ࡱ>  jy mbjbj @#{{QH7 66TD6:tttѣӣӣӣӣӣӣ$t9nXttt66;O~~~tn6"ѣ~tѣ~~yXrIa]%yL}b06ߝjHK}xHLIIH ~ttt~ttt6ttttHttttttttt :   EMBED PBrush CHAPTER 13 &14 NOTES PACKET THE BEHAVIOR OF GASES Big Picture Idea: Gases are affected by temperature, pressure, and volume changes. Big Picture Question: How are gases affected by temperature, pressure and volume? Suggested Resources Homework Assignments Classwork Assignments Laboratory Activities Formative Assessments Textbook pages: Chapter 14 Websites:  HYPERLINK "http://www.webelements.com/" www.webelements.com Key Terms: Diffusion Elastic collision Kinetic molecular theory STP Absolute zero Molar volume Partial pressure Ideal gas Real gas Gas constant PV=nRT (Ideal gas Law) Boyles Law Charles Law Gay Lussacs Law Grahams Law Daltons Law of partial pressures Combined Gas Laws Directions: Use this information as a general reference tool to guide you through this unit. Dont hesitate to ask your teacher for helpBy the conclusion of this unit, you should know the following: The kinetic molecular theory explains the behavior of gases. Gases are affected by temperature, pressure and volume changes. Relationships between temperature, pressure, and volume. How gas and atmospheric pressure are measured. The total pressure of a system of two or more gases would equal the sum of each gass partial pressure.By the conclusion of this unit, you should be able to do the following: Convert between different temperature, pressure and volume units. Solve problems using the Combined Gas Law and the Ideal Gas Law.  GASES Properties of Gases: Particles spread far apart Dispersion forces between molecules (some dipole) Exert pressure Kinetic Theory: The particles in a gas are assumed to be small, hard spheres with an insignificant volume Particles are far apart with no attraction between particles (empty space) The motion of particles in a gas is rapid and random. Gases fill containers, particles travel in straight paths until they collide with walls or other particles All collisions between gas particles are perfectly elastic. Kinetic energy is transferred without any being lost because they have no attraction to each other Pressure:  Definition: Force exerted by a gas per unit surface area on an object What creates pressure? Result of rapidly moving particles in a gas simultaneously colliding with the surface or container walls (more hits = more pressure; less hits = less pressure) Atmospheric Pressure: Barometer Number of collisions of atoms and molecules in air with the surface (measured by barometer) Pressure Units: 1 atmosphere = 760 mmHg = 101.3kPa Make the following pressure conversions 4.3 atm to mmHg  4.3 atm 760 mmHg = 3268 mmHg 1 atm 2.25atm to kPa  2.25 atm 101.3 kPa = 228 kPa  1 atm 450mmHg to kPa  450 mmHg 101.3 kPa = 60 kPa 760 mmHg Volume: Definition: measure of space occupied by matter Units: 1000 mL = 1 L = 1 dm3 Kinetic Energy and Temperature: Kinetic Energy: energy of motion dependent on mass (how heavy) and velocity (speed) Temperature: average kinetic energy of particles in a sample (think speed) Why Kelvin Temperature? Kelvin temperature is directly proportional to the average kinetic energy of the particles of the substance What is Absolute Zero? All motion stops ( 0 K or 273 C) What