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Definition
| Force applied per given area. |
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standard temp and pressure Table A
237 K ~ 0 C
1 atm ~ 101.3 kPa 760 torr or 760 mmhg |
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| kinetic molecular theory of gases |
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Definition
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| the gas molecules move in a continuous straight line w/ random movement. |
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| there are no forces of attraction between molecules |
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| molecules are so small they essentially have no volume. |
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| collisions are elastic between gas molecules (elastic indicates no energy expanded) |
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| there is a direct relationship between temperature and ave kinetic energy of a particle |
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Term
| which gases most resemble an ideal gas under most conditions: He |
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Definition
| The lighter the gas, the more ideal it will act (therefore H2 and He act the most idea. |
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low volume
low temperature
low pressure |
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high volume
high temperature
high pressure |
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Definition
| relationship between pressure and volume of gas at constant temp and number of particles. A increase in pressure causes a decrease in volume. |
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relationship between and volume of a gas
At constant pressure and number of particles. An increase in temperature causes an increase in volume. |
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| relationship between temp and pressure of gas. At constant volume and number of particles and an increase in pressure causes an increase of temperature. |
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By combining all the laws for an ideal gas, we can solve for all 3 variables
(P1 X V1)/T1 = (P2 X V2)/T2 |
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Term
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Definition
1. Pressure that is exerted the container walls as collisions occur.
2. The greater the temperature the greater the vapor pressure |
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Temperature goes up
pressure goes up |
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| What is the boiling point of water? |
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Definition
100 C
Mt Everest P525 torr 7 BP is lower because there are less air molecules applying pressure. Molecules vaporize more quickly. |
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| If something is volatile does i have a low vapor pressure or a high vapor pressure? |
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Definition
High vapor pressure-it vaporizes quickly
*unstable and volatile substance have high vapor point. |
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Term
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Definition
1. The point at which all the molecules have enough energy to change into vapor.
2. When the vapor pressure of the liquid equals or exceeds atmosphere pressure, the boiling occurs. |
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| What is Avogadro's hypothesis? |
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Definition
| Under the same conditions of temperature and pressure equal volumes of gasses contain the same number of particles. |
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unit number of particles
1. 1 mole of particles equals the formula mass of the substance express in grams
2. 1 mole refers to 6.02 x 10 (23) particles. |
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Term
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Definition
| 1 mole of any gas will occupy a volume of 22.4 liters @stp |
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Term
| Which does not have a molar volume of 22.4 liters? |
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Definition
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Term
| Graham's Law of Diffusion |
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Definition
| At a given temperature and pressure the great the density of the gas the slow the gas diffuses. Effusion is the process of a gas escaping through small pores/openings. This pollows the same principle. |
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Term
| What is the law of partial pressure? |
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Definition
| The total pressure in a container is equal to the sum of all the partial pressures of the gasses in the container. |
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