Unit 11 Packet - Page 1 Of 14 Honors Chemistry - Unit 11
Unit 11 Packet - Page 1 of 14Honors Chemistry - Unit 11Chapters 10 & 11 – Gases, Gas Laws, and Gas StoichiometryVocabulary Due:Quizzes:UT Quest(s):Test Date:VOCABULARY:Ideal gasdiffusionstandard atmospheric pressureeffusionstandard temperaturemolar volumeSTPCONSTANTS/FORMULAS:Boyle’s lawCharles’ lawGay-Lussac’s lawCombined gas lawDalton’s lawGraham’s lawIdeal gas lawMolar volumeMolecular Mass Determination (of a gas)OBJECTIVES: Memorize the values for STP. Memorize and be able to apply the gas laws: Boyle’s, Charles, Dalton’s law of partial pressure,Combined gas law, Gay-Lussac’s, and Graham’s. Be able to use molar volume of a gas at STP in problems. Be able to calculate gas density at STP. Memorize and be able to apply the ideal gas law. Memorize the gas constant R .0821 L-atm/mol-K. Be able to do problems involving gas stoichiometry (at STP and other conditions).STP: Standard temperature and Pressure; 00 C(273K) and 1 atmPressure conversions (all of these values are equal to each other and any two can be set-up as a ratio to beused in a factor label problem!)1 atm 760 torr 760 mm Hg 101.3 kPa 1.01 x 105 PaPRESSURE CONVERSION PROBLEMS(Show work on your own paper and attach to packet).Place these eight pressure measurementsin order from largest amount of pressure tosmallest amount of pressure:2) 72.0 kPa mm of HgA. 1.1 atmB. 59 kPa3) 435 mm of Hg atmC. 14 mm Hg4) 1100 torr mm HgD. 4000 kPaE. 6900 mm Hg1) 560 torr kPa5) 1.6 atm kPa6) 48.6 kPa atm7) 0.8 atm torr8) 82 torr kPa9) 760 mm Hg atm10) 2.0 kPa torr11) 485 mm Hg kPaF. 75.0 kPaG. 9.2 atmH. 436 torr
Unit 11 Packet - Page 2 of 14Unit 11 BELLWORK SET – Gases, Gas Laws, and Gas StoichiometryReview:1. Draw the dot diagram for Bismuth.2. Draw the Lewis Structure for the following and identify the VSEPR Shape:A. Carbonate ionB. silicon disulfideCurrent Unit Material3. A sample of diborane gas (B2H6) a substance that bursts into flame when exposed to air, has a pressureof 345 torr at a temperature of –150C and a volume of 3.48 L. If conditions are changed so that thetemperature is 360C and the pressure is 268 torr, what will be the volume of the sample?4. The density of a gas was measured at 1.30 atm and 470C and found to be 1.95 g/L. Calculate the molarmass of the gas.5. Mixtures of helium and oxygen are used in scuba diving tanks to help prevent “the bend”. For aparticular dive, 46 L of O2 at 250C and 1.0 atm and 12 L He at 250C and 1.0 atm were pumped into a tankwith a volume of 5.0 L. Calculate the partial pressure of each gas and the total pressure in the tank at250C. Hint: Label all of the variables and calculate each tank (oxygen and helium) as separate problems!6. Calculate the volume of oxygen gas at 85 0C and 789 torr, required for the complete combustion of 45 gof octane (C8H18).
