Packet 04 - Gasses

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Temple University *

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1032

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Chemistry

Date

Feb 20, 2024

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pdf

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Uploaded by ConstableTarsierMaster834

CHEM 1032, General Chemistry Recitation Packets Series, 2020 Packet 04 - Gasses Part 1: Prior knowledge needed to approach this topic. The following is a list of concepts you should have already mastered. It will be very hard for you to learn today’s topics and skills without it. If you are unfamiliar with any of the following, place a sign next to it and/or ask for help reviewing it. o Unit conversion (such as the factor-label method) o Stoichiometry o The mole and molar mass o Definition of pressure and force (from physics… P=F/A[area] and F=ma[acceleration]) Part 2: concepts from video/book. The following concepts should be somewhat familiar to you from watching the pre-lecture video and completing the assigned readings. If you are unfamiliar with any of the following, place a sign next to it and/or ask for help reviewing it. o Definition of pressure (mathematically and experimentally) o Units of pressure (atm, torr, mmHg, bars, Pa, psi) o Boyle’s Law (PV=PV) o Charle’s Law (V/T=V/T) o Avogadro’s Law (V/n=V/n) o Ideal Gas Law (PV=nRT) o Definition of ideal gas o R=gas constant: VALUE CHANGES WITH UNITS OF OTHER VARIABLES o STP and SATP (STP: T=273 K, P=1 bar; SATP: T=298 K, P=1 atm) o Molar volume (at TSP, V=22.4 L) o Dalton’s law of partial pressure. o Use ideal gas law to compute gas densities and molar masses. o Perform stoichiometric calculations involving gaseous substances. Part 3: activities of the day. The following activities are designed to help you master the concepts, apply it to problem solving and evaluating critical the results. You are encouraged to carry them out in groups and to ask questions to any of us at any time. A blank piece of paper can be intimidating; just try... it will slowly begin making sense!

CHEM 1032, General Chemistry Recitation Packets Series, 2020 Activity 1: proportionality relationships. Answer the following multiple-choice questions, basing your reasoning on the equation PV=nRT. a. If the absolute temperature of a gas is increased by a factor of two and the volume is increased by a factor of two, the pressure of the gas will: • increase by a factor of 4 • increase by a factor of 2 • stay the same • decrease by a factor of 2 • decrease by a factor of 4 b. If the absolute temperature of a gas is increased by a factor of two and the volume is reduced by a factor of two, the pressure of the gas will: • increase by a factor of 4 • increase by a factor of 2 • stay the same • decrease by a factor of 2 • decrease by a factor of 4 c. If the absolute temperature of a gas is doubled and the volume stays the same, the pressure of the gas will: • increase by a factor of 4 • increase by a factor of 2 • stay the same • decrease by a factor of 2 • decrease by a factor of 4

CHEM 1031/32, General Chemistry Worksheet Series, 2017 Page 3 of 5 Activity 2: ideal gas law. 1) If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 2) If I have an unknown quantity of gas at a pressure of 121.6 kPa, a volume of 31 liters, and a temperature of 87 0 C, how many moles of gas do I have? 3) If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container? 4) If I have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0 C, what is the volume of the container that the gas is in? 5) If I have 17 moles of gas at a temperature of 67 0 C, and a volume of 88.89 liters, what is the pressure of the gas? 6) If I have an unknown quantity of gas at a pressure of 50.65 kPa, a volume of 25 liters, and a temperature of 300 K, how many moles of gas do I have? 7) If I have 21 moles of gas held at a pressure of 7901kPa and a temperature of 900 K, what is the volume of the gas? 8) If I have 1.9 moles of gas held at a pressure of 5 atm and in a container with a volume of 50 liters, what is the temperature of the gas? 9) If I have 2.4 moles of gas held at a temperature of 97 0 C and in a container with a volume of 45 liters, what is the pressure of the gas? 10) If I have an unknown quantity of gas held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many moles of gas do I have? T = PV / nR T = (5.6 atm)(12 L) / (4 moles)(0.082 L•atm/mol•K) = 205 K n = PV / RT n = ( 121.6 kPa )( 31 L) / ( 8.31 L• kPa /mol•K) (360 K) = 1.26 moles P = nRT / V P = ( 3 moles )( 0.082 L•atm/mol•K ) (400 K) / ( 60 L ) = 1.64 atm V = nRT / P V = ( 7.7 moles )( 0.082 L•atm/mol•K ) ( 329 K) / ( 0.09 atm ) = 2380 L P = nRT / V P = ( 17 moles )( 0.082 L•atm/mol•K ) ( 340 K) / ( 88.89 L ) = 5.33 atm n = PV / RT n = ( 50.65 kPa)(25 L) / (8.31 L•kPa/mol•K)(300K) = 0.508 moles V = nRT / P V = ( 21 moles)(8.31 L•kPa/mol•K)(900K) / (7901 kPa) = 19.9 L T = PV / nR T = ( 5 atm)(50 L) / (1.9 moles)(0.082 L•atm/mol•K) = 1605 K P = nRT / V P = ( 2.4 moles )(0.082 L•atm/mol•K) (370 K) / (45 L) = 1.62 atm n = PV / RT n = (560 atm ) (25 L) / (0.082 L•atm/mol•K) (1195 K) = 143 moles