is STP? Standard temperature and pressure ( 0 C/ 273 K, 1atm/760 mmHg/101.3 kPa) Kelvin Temperature: Units: 1 K = 1 C K = C +273 Make the following temperature conversions: 100C to K 323 K to C 100 + 273 = 373 K 323 273 = 50 C  INCLUDEPICTURE "http://www.dlt.ncssm.edu/tiger/diagrams/gases/MolecularSpeed_vs_Temp-640.gif" \* MERGEFORMATINET  Which point on each curve represents the average kinetic energy? (label on diagram) Top of each peak Which point on each curve represents the slowest moving particles? (label on diagram) @ 0 m/sec Which point on each curve represents the fastest moving particles? (label on diagram) @ 1200 m/sec for 25C and 2000 m/sec for 1000C What do you think would happen to the first shape of the curve if the temperature were even lower? More extreme curve (higher peak) RELATIONSHIPS BETWEEN PRESSURE, VOLUME & TEMPERATURE OF A GAS Charless Law Volume and Temperature   Temp. (K)Volume (L)100200 400800 Practice problem: If a gas occupies 10.0 L at 50C, what volume will it occupy at 150C? You Try: If a gas occupies 33.7 L at 16C, what temperature will it be when it occupies a volume of 67.4 L? Gay-Lussacs Law - Pressure and Temperature  Temp. (K)Pressure (atm)100200400800 Practice problem: If a gas exerts a pressure of 2.5 atm at 100C, what pressure would it exert at 200C?  You Try: The pressure of a gas is 650mmHg at 23C. At what temperature will its pressure drop to 425mmHg? Boyles Law-Pressure and Volume   Volume (mL)Pressure ( )6055504530 Type of relationship? Inverse proportion Equation  P1V1 = P2V2 Practice problem: A gas occupies a volume of 7.5 L at 550 mmHg. What volume will it occupy at 850 mmHg? You Try: A gas occupies a volume of 7.5 L at 550 mmHg. What is the pressure of a gas that has a volume of 8.50 L? Combined Gas Law Equation: P1V1 = P2V2 T1 T2 Practice Problem: If a gas occupies 5.0 L at 1.25 atm and 75C, what volume will it occupy at 0.5 atm and 125C ? GAS LAW PRACTICE PROBLEMS Before beginning, write out all four formulas in the box below:  1. A gas occupies 450mL at 23C. Determine its volume at 75C if the pressure remains constant. Do you expect volume to go up or down? Formula: __ 529 mL______ 2. A gas in an expandable container has a pressure of 1.2atm when the volume is 10.0L. Determine its volume if the pressure is reduced to 0.85atm and the temperature remains constant. Do you expect volume to go up or down? Formula: __14.1 L_______ 3. A gas exerts a pressure of 106kPa in a sealed, rigid container at 25C. At what temperature will it exert a pressure of 149kPa? Do you expect temperature to go up or down? Formula: ___419 K_______ 4. A gas exerts a pressure of 1.2atm in a 525mL container. Find the pressure of the same gas in a 2.5L container. Do you expect pressure to go up or down? Formula: _0.25 atm_______ 5. The temperature of a gas sample at standard pressure is 25C. Find its pressure if it is heated to 98C. Do you expect pressure to go up or down? Formula: __ 1.2 atm_______ 6. A gas occupies 240mL at 23C and 650mmHg. It is transferred to a 375mL container at 30C. Find the pressure in the new container. Formula: ___ 425.8mmHg__ 7. A gas occupies 525mL at 30C and 1.2 atm. What volume will it occupy at STP? Formula: ___ 568 mL_____ Ideal Gas Law: Adding in the Mole moles and