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Unit 8
Gases
Term | Definition |
---|---|
Pressure | defined as the force per unit area on a surface |
Newton | the force that will increase the speed of a one kilogram mass by one meter or second each second that the force is applied |
Barometer | a device used to measure atmospheric pressure |
Millimeters of Mercury | the common unit of pressure os millimeters of Mercury symbolized mm hg |
Atmosphere of Pressure | one atmosphere of pressure is defined as being exactly equivalent to 760 mm hg |
Pascal | defined as the pressure exerted by a fore of one newton acting on an area of one square meter |
Partial Pressure | the pressure of each gas in a mixture is called the partial pressure of that gas |
Dalton's law of partial pressure | states that the total pressure of a gas mixture is the sum of the partial pressures of the component gases |
Boyles Law | states that the volume of a mixed mass o 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 |
Charle's law | states that 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 mixed mass of gas at constant volume varies directly with the temperature in kelvins |
Combined gas law | expresses the relationship between pressure volume and temperature of a fixed amount of gas |
Avogadro's law | states that equal volumes of gases at the same temperature and pressure contain equal number of molecules |
Standard molar volume of a gas | the volume occupied by one mole of a gas at STP is known as the standard molar volume of a gas. It has been found to be 22.414 10 L |
ideal gas law | the mathematical relationship among pressure volume temperature and the number of moles of gas |
ideal gas constant | in the equation representing the ideal gas law the constant R is known as the ideal gas constant |
Graham's law of effusion | states that the rate of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses |