Flashcards
MCAT Chemistry - Ideal Gases
Cards in this deck (11)
- 1Absolute temperatureA temperature scale whose lowest possible value is zero. Absolute temperature is measured in Kelvin.
- 2Avogadro's numberN A = 6.022×1023 . An avogadro's number of molecules equals one mole.
- 3Boyle's lawA gas law relating pressure and volume for a fixed amount of gas at a constant temperature. Mathematically:
PV = C
C is a constant unique to the amount of gas and temperature. - 4Dalton's lawThe total pressure of a mixture of gases is the sum of the pressures each constituent gas would exert alone. Mathematically:
P tot = P A + P B + P C + ƒƒƒ - 5Ideal gas lawA gas law stating that PV = nRT . The two main assumptions of the law are that the molecules of an ideal gas do not have volume and do not interact with each other. The ideal gas law is a good approximation when the pressure is low and the temperature is high.
- 6Isothermal conditionsTwo or more conditions that share the same temperature. In other words, T is constant.
- 7KelvinA unit of absolute temperature. Abbreviated with the letter "K." The Kelvin scale is related to the Celsius scale by T K = T C + 273.15 . Kelvin should be used for all classical and ideal gas law calculations.
- 8—Manometer
- 9ManometerA device used to measure the difference in pressure between two gases: "A" and "B" represent the atmosphere, a vacuum, or a pressurized gas.
- 10MoleOne mole contains Avogadro's number ( 6.022×1023 ) of particles. For example, one mole of H 2 would contain 6.022×1023 H 2 molecules. Moles are abbreviated as "mol."
- 11Partial pressureIn a mixture of gases, the pressure exerted by one constituent gas. The sum of the partial pressures of gases in a mixture is equal to the total pressure of the mixture.
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- SAT MCAT Flashcards on MCAT Chemistry - Ideal Gases, created by Ali Kane on 21/05/2014.
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