Unit 11 Packet - Page 3 of 14Unit 11 - Gas Laws NotesGases: 4 measurable quantities:Volume 1 ml 1 cm3PressureTemperature# of molesVariables?STP?**GAS LAWS – Must be Memorized!!**!Boyle’s law - P1 V1 P2 V2 (V varies inversely with P)Graph of P vs V?inversely?Example. If 1.0 L of a gas at 1.2 atm is allowed to expand to 5.0 L, what is the new pressure?You try: A sample of O2 gas has a volume of 150 ml when its pressure is 720 mm Hg, what willthe volume be if the pressure is increased to 750 mm Hg?(Answer: 144 ml)Charles law: V1/T1 V2/T2(V varies directly with the Kelvin temperature)T must be in Kelvin Graph of V vs T? Directly? Why T in K?Example: A helium filled balloon has a volume of 2.75 L at 20.0 0C . The volume of the balloondecreases to 2.46 L after it was placed outside on a cold day. What is the outside temperature?You try: A sample of neon occupies a volume of 752 ml at 25 0 C. What volume will the gasoccupy at 50. 0C?(Answer: 815 ml)
Gay-Lussac’s Law: P1/T1 P2/T2Unit 11 Packet - Page 4 of 14(P varies directly with Kelvin Temperature)Like which other law?You Try: Before a trip from Raleigh to NY, the pressure in a tire is 1.8 atm at 20 0C. At the endof the trip the pressure gauge reads 1444 mm Hg. What is the new temperature in the tire?(Answer: 309 K (or 36 0C))Combined Gas Law: P1V1 P2V2T1T2T must be in K!!!Example: If 282.4 ml of a gas at 25 0C and 1.3 atm is cooled to 20. 0C and 780 mm Hg. What isthe new volume?You try: a 700. ml gas sample at STP is compressed to a volume of 200. ml, and the temperatureis increased to 30.0 0C. What is the new pressure of the gas in kPa?(Answer: 394 kPa)
Unit 11 Packet - Page 5 of 14Dalton’s law of Partial Pressures: pressure of each gas in a mixture is called thepartial pressure of that gas. Total Pressure sum of partial pressuresPT P1 P2 P3 . etc.Special case: gases collected by water displacement – see diagram on board!Use formulaPT Patm Total atmosphere gasPatm from lab or is given:Pg PH2OwaterPH2O Table page 899Example: Oxygen is collected by water displacement. The barometric pressure andtemperature are 84.5 kPa and 20.0 0C. What is the partial pressure of O2?You try: A gas is collected over water and the atmospheric pressure is 101.1 kPa at 50 C. Whatis the partial pressure of the gas?(Answer: 88.8 kPa)Graham’s LawReview: Effusion? Diffusion?**Rate of effusion and diffusion varies inversely with the mass of the gas.**Rate of gas A Square Root Mass of gas BRate of gas BMass of gas AExample: Compare the rates of effusion of Hydrogen and oxygen at STP.You try: Compare the rates of effusion of Fluorine and chlorine(Answer: Fluorine is 1.4 x faster than chlorine)
Ideal Gas Law NotesUnit 11 Packet - Page 6 of 14PV nRTMust use the following units with the ideal gas law!P atmV LT Kn molesR gas constant 0.0821 L-atm/mol- K (memorize)Example: What is the pressure exerted by a 12.0 g sample of Nitrogen gas (N2) in a 10.0 Lcontainer at 25 0C?Practice Ideal Gas Law Worksheet: 1 – 4 (page 8 in packet)Gas StoichiometryMolar Volume - 1 mol of any gas at STP has a volume of 22.4 L1 mol22.4 L conversion factor (only to be used at STP)Example: What is the mass of 98.0 ml of sulfur dioxide at STP? (work together on board – copyinto your notes!)You try: What is the mass of 1.33 x 104 ml of O2 at STP?Gas Density: D ?At STP : D Molar massMolar volumeg/mol (PT)22.4 L/molEx: What is the density of CO2 at STP?You try: What is the molar mass of a gas with a density of 1.56 g/L ?