pressure direct proportion  moles and volume direct proportion moles and temperature inverse proportion Ideal Gas Law equation: PV = nRT Determining R: Other values for R: 8.31 kPa . L 0.0821 L. atm 62.4 mHg . L mol . K mol . K mol . K Example: What volume is occupied by 0.250 mol of carbon dioxide gas at 250C and 371mm Hg? 12.5 L 2. Find the mass of oxygen in a 750mL container at 745mmHg and 23C. 0.97 g O2 3. At what temperature will 12.0g of nitrogen occupy 32.0L if the pressure is 100kPa? 895.5 K GAS STOICHIOMETRY Avogadros law shows that the mole ratio of two gases at the same temperature and pressure is the same as the volume ratio of the two gases. Write the balanced equation when sodium reacts with water: __________2 Na + 2 HOH ( 2 NaOH + H2_____________________________________ What type of reaction is this? ___single displacement_____________________ How many liters of hydrogen gas will be produced at 280.0 K and 96.0 kPa if 40.0 g of sodium react with excess water? 40g Na 1 mole Na 1 mole H2 = 0.8658 mol  23.1 g Na 2 moles Na PV = nRT 96kPa (V) = 0.8658 mole (8.31 kPa L/ mole K) 280K V = 20.98 L Write the balanced that occurs when aluminum carbonate decomposes to form aluminum oxide and carbon dioxide. ____Al2(CO3)3 ( Al2O3 + 3 CO2_______________________________________________ What type of reaction is this? ____decomposition____________________ What volume of carbon dioxide, at 295.0 K and 880 mmHg, will be formed if 50.0g of aluminum carbonate decompose? 50g Na 1 mole Al2(CO3)3 3 mole CO2 = 0.641 mol  234g Al2(CO3)3 1 mole Al2(CO3)3 PV = nRT 880mmHg (V) = 0.641 mole (62.4mmHg L/ mole K) 295K V = 13.4 L USING THE IDEAL GAS LAW TO FIND MOLAR MASS AND DENSITY Molar Mass = mass of gas moles of gas What is the molar mass of the element that has a mass of 89.78g and occupies 45 L at 2.5 atm and 35oC.? Identify the element. PV=nRT 2.4atm (45L) = n (0.0821)(308K) n=4.4 mol MM = 89.78g = 20.4 g/mol = Neon 4.4 mol TRY: Find the molar mass of a gas if 0.75g of the gas fill a 500mL flask at 23C and 747mmHg. PV=nRT 747mmHg (0.5L) = n (62.4)(296K) n=0.02 mol MM = 0.75g = 37.5 g/mol 0.02 mol Density = mass of gas L of gas What is the density of carbon disulfide (gas) at STP? PV=nRT 1atm(1L) = n (0.0821)(273) n=0.0446 0.0446 moles 76.2 g = 3.4g/1L  1 mole What is the density of nitrogen gas at 102kPa and 45C? PV=nRT 102 kPa(1L) = n (8.31)(318) n=0.0386 0.0386 moles 28 g = 1.08g/1L  1 mole MOVEMENT OF GAS PARTICLES: MAXWELL-BOLTZMAN DISTRIBUTION  a. If both samples contain the same gas, which sample is at a higher temperature? B (higher speed = higher temp) b. If both samples are at the same temperature, which gas has the higher molar mass? A (lower speed, lower temp) GRAHAMS LAW: PARTICLE SPEED AND MASS Temperature is the average kinetic energy of particles in a sample. Kinetic energy is related to particle speed and mass. If two particles are at the same temperature, the lighter one will have the higher speed. If a sample of hydrogen and a sample of nitrogen are each is a sealed 1.0L container at the same temperature and the same pressure: which sample contains more molecules? ____ same_________________ which sample is heavier? ___ N2______ c. which sample has the greater average kinetic energy? ___ same______ d. in which sample are the particles moving faster? ____ H2_________ DALTONS LAW AND PARTIAL PRESSURE OF GASSES  DALTONS LAW: the total pressure of a system is equal to the sum of the pressures of all the gases in the system PT = P1 + P2 + Pn a. The container above contains 4.0moles of hydrogen, 3.0 moles of nitrogen and 2.0 moles of carbon dioxide. The total pressure of the container is 450mmHg. Determine the partial pressure of each gas.  