vapors: gases of substances that are normally liquids or solids 1 atm = 760 mm Hg = 760 torr = kpa = bar
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1 Gases A Chemistry Lecture Outline Name: Basics on Gases composition of the atmosphere: properties of gases: vapors: gases of substances that are normally liquids or solids Equation for pressure: 1 atm = 760 mm Hg = 760 torr = ka = bar vacuum air pressure BAROMETER OEN END MANOMETER AIR RESSURE CLOSED END MANOMETER SEALED END mercury (Hg) CONFINED GAS Hg HEIGHT DIFFERENCE The Gas Laws Boyle s law: Charles s law: Gay-Lussac s law: = constant /T = constant /T = constant T T 1
2 Avogadro s law: Equal volumes of gas at the same temperature and pressure have the same number of particles. Combined Gas law: merges Boyle s, Charles s, and Gay-Lussac s laws in one equation. **NOTE: For all gas law calculations, use the absolute temperature (in K). Ideal Gas law: n = number of moles of gas R = L-ka/mol-K = L-atm/mol-K Conditions of standard pressure and temperature (ST): Equation for gas density (in g/l): d = molar mass of gas RT To solve problems involving volumes of gases in chemical s: 1. Use = nrt to get any and all gases in terms of moles (i.e., n). 2. Solve the problem using stoichiometry. EX. Safety air bags in automobiles are inflated by nitrogen gas generated by the rapid decomposition of sodium azide, according to 2 NaN 3 (s) 2 Na(s) + 3 N 2 (g) If an air bag has a volume of 36 L and is to be filled with nitrogen at 1.15 atm and 26.0 o C, how many grams of sodium azide must be decomposed? 2
3 Dalton s law of artial ressure tot = total pressure of mixture partial pressures: Other equations: Total moles of gas in a mixture of gases can be found using: The mole fraction (X) of a gas in a mixture is found using: EX. Find the total pressure exerted by 14 g of carbon monoxide and 14 g of nitrogen in a 6.0-L container at 25 o C. Collecting Gases over Water filled with water, initially gas being collected collected gas (w/h 2 O vapor, too) gas from H 2 O levels even before during complete After the is complete, raise or lower the collecting vessel so that the water levels inside and out are the same. In this way... 3
4 EX. For the CaC 2 (s) + H 2 O(l) C 2 H 2 (g) + CaO(s)... If L of acetylene are collected over water at 20.0 o C, find the number of moles of acetylene collected and the number of grams of calcium carbide used. Assume the barometric pressure to be torr. EX. Find the total pressure in container Z. A B C Z 1.3 L 2.6 L 3.8 L 2.3 L 3.2 atm 1.4 atm 2.7 atm X atm X X Z X,Z A B C The Kinetic-Molecular Theory (the theory of moving molecules) 1. Gas particles are in constant, random motion. 2. The volume of the particles is negligible compared to the container volume. 3. The attractive-repulsive forces between particles are negligible. 4. Collisions are perfectly elastic (i.e., no energy is lost). 5. KE avg of molecules is proportional to absolute temperature. At a given temperature, the gas particles of Sample A have the same KE as the gas particles of Sample B. 4
5 pressure = how hard and how often gas particles collide with the sides of the container article-elocity Distribution (various gases, same T and ) article-elocity Distribution (same gas, same, various T) # of particles # of particles (SLOW) elocity of particles (m/s) (FAST) (SLOW) elocity of particles (m/s) (FAST) Equation for the rms (root-mean-square) speed of a gas: R = J/mol-K = molar mass, in kg KE avg for a particle = EX. Find the rms velocity of chlorine gas at 80 o C. effusion: the escape of gas particles through a tiny hole into an evacuated space diffusion: the spread of one substance from high concentration to low concentration 5
6 For gases, rates of diffusion & effusion obey Graham s law: The rate of diffusion of gases is slower than the molecular speeds because of The mean free path is the average distance traveled by a particle between collisions. -- it is shorter when the pressure is high EX. At a given temperature, an unknown noble gas travels 1.26 times faster than oxygen gas. What is the noble gas? Real Gases: Deviations from Ideal Behavior All real gases deviate, to some degree, from = nrt. The deviations are most pronounced at... Real gas particles... (1) (2) ideal gas (ideal gas equation): nrt nrt real gas (van der Waals equation): nrt - nb n 2 a 2 The constants a and b are unique for each gas. -- a is large when interparticle attractions are large -- b is large for large gas particles 6
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