Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet

Transcription

1 Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Name: Date In Class Homework 1/5 Tue 1/6 Wed 1/7 Thur 1/8 Fri 1/11 Mon. LSM Welcome (back), Semester Plan, Gas Law Activities Computers: set up Google Classroom, PHET Gas Law Simulation Discuss of examples from end of video KMT in class questions In class notes 1: Gas Variables Dalton s Law of Partial Pressure Discussion and Calculating with Gas Laws from Video 2 Predictions for Wed Class Activity Watch Gas Law Video 1 and complete turn in sheet Watch Gas Law Video 2 and complete turn in sheet Pre Lab for Pressure Temperature Lab 1/12 Tue Pressure Temperature Lab Watch Gas Law Video 3 and complete turn in sheet 1/13 Wed Discussion and Calculating with Gas Laws from Video 3 1/14 Thurs In class notes 2: Gas Stoichiometry 1/15 Fri Gas Stoichiometry Calculations & Nomenclature Review 1/18 Mon NO SCHOOL (MLK Day) Pre-Lab for Molar Mass of Butane Lab 1/19 Tue Molar Mass of Butane Lab 1/20 Wed Review for Gas Law Test Study for Gas Test 1/21 Thur Gas Law Test PreLab for Mixing a solution Lab 1/22 Fri Mixing a Solution Lab 1

2 Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Video 1. Gas Properties and the KMT: Textbook: Chapter 12.1 pages Guided Notes for Video on Gas Properties What is the difference atomically between a monoatomic, diatomic and polyatomic gas? What are the example I gave. Name: Questions: What is an ideal gas? List and describe the three postulates of the Kinetic Molecular Theory (KMT): List the four properties of gases: How do gases exert pressure? How can you increase the pressure of a gas? 2

3 Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Name: In Class Notes 1 on Gas Variables: 1. List the 4 variables when measuring gases, and the units they are in. Variable Unit measured in Description/important info (conversion factors, etc) 2. What is STP and what are the conditions for STP? 3. What is a barometer? 4. What did Dalton say was true about the pressure of a gas sample if it was composed of multiple gases? 5. What is Dalton s Law of Partial Pressures: a. In words: b. In equation form: 6. Show the calculation for the total pressure in a flask that contains 0.32 atm of water and 0.16 atm of oxygen: 7. Practice Problem: A mixture of O2 and N2 have a total pressure of 765 mmhg. If the partial pressure of O2 is 150 mmhg, what is the partial pressure of the N2? 3

4 Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Video 2. Gas Laws: Textbook: Chapter 13.1 pages Guided Notes for Video on Gas Laws What are the names of the four gas laws and what variables do they contain: Complete the following table: Law Name Equation Constant variables Relationship Name: Questions: What is the Combined Gas Law: In words: In equation form: Work out the practice problems from the video below: Boyles Law: A gas has a volume of 3.0 L at 2 atm. What will its volume be at 4 atm? Charles Law: A gas has a volume of 3.0 L at 127 C. What is its volume at 227 C? (CONTINUED ON NEXT PAGE) 4

5 Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Combined Gas Law Problem: A sample of helium gas has a volume of L, a pressure of atm & a temperature of 29 C. A) What is the new temperature( C) of the gas at a volume of 90.0 ml & a pressure of 3.20 atm? Name: B) What is the new volume of the gas if the conditions are changed to STP? Video 3. The Amount of a Gas and the Ideal Gas Law Textbook: Chapter 13.2 pages Guided Notes for Video on Amount and Ideal Gas Law What is Avogadro s Principle: In words: Questions: In equation form: Show your calculations for this problem: How many moles of He are contained in a 5 L balloon at STP? Show your calculations for this problem: You have 35 g of Neon gas in a 50 L container, what volume will 5 g occupy under that same temperature and pressure? (CONTINUED ON NEXT PAGE) 5

