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CHM 113 (103)
Ron Briggs (24)

Gas Properties and Laws

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Arizona State University
CHM 113
Ron Briggs

Gas Properties - A gas can be described by 4 variables: P, V, T, n - Pressure (P): force per unit area exerted on a surface (ex: container walls) o Common units: atm, mm Hg (torr), Pa, Bar, PSI o 1 atm = 760 mm Hg = 760 torr o 1 atm = 1.01325 x 10 Pa = 101.325 kPa o 1 bar = 100,000 Pa = 0.9869 atm o 1 atm = 14.6 PSI - Volume (V): amount of space occupied 3 3 o Common units: L, mL, m , cm - Temperature (T): how hot or cold. According to Kinetic Molecular Theory (KMT), a measure of average velocity and KE of gas particles o Common units: F, C, K o o o K = C + 273.15 o Standard Temperature and Pressure (STP): 273.15K, 1 atm  At STP, 1 mole of an ideal gas occupied 22.41 L - Quantity (n): number of gas particles (in moles) o 1 mole = 6.022 x 10 gas particles o Gas particles can be atoms (He, Kr, Ar) or much larger molecules (O , N , 2 2 CH ,4CCl ) 4 Gas Laws - Experimental Evidence has shown that the following 3 relations apply to gases: o Boyle’s Law: V = (1/P) x constant
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