Molecular Mass Determination from Ideal Gas Law:(see derivation on board)Unit 11 Packet - Page 7 of 14D PM density pressure (atm) x molar mass/ constant x temp (K)RTExamples & practice on ideal gas law worksheet!Stoichiometry of GasesCan do L-L conversions (just like mol-mol) with 2 gases and an equationExample: Given: C3H8 (g) 5 O2 (g) à 3 CO2 (g) 4 H2O (l)How many L of O2 are required to react with 0.35 L of propane?**You may have to use molar volume!****You may have to use the ideal gas law!**Example 2: Given CaCO3 (s) à CaO (s) CO2 (g)How many grams of calcium carbonate must decompose to from 5.0 L of CO2 at STP?You try: If 10.0 g of lithium chloride decomposes how many liters of Cl2 gas are produced atSTP? (write a balanced equation first!)Example 3: How many liters of H2 at 35 oC and 745 mm Hg are need to react completely with825 g of WO3?WO3(s) 3H2 (g) à W(s) 3H2O (l)You try:How many L of CO at 27 0C and 788 mm Hg can be produced from 65.5 g of carbon?2C(s) O2(g) à 2CO(g)Next: Practice Stoichiometry & Gas Stoichiometry Sheets
GAS LAW PROBLEMSUnit 11 Packet - Page 8 of 14Work the following problems and identify the gas law used; be sure your answer includes units!1. A gas occupies a volume of 35.9 ml at a temperature of 22.0 C. What volume will the samegas occupy at a temperature of 28.0 C?2. At a pressure of 780 mm Hg and 24.2 C a gas has a volume of 350.0 ml. What will the volumeof this gas be under standard conditions?3. A gas occupies a volume of 24.8 ml at 725 torr. What will the pressure of the gas be at 22.5ml?4. A gas occupies a volume of 40.8 ml at a temperature of 33.5 C. At what temperature will thevolume of the gas be 39.2 ml?5. If 45.0 ml of a gas is under 1.3 atm of pressure; at what pressure will the volume be 60.0 ml?6. Compare the rates of effusion of nitrogen and bromine gas at the same temperature andpressure.7. A gas at a temperature of 67.5 C and a pressure of 882 torr occupies a volume of 242.2 ml.What will the volume of the gas be at 840 torr and 80.0 C?8. A gas with a volume of 388.9 ml at a pressure of 1.0045 atm is subjected to a pressure of 1.877atm. What is its volume at the new pressure?9. Hydrogen gas is collected over water and the atmospheric pressure in 122kPa at 50 C. Whatis the partial pressure of hydrogen?Ideal Gas Law PracticeRemember: PV nRT and D PM/RTMust use atm, L, moles and K R .0821 L-atm/mol-K1. How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 25 0C ?2. What volume will 2.0 moles of nitrogen occupy at 720 torr and 20.0 0C?3. What pressure will be exerted by 25 g of CO2 at a temperature of 25 0C and a volume of 500.ml?4. At what temperature will 5.00 g of Cl2 exert a pressure of 900. torr at a volume of 750. ml?5. What is the density of NH3 at 800. torr and 25. 0 C?6. If the density of a gas is 1.2 g/L at 745 torr and 20. 0C, what is its molecular mass?7. How many moles of nitrogen gas will occupy a volume of 347 ml at 6680 torr and 27 0C?8. What volume will 454 grams of hydrogen occupy at 1.05 atm and 25 0C? (remember hydrogenis diatomic!)9. Find the number of grams of CO2 that exerts a pressure of 785 torrs at a volume 32.5 L and atemperature of 32 0C.10. An elemental gas has a mass of 10.3 g. If the volume is 58.4 L and the pressure is 758 torrat a temperature of 2.5 0C, what is the gas (Hint find the molar mass!)