PH2 = 4 moles H2 x 450 mmHg = 200 mmHg 9 moles total  PN2 = 3 moles N2 x 450 mmHg = 150 mmHg 9 moles total  PCO2= 2 moles CO2 x 450 mmHg = 100 mmHg 9 moles total b. The pressure of nitrogen in the classroom is approximately 0.82atm. The pressure of oxygen in the room is approximately 0.20atm and the pressure of water vapor in the room is approximately 0.02atm. a. The total pressure in the room is 1.10atm. Assuming carbon dioxide is the only other gas present, find the pressure of carbon dioxide in the room. 1.10 atm = 0.82 atm + 0.2 atm + 0.02 atm + PCO2 0.06 atm = PCO2 b. Find the number of moles of oxygen in the room if the room holds 8500 moles of air. 0.02 atm O2 = x moles O2  1.1 atm total 8500 moles total 154.55 atm = moles O2 COLLECTING GASSES OVER WATER.  Oxygen gas is collected by water displacement in a 250mL flask at 30C and a barometric pressure of 95.00kPa. The vapor pressure of water at 30C is 31.82kPa. Determine the pressure of the dry oxygen in the flask. Patm = PH2O + Pgas 95.00 kPa = 31.82 kPa + Pgas 63.18 kPa = Pgas Determine the number of moles of dry oxygen in the flask. PV=nRT 62.18kPa (0.25 L) = n (8.31)(303K) 0.006 mol = n HOMEWORK #1: MIXED GAS LAWS SHOW ALL WORK FOR ALL PROBLEMS 1.0 atm = 760 mmHg = 101.3 kPa And 0C = 273 K Change the following units: 359 kPa = ___3.5______ atm 10C = _283_______ K 6.2 atm = _4712_______ mmHg 10K = _-263______ C FOR EACH PROBLEM, WRITE OUT THE FORMUA YOU ARE USING. WRITE YOUR ANSWER IN THE SPACE PROVIDED. 1. The gas in a sealed can is at a pressure of 3.00 atm at 25C. A warning on the can tells the user not to store the can in a place where the temperature will exceed 52C. What would the gas pressure in the can be at 52C? P1 = P2 T1 T2 3atm = P2 298 K 325 K 3.27 atm = P2 2. A sample of hydrogen exerts a pressure of 0.829 atm at 47C. At what temperature will the pressure raise to 1.5atm. P1 = P2 T1 T2 0.829atm = 1.5 atm 320 K T2 579.0 K = T2 3. A sample of neon gas occupies a volume of 752 mL at 25C. What volume will the gas occupy at standard temperature if the pressure remains constant? V1 = V2 T1 T2 752 = V2 298 273 688.9 mL = V2 4. A sample of oxygen gas has a volume of 150 mL when its pressure is 440 mmHg. If the pressure is increased to standard pressure and the temperature remains constant, what will the new gas volume be? P1V1 = P2V2 440 (150) = 760 (V2) 86.6 mL = V2 5. Ralph had a helium balloon with a volume of 4.88 liters at 150 kPa of pressure. If the volume is changed to 3.15 liters, what would be the new pressure in atm? P1V1 = P2V2 150 (4.88) = P2 (3.15) 232.4 kPa= P2  232.4 kPa 1 atm = 2.29 atm  101.3 kPa 6. 