6 Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet What is the equation for the Ideal Gas Law? Name: What is the value of the gas constant? R = When calculating the ideal gas law, what units must be used for Pressure: Volume: Temperature: Amount: Show the work below to solve: How many grams N 2 is required to fill a small room with a volume of 27,000 L to 1.09 atm at 25 o C? In Class notes 2: Gas Stoichiometry Textbook Chapter 13.3 pages Show your calculations for this volume to volume conversion: 2 H2O2 (l) ---> 2 H2O (g) + O2 (g) 0.10 L of H2O2 is decomposed in a flask. What is the volume of O2 is produced at STP? 2. Show your calculations for this mass to volume problem: 2 H2O2 (l) ---> 2 H2O (g) + O2 (g) 1.1 g of H2O2 is decomposed in a flask. What is the volume of O2 produced under the same conditions? 3. When the conditions of the gas change during the chemical reaction, what are the steps for solving a gas stoichiometry problem? 4. Use the steps to solve this problem: A 2.0 L sample of oxygen gas reacts at 35 o C and a pressure of 2.5 atm. How many grams of NO are produced? 6

7 Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Name: 5. Show your work for this gas stoichiometry problem: If magnesium metal reacts with excess hydrochloric acid and 75.0 mls of H2 gas is produced, how many grams of Mg reacted? (The temperature is 24 o C and pressure is.966 atm) Mg(s) + HCl(aq) H2(g) + MgCl2(aq) 6. Last one: You try this on your own: Mg(s) + 2 HCl(aq) H2(g) + MgCl2(aq) What volume of H2 is produced (735mmHg and 15.0 o C) if 4.75 g of Mg react with excess HCl? 7

8 In Class Work Campbell Chemistry Video 1 Practice: 1. List the three postulates of the kinetic molecular theory and state whether or not you believe they do a good job of describing how real gases behave. 2. How could Kinetic Theory help you explain why you can smell cookies that is baking in the kitchen when you are in your bedroom? a. Would it make any difference if it were a hot or cold day? Why or why not? 3. Use diagrams to illustrate how an inflated balloon stays stretched. (What are the gas particles inside doing to keep it inflated?) 4. When you increase the temperature of a gas, what happens to the pressure? 5. When you increase the number of particles of a gas, what happens to the pressure? 6. When you increase the temperature, do the particles move faster or slower? 7. When the particles are moving are they moving in a pattern or randomly? In Class Notes 1 Practice: 8. What are the units of each property we are studying? a. Temperature? b. Pressure? 9. Convert the following: a C = K d atm = mmhg b. 145 K = 0 C? e mm Hg = atm c C = K f ml = L 8

9 In Class Work Campbell Chemistry 10. Dalton's Law of Partial Pressures a. A mixture of CO2 and N2 has a total pressure of 840 mmhg. If the partial pressure of the CO2 is 250 mmhg, what is the partial pressure of the N2? b. What would be the total pressure in atm in container that had a mixture of hydrogen gas at 0.5 atm and helium at 0.75 atm? What would that be in mmhg? Video 2 Practice: 11. Boyle's law. For each of the following sets of pressure/volume data, calculate the missing quantity. Assume that the temperature and the amount of the gas remain constant. a. V = 541 ml at 1.00 atm what is new Volume at 1.75 atm b. V = 2.32 L at mmhg what is new Volume at 995 mmhg c. V = 4.15 ml at 135 atm what is new Pressure in mmhg if V = 10.0 ml 12. Charles' Law. For each of the following sets of volume/temperature data, calculate the missing quantity. (Pay attention to units!!! Assume that the pressure and amount of the gas remain constant. a. V = 25.0 L at 0 o C what is the temperature in o C if V = 50.0 L? b. V = 247 ml at 25 o C what is the temperature in o C if V = 255 ml? c. V = 1.00 ml at 272 o C what is the volume in ml at 25 o C 13. Combined gas law. Given a gas under initial conditions, calculate the unknown quantity under new conditions. (Pay attention to units!!!) Initial conditions New conditions a. T = 285K, V = 1300 ml, P = 825mmHg T = 235 K, V =? P = 450 mmhg b. T= 265K, V = 2.57 L, P = 1455 mmhg T = 455 K, V = 1.45 L, P =? c. T = C, V = 1.45 ml, P =.42 atm T =? 0 C, V =.035 L, P = 625 mmhg 9