STOICHIOMETRY WORKSHEETUnit 11 Packet - Page 9 of 14Work the following stoichiometry problems on your own paper and attach to packet.1. Write the correctly balanced equation for the decomposition of MgCl2.2. Using the above equation and given 5.0 grams of MgCl2, how many grams of magnesium areproduced?HINT: grams ßà moles ßà mole ratio ßà moles ßà grams3. What is the volume of 1 mole of a gas at STP?4. Using the equation from #1 determine the volume of chlorine gas produced from 5.0 grams ofmagnesium chloride.5. Balance the following equation:Cu HNO3 à Cu(NO3)2 H26. Given 2.00 grams of copper and an excess of nitric acid how much hydrogen gas is produced?7. How many grams of copper (II) nitrate are produced?Answer the following questions about the ideal gas law.8. Write out the ideal gas equation.9. What is the ideal gas constant?10. What is the volume of a 2.00 mol gas sample at a pressure of 1.2 atm and a temperature of301K?Gas Stoichiometry Worksheet1. What is the density of nitrogen trioxide at STP?2. How many moles of helium gas are there in 23 L of helium at STP?3. What is the volume of 1.5 g of PCl gas at 545 mm Hg and 55 C?4. How many moles of iodine gas are there in 550 ml of gas at 2.1 atm and 27 C?5. At STP how many liters of carbon monoxide can be produced from burning 32.5 g of oxygenaccording to the following equation:2 C (s) O2 (g)à2 CO (g)6. Using the above equation, what volume of oxygen is required to produce 375 ml of CO at STP?7. What volume of oxygen in liters can be collected at 750 mm Hg and 25.0 C when 36.0 g ofKClO3 decomposes according to the following equation? BALANCE THE EQ FIRST!KClO3à KCl O28. What is the mass of 1258 ml of hydrogen gas at STP?
Unit 11 Packet - Page 10 of 14Mini Lab – CARTESIAN DIVERWork in a group with your lab table.Each person will answer the questions after doing the lab.You do not have to do a “formal” lab write up.Materials (per table)1 empty plastic 2 Liter bottletap water1 dropperProcedure:1. Using the prepared Cartesian Diver bottles. Squeeze the middle of the each bottle with as much force aspossible.2. Rank the bottles in the order of hardest to squeeze (requires most pressure to cause the dropper to sink) toeasiest to squeeze and record your ranking order here:Questions:1. What happened when you squeezed the bottle? Explain why this happens.(use ‘chemistry’ ideas and terms)2. Can you get the dropper to ‘float’ in the middle of the bottle? How?3. What gas law does the Cartesian diver demonstrate?Mini-lab - Marshmallow Fun!Procedure:1. Each group will receive one syringe and two mini marshmallows (do not eat them!)2. Pull the plunger out of the syringe.3. Place one marshmallow in the syringe – replace the plunger – do not squish the marshmallow!4. Set the syringe around 3ccs and then cover the tip of the syringe with your thumb – pull back on the plungerwithout removing your thumb. Observe.QUESTION # 1 – What happened? Use chemistry ideas in your explanation.5. Remove your thumb – reset the plunger as high as possible (around 12 ccs) put your thumb back over thesyringe and press down on the plunger.QUESTION # 2 - What happened? Use chemistry ideas in your explanation.6. Replace with a “fresh” marshmallow when necessary.7. Clean up throw away used marshmallows and return syringe to your teacher.Question # 3 - What gas law does this demonstrate?Question # 4 - If the original pressure inside the syringe is 1.0 atm and the marshmallow has a volume of 1.3ml what volume will the marshmallow occupy if the pressure is decreased to 0.75 atm?Question # 5 - Why do you eventually need a “fresh” marshmallow?
Unit 11 Packet - Page 11 of 14MINI LAB - THE COLLAPSING SOFT DRINK CANDo this lab as a group – the whole table will work together to perform the procedure. Eachstudent is to individually answer the questions.Procedure:1. Place about 5 ml of water in an empty aluminum soft drink can. (Be sure the can is cleanfirst. Place on a hot plate.2. Boil the water in the can vigorously for a minute, until the can is filled with water vapor.(Watch for steam to escape for about 30 seconds).3. Carefully (using tongs) and quickly invert the can and place it, top down, into a large beakercontaining about 1 –2 inches of water a few ice cubes. Your teacher will demonstrate howthis is to be done.4. Observe!Answer the following questions:1. What happened when the can was placed in the water?2. Explain “why” using chemistry terms!3. What gas law does this demonstrate?Empty water from the can and place it in the can recycling.Put hot plate to the side – make sure it is UNPLUGGED!Return safety glasses.
