Chemistry vocab
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| 349006153 | diffusion | Spontaneous mixing of the particles of two substances caused by their random motion | |
| 349006154 | effusion | Process by which gas particles under pressure pass through a tiny opening | |
| 349006155 | elastic collision | Collision between gas particles and between particles and container walls. These collisions have no net loss of kinetic energy | |
| 349006156 | fluid | Gas particles glide easily past one another. Both liquids and gases flow so they are both considered this. These take the shape of their container. | |
| 349006157 | ideal gas | An imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory. | |
| 349006158 | kinetic-molecular theory | Particles of matter are always in motion. | |
| 349006159 | real gas | A gas that does not behave completely according to the assumptions of the kinetic-molecular theory | |
| 349006160 | atmosphere of pressure | Exactly 760 mm Hg. | |
| 349006161 | barometer | Device used to measure atmospheric pressure. | |
| 349006162 | millimeter of mercury | A common unit of pressure, symbolized by mm Hg. | |
| 349006163 | newton | It is the force that will increase the speed of one kilogram mass by one meter per second each second it is applied. It is the SI unit of force. | |
| 349006164 | pascal | The pressure exerted by a force of one newton (1N) acting on an area of one square meter. | |
| 349006165 | standard temperature and pressure | For purposes of comparison, scientists have agreed on standard conditions of exactly 1 atm pressure and 0°C. These conditions are commonly abbreviated STP. | |
| 349006166 | absolute zero | -273.15°C or 0 K. The theoretical lowest temperature possible to achieve. | |
| 349006167 | Boyle's law | The volume of a fixed mass of gas varies inversely with the pressure at constant temperature. (simply - when volume goes up the pressure goes down, and when volume goes down the pressure goes up when temperature is kept constant) | |
| 349006168 | Charles's Law | The volume of a fixed mass at constant pressure varies directly with the Kelvin temperature (simply - when the temperature goes up the volume goes up, when the temperature goes down, the volume goes down if pressure is constant) | |
| 349006169 | combined gas law | Expresses the relationship between pressure, volume, and temperature of a fixed amount of gas. | |
| 349006170 | Dalton's Law of partial pressures | The total pressure of a mixture of gasses is equal to the sum of the partial pressures. | |
| 349006171 | gas laws | Simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas. | |
| 349006172 | Gay-Lussac's Law | The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin Temperature. (simply - pressure goes up with the temperature, and down with temperature if volume is kept constant) | |
| 349006173 | partial pressure | The pressure of each gas in a mixture. | |
| 349006174 | Avogadro's law | Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. | |
| 349006175 | Gay-Lussac's law of combining volumes of gases | At constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers | |
| 349006176 | standard molar volume of a gas | The volume occupied by one mole of a gas at STP. This has been found to be 22.41410 L. | |
| 349006177 | ideal gas constant | The constant R. | |
| 349006178 | ideal gas law | The mathematical relationship of pressure, volume, temperature, and the number of moles of a gas. | |
| 349006179 | capillary action | The attraction of the surface of a liquid to the surface of a solid. | |
| 349006180 | evaporation | The process by which particles escape from the surface of a nonboiling liquid and enter the gas state. | |
| 349006181 | surface tension | A force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size. | |
| 349006182 | amorphous solid | The particles are arranged randomly. | |
| 349006183 | crystal structure | The total three-dimensional arrangement of particles of a crystal. | |
| 349006184 | melting | The physical change of a solid to a liquid by the addition of heat. | |
| 349006185 | supercooled liquid | Substances that retain certain liquid properties even at temperatures at which they appear to be solid. | |
| 349006186 | freezing | The physical change of a liquid to a solid by removal of heat. | |
| 349006187 | vaporization | The process by which a liquid or solid changes to a gas. | |
| 349006188 | crystal | A substance in which the particles are arranged in an orderly, geometric, repeating pattern. | |
| 349006189 | crystalline solid | Most solids are this. They consist of crystals. | |
| 349006190 | melting point | The temperature at which a solid becomes a liquid. | |
| 349006191 | unit cell | The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice. | |
| 349006192 | boiling | The conversion of a liquid to a vapor within the liquid as well as at its surface. It occurs when the equilibrium vapor pressure of the liquid equals the atmospheric pressure. | |
| 349006193 | boiling point | The temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure. | |
| 349006194 | condensation | The process by which a gas changes to a liquid. | |
| 349006195 | critical point | Indicates the critical temperature and critical pressure. | |
| 349006196 | critical pressure | The lowest pressure at which the substance can exist as a liquid at the critical temperature. | |
| 349006197 | critical temperature | The temperature above which the substance cannot exist in the liquid state. | |
| 349006198 | deposition | The change of state from a gas directly to a solid. | |
| 349006199 | equilibrium | A dynamic condition in which two opposing changes occur at equal rates in a closed system. | |
| 349006200 | equilibrium vapor pressure | The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature. | |
| 349006201 | freezing point | The temperature at which the solid and liquid are in equilibrium at 1 atm pressure. | |
| 349006202 | Le Chatelier's principle | When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress. | |
| 349006203 | Molar heat of fusion | The amount of heat energy required to melt one mole of solid at its melting point. | |
| 349006204 | molar heat of vaporization | The amount of heat energy needed to vaporize one mole of liquid at its boiling point. | |
| 349006205 | phase | Any part of a system that has uniform composition and properties. | |
| 349006206 | phase diagram | A graph of pressure versus temperature that shows the conditions under which the phases of as substance exist. | |
| 349006207 | sublimation | The change of state from a solid directly to a gas. | |
| 349006208 | triple point | Indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium. | |
| 349006209 | volatile liquid | Liquids that evaporate readily. |
