Marchand. VOCABULARY: Ideal gas standard atmospheric pressure standard temperature STP diffusion effusion molar volume
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1 Honors Chemistry Unit 11 Chapters 10 & 11 Gases, Gas Laws, and Gas Stoichiometry Vocabulary Due: Thurs Marchand. Quiz: Test Date: VOCABULARY: Ideal gas standard atmospheric pressure standard temperature STP diffusion effusion molar volume CONSTANTS/FORMULAS: Boyle s law Charles law GayLussac s law Combined gas law Dalton s law Graham s law Ideal gas law Molar volume Molecular Mass Determination (of a gas) Unit 11 Packet Page 1 of 14 Tues, Marat Tues.Marchk1 Bdrwimhfhwm Cans! 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, GayLussac 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 Latm/molK. Be able to do problems involving gas stoichiometry (at STP and other conditions).
2 Unit 11 BELLWORK SET Gases, Gas Laws, and Gas Stoichiometry Unit 11 Packet Page 2 of 14 Review: 1. Draw the dot diagram for Bismuth. 2. Draw the Lewis Structure for the following and identify the VSEPR Shape: A. Carbonate ion B. silicon disulfide Current Unit Material 3. A sample of diborane gas (B2H6) a substance that bursts into flame when exposed to air, has a pressure of 345 torr at a temperature of 15 0 C and a volume of 3.48 L. If conditions are changed so that the temperature is 36 0 C 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 47 0 C and found to be 1.95 g/l. Calculate the molar mass of the gas. 5. Mixtures of helium and oxygen are used in scuba diving tanks to help prevent the bend. For a particular dive, 46 L of O2 at 25 0 C and 1.0 atm and 12 L He at 25 0 C and 1.0 atm were pumped into a tank with a volume of 5.0 L. Calculate the partial pressure of each gas and the total pressure in the tank at 25 0 C. 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 0 C and 789 torr, required for the complete combustion of 45 g of octane (C8H18).
3 Unit 11 Gas Laws Notes Gases: 4 measurable quantities: Unit 11 Packet Page 3 of 14 Volume 1 ml = 1 cm 3 Pressure Temperature # of moles Variables? STP? V Standard Temp **GAS LAWS Must be Memorized!!**! 0 C Boyle s law P1 V1 = P2 V2 (V varies inversely with P) Graph of P vs V? inversely? P k 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 will the volume be if the pressure is increased to 750 mm Hg?? TE (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? on.tw#m5ooimmd='44md tuff VPTT Vbtb Example: A helium filled balloon has a volume of 2.75 L at C. The volume of the balloon decreases to 2.46 L after it was placed outside on a cold day. What is the outside temperature? Tz It? I VI VFQ.75L V+ =V= You try: A sample of neon occupies a volume of 752 ml at 25 0 C. What volume will the gas occupy T±@g3pI at C? (Answer: 815 ml) =Vyq k=v jh=752mdga3# 298k T ; stdpressurettaotmmm P4Vb Pby N '\Mr3Kpa =p # Pet.2aimPNi=Rk PIyIPY u Pity t.am#@.l=o.24atmiv,=1.0lvz=5r0l Be 720mm RVFPZVZ Y IEmohm T,= =29312 hippy V Tz V, tkmfz.tk?5k#=262@@z3a3k Vz= 2.46L V, #Vsti 815.1C Pz
4 Unit 11 Packet Page 4 of 14 GayLussac s Law: P1/T1 = P2/T2 (P varies directly with Kelvin Temperature) Like which other law? Charles Law P PTTP Pb± You Try: Before a trip from Raleigh to NY, the pressure in a tire is 1.8 atm at 20 0 C. At the end of the trip the pressure gauge reads 1444 mm Hg. What is the new temperature in the tire? tf " =tfzp 2e t.ca#d@3k)1z=1444mm*e=l.gatm ( 1. 8am ) Yodtmarraak Tz=? (Answer: 309 K (or 36 0 C)) Combined Gas Law: P1V1 = P2V2 T must be in K!!! 309,3*4=282 T1 T2 Example: If ml of a gas at 25 0 C and 1.3 atm is cooled to C and 780 mm Hg. What is the new volume?. 4mL VE? R =RV= VERVE 273=29312 Tz RT, Te25t273=298KT 2Ot P,=h3atm ebay.tl?wmyydfyy#=1.03atnpttpztu Remanded PNFEEVQI 350.4C You try: a 700. ml gas sample at STP is compressed to a volume of 200. ml, and the temperature is increased to C. What is the new pressure = of the gas in kpa? mdbo3k)t RYyd=RV= md 2 =3q3h@ (Answer: 394 kpa)