10 In Class Work Campbell Chemistry 14. What pressure (in atm) is required to compress 1000 ml of gas at 760 mmhg to a volume of 50.0 ml? L of a gas has a temperature of C. To what temperature ( 0 C) would you have to cool it to reduce the volume to 5.0 L? (constant pressure) 16. If 325 ml of a gas at 215 o C and 465 mmhg is changed to STP, what would be the new volume? Video 3 Practice: 17. Avogadro's law. a. If mol of nitrogen gas occupies a volume of 11.2 L at 0 o C, what volume will 2.00 mol of nitrogen occupy at the same temperature and pressure? b. If 46.2 g of oxygen gas occupies a volume of 100. L at a particular temperature and pressure, what volume will 5.00 g of oxygen gas occupy under the same conditions (remember oxygen gas is diatomic )? 18. Ideal gas law. Given each of the following sets of values for an ideal gas, calculate the unknown quantity. a. P = mm Hg; V = 644 ml; n = mol; T = 303 K b. P = 745 mm Hg; V = 11.2 L; n = mol; T = K 19. What volume is occupied by 5.03 g of O2 at 28 o C and a pressure of atm? 20. At what temperature Celsius does 16.3 g of nitrogen gas have a pressure of 1.25 atm in a 25.0 L tank? 10

11 In Class Work Campbell Chemistry 21. What is the pressure in atm if 25.0 g of He gas at 100 o C is in a 2500ml tank? 22. How many grams of carbon dioxide (CO2) are in a 2.00 liter container when the gas is under a pressure of 2.45 atm at C? In Class Notes 2 Practice: Gas stoichiometry 23. Given the following reaction: CH4(g) + O2(g) CO2(g) + H2O(g) How many grams of carbon dioxide are produced if 35.5 L of oxygen at C and 745 mmhg react with excess methane? 24. If 2.5 L of N2 react with excess H2, how many liters of NH3 are produced under the same conditions? N2(g) + H2(g) NH3(g) 25. How many grams of O2 are needed to completely react with 4.5 L of H2 at 1250 mmhg and C? H2(g) + O2(g) H2O(g) 26. If 1.25 L of O2 reacts with excess SO2, how many liters of SO3 are produced under the same conditions? SO2(g) + O2(g) SO3(g) 27. If 2.25 g of solid Ca(ClO3)2 decompose to give CaCl2 and O2, how many liters of O2 gas will be produced at C and 835 mmhg? (write and balance the chemical reaction first) 11

12 In Class Work Campbell Chemistry Nomenclature Review: Name or write the formula for the following polyatomic ions: Formula SO 4-2 NO 2-1 CO 3-2 HCO 3-1 ClO 3-1 OH -1 NH 4 +1 Name sulfite nitrate chlorite phosphate acetate Provide the formula for the following: 1. calcium phosphide 6. hydrobromic acid 2. aluminum hydroxide 7. carbonic acid 3. magnesium acetate 8. nitrous acid 4. tin (II) chlorite 9. trinitrogen heptasulfide 5. iron (III) sulfide 10. tetracarbon hexaselenide Provide the name for the following: 1. Li3N 6. H2S 2. (NH4)2CO3 7. H3PO4 3. Ba(NO2)2 8. H2SO3 4. Cu2O 9. OCl9 5. Pb(OH)4 10. CO 12

