb) =nRT |  | 37 |
