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Sec. 12.3: Molecular Composition of Gases 1) Boyle’s Law: a) Charles’ Law: b) Gay-Lussac’s Law: c) Avogadro’s Law: 2) Ideal gas: an _________________ gas whose particles are infinitely ____________ and do ____________ interact with each other. a) An ideal gas: i) Does _____ condense to a _____________ at ___________ temperatures. ii) Does not have forces of ______________ or repulsion between the ____________. iii) Is composed of ______________ that have no ______________. 3) Ideal gas law: the law that states the mathematical relationship of pressure (P), volume (V), temperature (T), the gas constant (R), and the number of moles of a gas (n). a) Ideal gas law equation: 4) R is a: ______________________________________________________________ a) For Pressure in kPa, R = b) For Pressure in atm, R = 5) Real gases _____________ somewhat from an __________ gas and more so at very _____________ ______________. 6) Sample problem E, pg 435 How many moles of gas are contained in 22.41 liters at 101.325 kPa and 0˚C? 7) Additional Practice a) What is the volume of 4.35 moles of a gas at a pressure of 85.6 kPa and 26.0˚C? 8) Diffusion: the _________________ of particles from regions of _____________ density to regions of lower ________________. a) The process of _____________ involves an ______________ in _____________. 9) Effusion: the passage of gas under ______________ through a tiny _____________. a) Scottish scientist Thomas Graham found that at constant ____________ and _____________, the rate of effusion of a gas is __________ proportional to the square root of the gases __________ __________, M. 10) Graham’s law of diffusion equation: V = velocity (molecular speed) of gas A and B M = molar mass of gas A and B a) Particles of __________ molar mass travel __________ than __________ particles. 11) Sample problem F, pg. 438 Oxygen molecules have an average speed of about 480 m/s at room temperature. At the same temperature, what is the average speed of molecules of sulfur hexafluoride, SF6? 12) Additional Practice The average velocity of CO2 molecules at room temperature is 409 m/s. What is the molar mass of a gas whose molecules have an average velocity of 322 m/s under the same conditions? 13) In 1808, Joseph Gay-Lussac made an important discovery: if the __________ and ______________ are kept constant, gases react in ____________ proportions that are __________ __________ __________. a) Gay-Lussac’s law of combining volumes: the law that states that the _____________ of gases involved in a chemical _____________ can be represented by the ____________ of small whole numbers. 14) Gas reactions allow __________ ____________ to be deduced. a) Hydrogen molecules combine with __________ molecules in a 1:1 volume ratio to produce __________ the volume of hydrogen chloride. 15) In 1805, John Dalton showed that in a ______________ of gases, each gas exerts a certain ____________ as if it were ______________ with no other gases mixed with it. a) Partial Pressure: the _____________ of each gas in a ________________. b) Dalton’s law of partial pressure: the law that states that the ____________ ____________ of a mixture of gases is the __________ of the ____________ ____________ of the component gases. 16) Dalton’s law of partial pressures equation: a) P total = total pressure b) PA = partial pressure of gas A c) PB = partial pressure of gas B d) PC = partial pressure of gas C 17) Dalton’s law of __________ __________ is explained by the ____________ ____________ theory. a) All the gas molecules are moving _____________, and each has an __________ chance to ____________ with the _____________ __________. b) Each gas exerts a pressure _______________ to its number of _____________ in the container. The presence of other gas molecules __________ __________ change this fact. 18) Ratios of __________ __________ will be the same as __________ __________ of gases in _______________ _______________. a) Avogadro’s law shows that the __________ __________ of two gases at the same temperature and pressure is the same as the _____________ ratio of the two gases. 19) For example: 3 H2 (g) + N2 (g) 2 NH3 (g) a) 3 L of H2 react with 1 L of N2 to form 2 L of NH3 with no H2 or N2 left over b) If we know the number of __________ of a gaseous substance, we can use the __________ __________ __________ to calculate the __________ of that gas. 20) Sample problem G, pg, 441 How many liters of hydrogen gas will be produced at 280.0 K and 96.0 kPa if 1.74 mol of sodium react with excess water according to the following equation? 2Na (s) + 2 H2O (l) 2 NaOH (aq) + H2 (g) 21) Additional Practice A student wished to prepare oxygen by using the thermal decomposition of potassium chlorate, KClO3. Given that the gas will have a temperature of 700˚C and a pressure of 98.6 kPa, how much potassium chlorate will be necessary to produce 125 mL of oxygen? Δ 2 KClO3 3 O2 + 2 KCl 22) Methane has a volume of 0.65 L when under 100 kPa of pressure at a temperature of 305 K. Using the balanced equation below, find the mass of oxygen that is needed to use up all of the methane. CH4 + 2 O2 CO2 + 2 H2O