13 In Class Work Campbell Chemistry 9a K 9b C 9c K 9d mmhg 9e atm 9f L 10 a. 590 mmhg 10 b atm or 950 mmhg 11 a. V= 309 ml 11 b. V =.257 L 11 c. P = 42,560 mmhg 12 a. T = C 12 b. T = 35 0 C 12 c. V = 298 ml 13 a. V = 1965 ml 13 b. P = 4428 mmhg 13 c. T = C atm C ml 17 a L 17 b a P = 2703 mm Hg 18 b. T = 333 K L o C atm g CO g CO L g O L L Answers to nomenclature review: Formula SO4-2 SO3-2 NO3-1 NO2-1 CO3-2 HCO3-1 ClO3-1 ClO2-1 PO4-3 C2H3O2-1 OH -1 NH4 +1 Name sulfate sulfite nitrate nitrite carbonate bicarbonate chlorate chlorite phosphate acetate hydroxide ammonium Provide the formula for the following: 1. calcium phosphide Ca3P2 2. aluminum hydroxide Al(OH)3 3. magnesium acetate Mg(C2H3O2)2 4. tin (II) chlorite Sn(ClO2)2 5. iron (III) sulfide FeS 6. hydrobromic acid HBr 7. carbonic acid H2CO3 8. nitrous acid HNO2 9. trinitrogen heptasulfide N3S7 10. tetracarbon hexaselenide C4Se6 Provide the name for the following: 1. Li3N 2. (NH4)2CO3 3. Ba(NO2)2 Lithium nitride Ammonium carbonate Barium nitrite 4. Cu2O Copper (I) Oxide 5. Pb(OH)4 Lead (IV) hydroxide 6. H2S Hydrosulfuric acid 7. H3PO4 Phosphoric acid 8. H2SO3 Sulfurous acid 9. OCl9 Oxygen nonachloride 10. CO Carbon monoxide 13

14 Video 1 Turn in Sheet Name: Due 1/7 (Thursday) Scenarios from the video; for each scenario shown in the video explain what property it represents and how it demonstrates one of the assumptions of the kinetic molecular theory (there maybe more than one correct answer) Answer the following questions based on the video and hand in when you come to class on Thursday. 1. At the start of the video I gave some examples of monoatomic, diatomic and polyatomic gases, but there are many others. Give some others that you know of (or find on the internet!) 2. Explain the effect of pressure in terms of the kinetic molecular theory (how is pressure created?) 3. A gas in an expandable container is heated. Explain what happens in terms of the kinetic molecular theory. 14

15 Video 2 Turn in Sheet Due 1/11 (Monday) Name: Answer the following questions based on the video and hand in when you come to class on Monday. 1. Use each of the terms below to complete the passage. Each term may be used more than once. Pressure Temperature Volume a. Boyle s law relates and if and amount of gas are held constant. b. Charles s law relates and if and amount of gas are held constant. c. Gay-Lussac s law relates and if and amount of gas are held constant. 2. According to Boyle s Law: a. if you decrease volume what should happen to pressure? b. Is this a direct or inverse relationship? c. Give a real life example of this relationship. 3. According the Charles Law: a. if you decrease temperature what should happen to volume? b. Is this a direct or inverse relationship? c. Give a real life example of this relationship. 4. Fill in the following table with one of these terms: increases, decreases, stays the same. Each term may be used more than once. Assume the amount of gas is constant. Volume Pressure Temperature Increases Stays the same Increases Stays the same Increases Stays the same Stays the same Increases Stays the same Increases Decreases Stays the same 15

16 Video 3 Turn in Sheet Name: Due 1/13 (Wednesday) Answer the following questions based on the video and hand in when you come to class on Wednesday. 1. What is Avogadro s Principle and what does it tell us about gases? 2. Explain what happens when you add more moles of gas to a. An expandable container, like a balloon? b. A non-expandable container, like a metal air tank? 3. What Gas Laws have you learned about so far are demonstrated by the two examples above? a. b. 4. Why did I say that the Ideal Gas Law combines all of the individual gas laws? 5. Given the following data, use the Ideal Gas Law to calculate the volume of the gas: P = 1.25 atm; V = ; n = mol; T = 27 o C 6. In one of the slides there was a caricature of a man pointing at something. What was he pointing at? 16