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CHEM 1031/32, General Chemistry Worksheet Series, 2017 Page 4 of 5 Activity 3: applications of the ideal gas law. A sealed, rigid container holds pure argon at 3000.0 torr and 300.0 o C. What will the pressure be if the container is cooled to 30.0 o C? (6 pts.) 2. What is the density of krypton gas at STP? (6 pts.) 3. 1.32 mmol of an ideal gas are expanded at the constant temperature of 298K. a. Calculate the Volume the gas will occupy at the pressures provided in the table below. Pressure (atm) Volume (L) density (g/L) (Ref. 5c) 1 0.5 0.1 0.05 0.01 0.005 b. Plot the data in a (x,y) = (V,P) set of Cartesian coordinates. T 1 = 300.0 °C = 573.15 K T 2 = 30.0 °C = 303.15K P 1 / T 1 = P 2 / T 2 ... P 2 = P 1 T 2 / T 1 ... plug in the corresponding values P 2 = (3000.0 torr)(303.15K) / (573.15K) = 1587 torr D = (molar mass)(P) / RT ... plug in the corresponding values D = (83.80 g/mol)(1 atm) / (0.082 L•atm/mol•K)(273.15K) = 3.719 g/L 32.35 64.50 322.5 645.0 3225.0 6450.0 3.44 1.72 0.344 0.172 0. 0344 0. 0172 1 0.5 0.1 3200 6400 640 320 64 32

CHEM 1031/32, General Chemistry Worksheet Series, 2017 Page 5 of 5 c. In the table in part a, calculate the density at each pressure, knowing that the molar mass is 84. d. Plot the data in a (x,y) = (d,P) set of Cartesian coordinates. 4. A gas has the following elemental composition: C = 82.7%; H = 17.3% in mass. At stp (room temperature, 0°C, and pressure, 760 mmHg), its density is 2.496 Kg/m 3 . Assuming that this gas behaves ideally, what’s it’s molecular formula? 5. Question: 0.50 moles of H 2 gas and 0.5 moles of O 2 gas are introduced in a 1.0-L vessel at 100 o C and they are reacted to produce water with a 100% yield. What is the total pressure in the container at the beginning of the reaction? What is the total pressure in the container at the end of the reaction? C = 82.7 g = 6.89 mol H = 17.3 g = 17.3 mol ratio = 1:2.5 empirical formula = C 2 H 5 ... molecular formula = C 4 H 10 molar mass = 2.496 g/L • [(0.082 L•atm/K•mol)(273.15K)] / [1 atm] = 56 g/mol 1 2 3 0. 5 1 0.1 PV = nRT ... P = nRT / V P 2H2 = [(1.00 moles)(0.082L•atm/K•mol)(273.15K)] / [1.0 L] = 22 atm P O2 = [(0.50 moles)(0.082L•atm/K•mol)(273.15K)] / [1.0 L] = 11 atm ... total pressure is 33 atm at the beginning of the reaction PV = nRT ... P = nRT / V P 2H20 = [(2.00 moles)(0.082L•atm/K•mol)(273.15K)] / [1.0 L] = 44 atm ... total pressure is 44 atm at the end of the reaction

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