var nc = 27,
fc = new Array(nc);
fc[0] = {t:"Absolute Temperature",d:"Temperature expressed in kelvins on the absolute temperature scale, on which 0 K is the lowest possible temperature."};
fc[1] = {t:"Amonton’s Law",d:"As the absolute temperature of a fixed amount of gas increases, the pressure increases as long as the volume and quantity of gas remain constant."};
fc[2] = {t:"Atmospheric Pressure (*P*atm)",d:"The force exerted by the gases surrounding Earth on Earth’s surface and on all surfaces of all objects."};
fc[3] = {t:"Avogadro’s Law",d:"The volume of a gas at a given temperature and pressure is proportional to the quantity of the gas."};
fc[4] = {t:"Barometer",d:"An instrument that measures atmospheric pressure."};
fc[5] = {t:"Boyle’s Law",d:"The volume of a given amount of gas at constant temperature is inversely proportional to its pressure."};
fc[6] = {t:"Charle’s Law",d:"The volume of a fixed quantity of gas at constant pressure is directly proportional to its absolute temperature."};
fc[7] = {t:"Dalton’s Law of Partial Pressures",d:"The total pressure of any mixture of gases equals the sum of the partial pressures of all the gases in the mixture."};
fc[8] = {t:"Diffusion",d:"The spread of one substance (usually a gas or liquid) through another."};
fc[9] = {t:"Effusion",d:"The process by which a gas escapes from its container through a tiny hole into a region of lower pressure."};
fc[10] = {t:"General Gas Equation",d:"(also called *combined gas law*)

Based on the ideal gas law and used when one or more of the four gas variables are held constant while the remaining variables change."};
fc[11] = {t:"Graham’s Law of Effusion",d:"The rate of effusion of a gas is inversely proportional to the square root of its molar mass."};
fc[12] = {t:"Ideal Gas Law",d:"(also called *ideal gas law*)

Relates the pressure, volume, number of moles, and temperature of an ideal gas; expressed as *PV* = *nRT,* where *R* is the universal gas constant."};
fc[13] = {t:"Ideal Gas",d:"A gas whose behavior is predicted by the linear relations defined by Boyle’s, Charles’s, Avogadro’s, and Amontons’s laws."};
fc[14] = {t:"Kinetic Molecular Theory",d:"A model that describes the behavior of gases; all equations defining relationships between pressure, volume, temperature, and number of moles of gases can be derived from the theory."};
fc[15] = {t:"Manometer",d:"An instrument for measuring the pressure exerted by a gas."};
fc[16] = {t:"millimeters of Mercury (mmHg)",d:"(also called *torr*)

A unit of pressure where 1 atm = 760 mmHg = 760 torr."};
fc[17] = {t:"Miscible",d:"Capable of being mixed in any proportion (without reacting chemically)."};
fc[18] = {t:"Molar Volume",d:"Volume occupied by 1 mole of an ideal gas at STP; 22.4 L."};
fc[19] = {t:"Mole Fraction (*X*x)",d:"The ratio of the number of moles of a component in a mixture to the total number of moles in the mixture."};
fc[20] = {t:"Partial Pressure",d:"The contribution to the total pressure made by a component in a mixture of gases."};
fc[21] = {t:"Pressure (*P*)",d:"The ratio of force to surface area over which the force is applied."};
fc[22] = {t:"Root-Mean-Square Speed (*u*rms)",d:"The square root of the average of the squared speeds of all the molecules in a population of gas molecules; a molecule possessing the average kinetic energy moves at this speed."};
fc[23] = {t:"Standard Atmosphere (1 atm)",d:"The pressure capable of supporting a column of mercury 760 mm high in a barometer."};
fc[24] = {t:"Standard Temperature and Pressure (STP)",d:"0°C and 1 bar as defined by IUPAC; in the United States, 0°C and 1 atm."};
fc[25] = {t:"Universal Gas Constant",d:"The constant *R* in the ideal gas equation; its value and units depend on the units used for the variables in the equation."};
fc[26] = {t:"van der Waals Equation",d:"An equation that includes experimentally determined factors *a* and *b* that quantify the contributions of nonnegligible molecular volume and nonnegligible intermolecular interactions to the behavior of real gases with respect to changes in *P,* *V,* and *T.*"};