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Unit 8: Gases

Chemistry

TermDefinition
Pressure The force per unit area on a surface.
Newton Force that will increase the speed of a one-kilogram mass by one meter per second each second that the force is applied.
Barometer Device used to measure atmospheric pressure.
Millimeters of Mercury The most common unit of pressure; symbolized as mm Hg.
Atmosphere of Pressure Being exactly equivalent to 760 mm Hg.
Pascal The pressure exerted by a force of one newton (1 N) acting on an area of one square meter; symbolized as Pa.
Partial Pressure The pressure of each gas in a mixture of that gas.
Dalton's Law of Partial Pressure States that the total pressure of a gas mixture is the sum of the partial pressure of the component gas.
Boyles Law The volume of a fixed mass of a gas varies inversely with the pressure at constant temperature.
Absolute Zero The lowest possible achievable temperature is assigned the value of zero on the Kelvin temperature scale.
Charles' Law The volume of a fixed mass of gas at constant pressure varies directly with the temperature in kelvins.
Gay-Lussac's Law The pressure of a fixed mass at constant volume varies directly with the temperature in kelvins.
Combined Gas Law Expresses the relationship between the pressure, volume, and temperature of a fixed amount of gas.
Avogadro's Law The equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
Standard Molar Volume of a Gas The volume occupied by one mole of a gas at STP is known as that; it has been found to be 22.414 10 L.
Ideal Gas Law The mathematical relationship among, pressure, volume, and temperature, as well as the number of moles of a gas.
Ideal Gas Constant Representing the ideal gas law; the constant R.
Graham's Law of Effusion Rates of effusion of gases at the same temperature & pressure are inversely proportional to the square roots of their molar masses.
Created by: mv383931
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