536 mL of nitrogen gas are at -25C. At what temperature will it expand to 2.2L if the pressure remains constant. V1 = V2 T1 T2 0.536 L = 2.2 L 248 K T2 1017.9 K = T2 HOMEWORK #2: COMBINED GAS LAW/MIXED A gas has a pressure of 725mmHg in a 2.0L container at 33C. Determine its pressure in a 3.5L container at 100.0C. P1V1 = P2V2 T1 T2 725mmHg (2.0 L) = P2 (3.5L) 306K 373K 505 mmHg= P2 A gas occupies 550mL at 98C and 890mmHg. Determine its volume at STP. P1V1 = P2V2 T1 T2 550mL (890mmHg) = 760 mmHg (V2) 371K 273 K 473.9mL= V2 Determine the temperature of a gas at 650mmHg in a 5.0L container if it occupies 875mL at 23C and 425mmHg. P1V1 = P2V2 T1 T2 650 mmHg (5L) = 425mmHg (0.875 L) T1 296K 2586.9 K = T1 4. A gas expands to 4.4L at 65C. At what temperature will it contract to 950mL. V1 = V2 T1 T2 4.4 L = 0.950 L 338 K T2 73.0 K = T2 5. Find the volume of a gas at 1.2atm if its volume is 650mL at 600mmHg. P1V1 = P2V2 912 mmHg (V1) = 650mL (600mmHg) V1 = 427.6mL 6. A gas occupies 855mL at 32C and 455mmHg. At what temperature will it occupy 1.8L at 99kPa? P1V1 = P2V2 T1 T2 455 mmHg (0.855L) = 742.7mmHg (1.8 L) 305 K T2 1048.2 K = T2 7. Find the volume of a gas at STP if it occupies 2.3L at 29C and 1.1atm. P1V1 = P2V2 T1 T2 1.1atm (2.3L) = 1atm (V2) 302 K 273K 2.3 L = V2 HOMEWORK #3: IDEAL GAS LAW  1) How many moles of a gas at 100C does it take to fill a 1.00 L flask to a pressure of 1.50 atm? 0.05 moles 2) A camping stove uses a 2.0L propane tank that holds 30g of liquid C3H8. Find the pressure in the tank at 25C. 8.3 atm 3) What volume would be occupied by 100 g of oxygen gas at a pressure of 1.50atm and a temperature of 25C? 51.0 L 4) On a warm day, a very large amusement park balloon is filled with 47.8 g of helium. The temperature is 33C and the pressure in the balloon is 785mmHg. Calculate the volume of the balloon. 290.7 L 5) A ten-liter gas cylinder contains 380 g of nitrogen. What pressure, in kPa, is exerted by the nitrogen at 25C? 3367.9 kPa 6) A drum used to transport crude oil has a volume of 162 L. How many water molecules, as steam, are required to fill the drum at 1.00 atm and 100C? 3.2 x 1024 molecules 7) How many moles of air are there in a 125 mL erlenmeyer flask if the pressure is 755 mm Hg and the temperature is 20C? 0.005 moles HOMEWORK #4: GAS STOICHIOMETRY, ETC 1. Write the balanced equation for the reaction that occurs when chlorine gas is bubbled through a solution of sodium iodide. Cl2 + 2 NaI ( 2 NaCl + I2 Use stoichiometry to predict the volume of chlorine gas, at STP, needed to react with 45.0g of sodium iodide. 45 g NaI 1 mole NaI 1 mol Cl2 22.4 L Cl2  149.9g NaI 2 mol NaI 1 mol Cl2 3.4 L Cl2 Use stoichiometry and gas laws to predict the volume of chlorine gas, at 32C and 750mmHg, needed to react with 125g of sodium iodide.  125 g NaI 1 mol NaI 1 mol Cl2 = 0.4169 mol Cl2  149.9 g NaI 2 mol NaI PV=nRT 750mmHg(V) = 0.4169mol (62.4)(305K) 10.6 L = V 2. Write the balanced equation for the combustion of ethylene, C2H2. 2 C2H2 + 5 O2 ( 4 CO2 + 2 H2O What mass of ethylene must burn in order to form 2.2L of carbon dioxide, at 98kPa and 25C? PV=nRT 98kPa (2.2L) = n(8.31)(298K) 0.087 = moles CO2  0.087mole CO2 2 mole C2H2 26 g C2H2 = 1.13g C2H2  4 mole CO2 1 mole C2H2 3. After the reaction, a student measures the volume of carbon dioxide actually formed. He measures 1.8L. Determine the percent yield and percent error. 