Unit 11 – Gases, Gas Laws, & Gas StoichiometryUnit 11 Packet - Page 12 of 14STUDY GUIDE REVIEWINFORMATION TO BE MEMORIZED/Used:As practice; write the formulas without your notes!Charles’ LawBoyle’s LawGay-Lussac’s LawCombined gas lawDalton’s lawGraham’s lawIdeal gas lawR Molar volume at STPSTP Density at STP and Density NOT at STPMolar Mass from the Ideal Gas LawPRACTICE PROBLEMS: Work without your notes – just your reference packet!1. If 259 ml of oxygen gas is at 112 kPa, what will the volume be at standard pressure?2. What is the pressure of helium gas collected over water, if the barometric pressure is 88.3kPa and the temperature is 30 C?3. What is the volume of a gas at 273 K, if it had a volume of 22.8 ml at 48 C?4. If a 25 ml of sulfur dioxide is at 37 C and 90.2 kPa, what will the temperature be if thevolume becomes 19.6 ml and the pressure is 760 torr.5. What is the volume of 156 grams of chlorine gas at STP?6. What is the pressure exerted by 1.32 moles of gas in an 18 L vessel at 27 C?7. A 759 ml vessel contains 0.0945 mol of a gas at 98.6 kPa. What is the temperature of the gas?8. What volume of hydrogen gas at STP will be produced from 16.7 g of magnesium reactingwith an excess amount of hydrochloric acid?9. What volume of fluorine gas is required to react with 2.67 g of calcium bromide to formcalcium fluoride and bromine at 41 C and 4.31 atm?10. Which one of the following will diffuse the fastest at STP: NH3, CH4, Ar, HBr?ANSWERS:1. 286 ml5. 49.2 L9. 79.9 ml2. 84.1 kPa6. 1.81 atm10. CH43. 19.4 ml7. 95.3 K4. O C (273 K)8. 15.4 L H2
Unit 11 Packet - Page 13 of 14Flick Your Bic – Molar Mass Determination of ButaneObjective: To use the ideal gas law to determine the molar mass of butane.Equipment: make an equipment list after reading the procedureProcedure:1. Weigh the lighter.2. Fill a graduated cylinder up with water and invert it into a large beaker/container. Make sure thereare NO bubbles in the cylinder!3. Through water displacement collect about 25-40 ml of butane gas in your cylinder. You will do this byplacing the lighter under the water into the mouth of the cylinder. Then press the button to releasegas into the cylinder – the gas should displace the water and you should get a graduated cylinderfilled with gas – do not light the lighter.4. Carry your inverted cylinder with to the fume hood and release the butane in the hood – do not inhale.5. Dry off the lighter and reweigh it. The lighter must be VERY dry or the moisture will interfere withyour results.6. Use a thermometer to get the temperature of the room.7. Check the whiteboard to get the atmospheric pressure.Data Table with Results (Shaded Areas are Calculated Results!)Data Collection (don’t forget units!):Mass of Butane lighter (before):Mass of Butane lighter (after):Mass of butane used:Volume of water displaced volume of butanecollected from the lighter:Temperature of the room:Atmospheric pressure:Calculations:Pressure of the butane:Moles of butane:Molar mass of butane:Empirical Formula/Molecular FormulaPercent error:Calculations: Show all work here!1. Using Dalton’s law of partial pressures – calculate the partial pressure of the butane and enter inyour data table beside the pressure of butane.2. Using the ideal gas law, calculate the moles of butane and enter in your data table.
