chapter 5
Terms : Hide Images
| a device for measuring atmospheric pressure | ||
| a device for measuring the pressure of a gas in a container | ||
| a unit of pressure, also called a torr, 760 mm Hg = 760 torr = 101,325 Pa = 1 standard atmosphere | ||
| another name for millimeter of mercury (mm Hg) | ||
| a unit of pressure equal to 760 mm Hg | ||
| the SI unit of pressure; equal to newtons per meter squared | ||
| the volume of a given sample of gas at constant temperature varies inversely with the pressure; V = k/P (at constant T and n) | ||
| a gas that strictly obeys Boyle's law | ||
| the volume of a given sample of gas at constant pressure is directly proportional to the temperature in kelvins; V = bT (at constant P and n) | ||
| also called 0 K; this temperature cannot be attained; at temperatures below this point, the extrapolated volumes would become negative | ||
| equal volumes of gases at the same temperature and pressure contain the same number of particles; V = an (at constant T and P) | ||
| the combined proportionality constant in the ideal gas law; 0.08206 L • atm/K • mol or 8.3145 J/K • mol | ||
| an equation of state for a gas, where the state of the gas is its condition at a given time; expressed by PV = nRT, where P = pressure, V = volume, n = moles of the gas, R = the universal gas constant, and T = absolute temperature; this equation expresses behavior approached by real gases at high T and low P | ||
| the volume of one mole of an ideal gas; equal to 22.42 liter at STP | ||
| the condition 0 °C and 1 atmosphere of pressure | ||
| for a mixture of gases in a container, the total pressure exerted is the sum of the pressures that each gas would exert if it were alone | ||
| the independent pressures exerted by different gases in a mixture | ||
| the ratio of the number of moles of a given component in a mixture to the total number of moles in the mixture | ||
| a model that assumes that an ideal gas is composed of tiny particles (molecules) in constant motion | ||
| the square root of the average of the squares of the individual velocities of gas particles | ||
| defined as a kilogram meter squared per second squared (kg • m^2/s^2) | ||
| the mixing of gases | ||
| the passage of a gas through a tiny orifice into an evacuated chamber | ||
| the rate of effusion of a gas is inversely proportional to the square root of the mass of its particels | ||
| gas that behaves ideally only at high temperatures and low pressures | ||
| a mathematical expression for describing the behavior of real gases | ||
| the mixture of gases that surrounds the earth's surface | ||
| contamination of the atmosphere, mainly by the gaseous products of transportation and production of electricity | ||
| air pollution produced by the action of light on oxygen, nitrogen oxides, and unburned fuel from auto exhaust to form ozone and other pollutants | ||
| a result of air pollution by sulfur dioxide |