1.8L/2.2L x 100 = 81.8 % yield 100-81.1 = 18.2% error HOMEWORK #5: MIXED GAS LAWS 1. A container holds 1 mole of nitrogen, 6 moles of methane and 5 moles of carbon dioxide. The total pressure in the container is 800mmHg. Find the pressure of each individual gas. PN2 = 66.7mmHg PCH4 = 400mmHg PCO2 = 333.3 mmHg 2. a) A student collects oxygen over water at 23C. The atmospheric pressure is 755mmHg. The water vapor pressure at this temperature is 21.1mmHg. Find the pressure of the dry oxygen gas. 733.9mmHg ***b. The student collected a total of 5.0moles of gas. Using your answer from part a, how many moles of oxygen did he collect? ________________ 3. Find the temperature of a gas sample that contains 54g of oxygen in a 32L container at 1.2atm. 275.1 K 4. A gas exerts a pressure of 88kPa in a 3.0L container. The container expands to 4.5L. 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A gas occupies 250mL at 60C and 425mmHg. Determine its volume at STP. 114.6 L 6. A student has a 500mL flask filled with NO2 at 1.2atm and 25C. He fills a second 500mL flask with O2 at 1.2atm and 25C. Which flask is heavier? NO2 Which flask has more molecules? same Which flask has the higher average kinetic energy? same In which flask are the molecules moving faster? O2 HOMEWORK #6: CHAPTER 13-14 REVIEW 1. A gas occupies a volume of 6.25 liters at 25.0C. What volume would it occupy at  25.0C? 5.2 L 2. If a gas occupies a volume of 3.75 liters and exerts a pressure of 925 mm Hg at 95.0C, what pressure would it exert at 75.0C and in a volume of 1.90 liters? 1726.4 mmHg 3. Find the density of carbon monoxide at 600mmHg and 33C. 0.88 g/L 4. If a gas occupies a volume of 125 ml at a pressure of 0.415 atm, what pressure will the gas exert in a 79.0 ml container? 0.66 atm 5. What mass of chlorine gas will occupy 1250 ml and exert a pressure of 2100 mm Hg at 100.0C? 8.0 g Cl2 6. What volume will 1.85 moles of xenon occupy at 1025 mm Hg and 100.0C? 42.0 L 7. 70.4g of a gas occupies 40.0L at 23C and 745mmHg. Find the molar mass of the gas. 43.7 g/mol 8. Write the reaction for the decomposition of sodium chlorate to form sodium chloride and oxygen. 2 NaClO3 ( 2 NaCl + 3 O2 What volume of oxygen, at 755mmHg and 25C, will be formed by the complete decomposition of 125g of sodium chlorate? 43.3 L 9. A container holds 2.5moles of nitrogen and 5.5 moles of helium at STP. The total pressure of the container is 600mmHg. Find the pressure of the helium. 412.5 mmHg Which gas is moving faster, the helium or the nitrogen? He     %Ci    YZ[\]ij7$gd\B Agd_qgd & FgdVX|~ Y]`hi    ( * ,                   K L M źźХۡhR/hIhIhIB*H*phh\BB*phhIhB*phhIh_qB*phhIhIB*phh_qhOJQJh5OJQJh5wqh5OJQJh>jk      , .             Agd_qgd      L M f g h                  $a$gdI Agd_qgdM T U V W d e f                         -.45K]_goyhGih*5>*h*B*phh%Lh*mH sH h*mH sH hPmHnHuUjh*Uh*hqq}jhqq}U ho\hh_qhIh_qB*ph jhIhIB*phhIhIB*H*phhIhIB*ph-                  ./012345  $&gdIgd-[ygdT)$ Agd_qgd PAGE \* MERGEFORMAT 16 Ch 13 & 14 Notes Type of relationship? Direct proportion Equation P1 = P2 T1 T2 Temperature MUST be in Kelvins (K = C + 273) Type of relationship? Direct proportion Equation: V1 = V2 T1 T2 Temperature MUST be in Kelvins (K = C + 273) H2 N2 H2 CO2 H2 N2 CO2 H2 N2 8.31 kPa . L 0.0821 L. atm 62.4 mHg . L mol . K mol . K mol . 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