Unit 11 Packet - Page 14 of 143. Using your answer for the moles of butane from (2) and your mass of butane used (data table) –calculate the molar mass of butane.4. The percentage composition of the gas in the lighter is as follows: carbon, 82.63% and hydrogen,17.37%. Calculate the empirical formula for butane and enter in the data table.5. Using your molar mass, see if you can get a whole-number multiple of the empirical formula for themolecular formula of the gas and enter your result in the data table.6. Given that the molar mass of butane is 58 g/mol – calculate your percent error.Questions:1. How do you explain the fact that the “gas” is a liquid in the lighter, but a gas when it is collected(think phase diagram .)?Complete the following Error Analysis Table – listing at least two possible errors and their effect onthe molar mass (would it be higher or lower – and why!)ErrorAnalysisConclusion: Write a paragraph conclusion – a minimum of three grammatically correct sentences!
Boyle’s law Charles’ law Gay-Lussac’s law Combined gas law Dalton’s law . Practice Ideal Gas Law Worksheet: 1 – 4 (page 8 in packet) Gas Stoichiometry . Work the following problems and identify the gas law used; be sure your answer includes units! 1. A gas
Acme Packet 1100 Acme Packet 3900 Acme Packet 4600 front bezel hides the fan assemblies without restricting airflow through the system. Acme Acme Packet 6100 Acme Packet 6300 Packet 6300 Acme Packet 6350 The rear of Acme Packet 6300 least one slot reserved for an NIU.
Trigonometry Unit 4 Unit 4 WB Unit 4 Unit 4 5 Free Particle Interactions: Weight and Friction Unit 5 Unit 5 ZA-Chapter 3 pp. 39-57 pp. 103-106 WB Unit 5 Unit 5 6 Constant Force Particle: Acceleration Unit 6 Unit 6 and ZA-Chapter 3 pp. 57-72 WB Unit 6 Parts C&B 6 Constant Force Particle: Acceleration Unit 6 Unit 6 and WB Unit 6 Unit 6
Bonding Unit 2.10: Compounds and Bonding Unit 4.10: The Mole and Stoichiometry . Unit 10 Packet page 1 IF 35 – Half Life of Radioactive Isotopes Unit 10 Packet page 2 : Half Life Practice Worksheet. Unit 10 Packet page s 3 – 4 . Limiting Reactants and Percent Yield. Week 9: May 11 – 15, 2020 (Unit 10) Monday Tuesday Wednesday Thursday Friday
ef-fec1we issued by sandy valley water district ,-eb ri 7 '. ovh :- vi) hjj\j (name by -@- index page 1. page 2. page 3. page 4. page 5. page 6. page 7. page 8. page 9. page 10. page 1 1. page 12. page 13. page 14. page 15. page 16. page 17. page 18. page 19. page 20. .
Acme Packet 1100 and 3900 Security Policy Page 1 of 32 1. Introduction 1.1 Overview This document is the Security Policy for the Acme Packet 1100 [1] and Acme Packet 3900 [2] appliances manufactured by Oracle Communications. Acme Packet 1100 [1] and Acme Packet 3
CONTENTS Page Thank you page 3 About the book 4 UNIT 1: About Academic IELTS Task 1 6 UNIT 2: Line Graphs – Language of Change 8 UNIT 3: Introducing a graph 20 UNIT 4: Grouping Information 26 UNIT 5: A More Complicated Line Graph 29 UNI T 6: Describing Bar Charts 36 UNIT 7: Describing Pie Charts 44 UNIT 8: Describing Tables 49
wavelet transform combines both low pass and high pass fil-tering in spectral decomposition of signals. 1.2 Wavelet Packet and Wavelet Packet Tree Ideas of wavelet packet is the same as wavelet, the only differ-ence is that wavelet packet offers a more complex and flexible analysis because in wavelet packet analysis the details as well
Packet 3 Packet 2 Packet 1 d. Spatial Reuse S N1 N2 N3 N4 N5 N6 N7 D d e Packet 3 Packet 2 Packet 1 d. Spatial Reuse L minimum hop separation for concurrent transmissions. Ω number of simultaneous transmissions. Accounting for interference from two other transmissions with L 3 yields.