5 Unit 11 Packet Page 5 of 14 Dalton s law of Partial Pressures: pressure of each gas in a mixture is called the partial pressure of that gas. Total Pressure = sum of partial pressures PT = P1 + P2 + P3. etc. Special case: gases collected by water displacement see diagram on board! Use formula PT = Patm = Pg + PH2O Total atmosphere gas water Patm from lab or is given: PH2O = Table page 899 o Bluebook ) Example: Oxygen is collected by water displacement. The barometric pressure and temperature are 84.5 kpa and C. What is the partial pressure of O2? Palm =.tt?hotpozpoz=patm Pao Pµzo@ 20.8C =234KR = 84.51Pa 2.341Pa 82.21Pa You try: A gas is collected over water and the atmospheric pressure is kpa at 50 C. What is the partial pressure of the gas? Palm.tl?tzotPg;Pg=PatmPtw=1O1.1KPa12.34KPa=88.7bKPa (Answer: 88.8 kpa) Graham s Law Review: Effusion? Diffusion? **Rate of effusion and diffusion varies inversely with the mass of the gas.** Rate of gas A = Square Root Mass of gas B Rate of gas B Mass = of gas A Hzgaseffuses pthan 3.98 xfaster Example: Compare the rates of effusion of Hydrogen and oxygen at STP. rate of Hz 02 Ito.fm#Eh=FI=F.84=3.98 You try: Compare the rates of effusion of Fluorine and chlorine (Answer: Fluorine is 1.4 x faster than chlorine)
6 Examples of Dalton's Law ; :* " w?itii! ± : DEF 7dm + Water Displacement IIIe.ee#:.:IiItiiI : gas molecules Pitzo + Pg = Palm
7 ' Ideal Gas Law Notes Depends on Mass of Unit 11 Packet Page 6 of 14!! Keywords : gas (amounts. PV = nrt mass,md, g. Must paged use the following units with the ideal gas law! amount P = atm V = L T = K n = moles ) always! nlmustconuert R = gas constant Latm/mol K (memorize) p? Example: What is the pressure exerted by a 12.0 g sample of Nitrogen gas (N2) in a 10.0 L container at 25 0 C?. p=? P=1O5atmf 12=00821 toatmlmokk (0,43mg.( L p=nri F =29812 Practice Ideal Gas Law Worksheet: 1 4 (page 12 in packet) t.mg?d)(2q8k)n=12.0gnz#ghg=o.43mo1pv=nrtvelo.0l * Gas Stoichiometry a Molar Volume 1 mol of any gas at STP has a volume of 22.4 L f) 1 mol = conversion factor (only to be used at STP) 22.4 L 1. Example: What is the mass of 98.0 ml of sulfur dioxide at STP? (work together on board copy into your notes!) You try: What is the mass of 1.33 x 10 4 ml of O2 at STP? p@ Note :2Y4moI. canalsobewsed,?l 502 or canusemdarvolume! 1j3L t.gsoa98.my#.&4xq=o.28gs0z Gas Density: D =? FEFe=F At STP : D = Molar mass g/mol (PT) #=@ Molar volume 22.4 L/mol L Ex: What is the density of CO2 at STP? Dq= Mdarmasscoz Inyo #, = The 1.964, You try: What is the molar mass of a gas with a density of 1.56 g/l? D= MY ; gOz T.to#mM=34..9mEo,
8 Unit 11 Packet Page 7 of 14 Molecular Mass Determination from Ideal Gas Law: (see derivation on board) D = PM density = pressure (atm) x molar mass (PT)/ constant x temp (K) RT Examples & practice on ideal gas law worksheet! 35L Stoichiometry of Gases Can do LL conversions (just like molmol) with 2 gases and an equation Oz. Example: 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!** 0.35LHspI0wel.75L@7.g 5.0L 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? n wmonwwrsveaume 5.at?#HdH09I3Ij=22.34gCa03J2LiCls2LitqLz You try: If 10.0 g of lithium chloride decomposes how many liters of Cl2 gas are produced at STP? (write a balanced equation first!) 10.0g Example 3: How many liters of H2 at 35 o C and 745 mm Hg are need to react completely with 825 g of WO3? PV=nRT WO3(s) + FL 3H2 (g) à W(s) + 3H2O (l) D7.moIHe825sW03MgygM3Etgg10.68mdHz@usePVEnnaRTytovnrpI.io.68molK00o8.2gkahtamdG08Kf.gE2n5.5ITL.mo1co65o5gYwkq5.n You try: How many L of CO at 27 0 C 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,5yye rf#i45mp0jg8afmftkd cg
9 be GET = = gdtfptm2t@0pnriuremne.m p= TFRI DRNI P= DR_µT solve for D : PM = DRT Phd
10 Unit 11 Packet Page 8 of 14 GAS LAW PROBLEMS Work 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 same gas 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 ml. What will the volume of 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 22.5 ml? 4. A gas occupies a volume of 40.8 ml at a temperature of 33.5 C. At what temperature will the volume 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 and pressure. 7. A gas at a temperature of 67.5 C and a pressure of 882 torr occupies a volume of ml. What will the volume of the gas be at 840 torr and 80.0 C? 8. A gas with a volume of ml at a pressure of atm is subjected to a pressure of atm. What is its volume at the new pressure? 