Lab Report Of Gas Laws In Chemistry 1101

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Gas Laws: Relationship between Pressure (P), Volume (V), Temperature (T) and quantity; Moles (n) Boyle’s Law (PV = constant) This is an inverse relationship: As volume decreases, pressure increases. Charles’ Law: (V/T = constant) This is a direct relationship. As Temperature decreases, Volume decreases. Avogadro’s Law: (V/n = constant) This is a direct relationship. As the number of moles decreases, the volume decreases Summary: Combined Gas Law: PV/nT = constant (T in Kelvins) P1V1/n1T1 = P2V2/n2T2 Ideal gas Law: PV = nRT R = .0821L atm/mol K Gay-Lussac’s/Avogadro’s Law of Combining Volumes Equal volumes of any gases at the same temperature and pressure contain the same number of moles of gas. The coefficients of a balanced equation can be used to calculate relative volumes. Standard Molar Volume: At standard temperature and pressure (STP = 1atm and 273.15K) 1 mole of any ideal gas has a volume of 22.4L Variations on the ideal gas law equation: PV = mRT/M (m = sample mass, M = molar mass of the gas) d = MP/RT (d = density of the gas in g/L) Examples: 1. Calculate: a. The new pressure in a closed container if a 5.0L volume of gas at 2.5atm has its volume increased to 7.5L. b. The new volume of gas (at constant T and P) if 2.0mol of He in a 3.0L container has another 3.0mol of He placed into the container. Answers: a. (5.0L)(2.5atm) = (7.5L)(P2) P2 = 1.7atm b. 3.0L/2.0mol = V2/5.0mol V2 = 7.5L 2. When a rigid hollow sphere containing 680 L of helium gas is heated from 300.K to 600.K, the pressure of the gas increases to 18atm. How many moles of helium does the sphere contain? Answer: n = PV/RT = (18atm)(680L)/(.0821)(600.K) n = 248.48 = 250moles 3. A child has a lung capacity of 2.2 L. How

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