9. Hydrogen gas is collected over water and the atmospheric pressure in 122kPa at 50 C. What is the partial pressure of hydrogen? Ideal Gas Law Practice Remember: PV = nrt and D = PM/RT Must use atm, L, moles and K R =.0821 Latm/molK 1. How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 25 0 C? 2. What volume will 2.0 moles of nitrogen occupy at 720 torr and C? 50,8L 0.12mA 3. What pressure will be exerted by 25 g of CO2 at a temperature of 25 0 C and a volume of 500. ml? 27,8ohm 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 C? 0.739k * 6. If the density of a gas is 1.2 g/l at 745 torr and C, what is its molecular mass? 29.5ft 7. How many moles of nitrogen gas will occupy a volume of 347 ml at 6680 torr and 27 0 C? * 8. What volume will 454 grams of hydrogen occupy at 1.05 atm and 25 0 C? (remember hydrogen is diatomic!) 9. Find the number of grams of CO2 that exerts a pressure of 785 torrs at a volume 32.5 L and a temperature of 32 0 C. 10. An elemental gas has a mass of 10.3 g. If the volume is 58.4 L and the pressure is 758 torr at a temperature of C, what is the gas (Hint find the molar mass!) D=PnPf ;na f*)( 0.082k axm 75%6, = =4 0smt,;ThedementisHe 154k
11 STOICHIOMETRY WORKSHEET Unit 11 Packet Page 9 of 14 Work the following stoichiometry problems in the space provided. 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 are produced? HINT: grams ßà moles ßà mole ratio ßà moles ßà grams 3. 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 of magnesium chloride. 5. Balance the following equation: Cu + HNO3 à Cu(NO3)2 + H2 6. 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 gas at a pressure of 1.2 atm, a temperature of 301 K and 2.00 moles. Gas Stoichiometry Worksheet 1. 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 oxygen according to the following equation: 2 C (s) + O2 (g) à 2 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 of KClO3 decomposes according to the following equation? BALANCE THE EQ FIRST! KClO3 à KCl + O2 8. What is the mass of 1258 ml of hydrogen gas at STP?
12 Mini Lab CARTESIAN DIVER Work 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. Unit 11 Packet Page 10 of 14 Materials (per table) 1 empty plastic 2 Liter bottle tap water 1 dropper Procedure: 1. Fill the 2Liter up with water until it overflows; it must be completely full. 2. Fill dropper about ½ to 2/3 full of tap water. 3. Place the dropper gently into the bottle; try not to displace too much water. 4. Screw cap back on tightly. Do NOT tip bottle upside down any time during the lab. 5. Squeeze the middle of the bottle with as much force as possible. 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? 3. What gas law does the Cartesian diver demonstrate? Minilab 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 plunger without 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 the syringe and press down on the plunger. QUESTION # 2 What happened? Use chemistry ideas in your explanation. 6. Replace with a fresh marshmallow when necessary.
13 Unit 11 Packet Page 11 of 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 1.3 ml 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? MINI LAB THE COLLAPSING SOFT DRINK CAN Do this lab as a group the whole table will work together. Answer the questions. Procedure: 1. Place about 5 ml of water in an empty aluminum soft drink can. (Be sure the can is clean first. 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 beaker containing about 1 2 inches of water a few ice cubes. Your teacher will demonstrate how this 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.
14 Unit 11 Packet Page 12 of 14 Unit 11 Gases, Gas Laws, & Gas Stoichiometry STUDY GUIDE REVIEW INFORMATION TO BE MEMORIZED/Used: As practice; write the formulas without your notes! Charles Law Boyle s Law GayLussac s Law Combined gas law Dalton s law Graham s law Ideal gas law R = Molar volume at STP STP = Density at STP and Density NOT at STP Molar Mass from the Ideal Gas Law PRACTICE 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 88.3 kpa 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 the volume 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 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 reacting with an excess amount of hydrochloric acid? 9. What volume of fluorine gas is required to react with 2.67 g of calcium bromide to form calcium 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: ml kpa ml 4. O C (273 K) L atm K L H ml 10. CH4
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