Name Period Date. Lab 5: The Molar Volume of a Gas
|
|
- Nelson Rogers
- 6 years ago
- Views:
Transcription
1 Name Period Date Lab 5: The Molar Volume of a Gas Objective: To determine the actual molar volume of oxyen as To determine an experimental value for the universal as constant Introduction To calculate the molar volume of a as, you must create a as and determine the volume and number of moles of as created. To do this, you will be heatin a mixture of potassium chlorate and mananese dioxide (a catalyst). Catalysts are substances which increase the rate of a reaction but are not used up by the reaction. Mananese dioxide functions by lowerin the temperature required to decompose the potassium chlorate. When heated to a temperature between 80 and 400 C all of the potassium chlorate is decomposed to potassium chloride and oxyen as. The only reaction that will occur under the conditions of the reaction is the followin: 2 KClO (s) 2 KCl (s) + O 2 () The oxyen formed will be collected as a as. The mananese dioxide and potassium chloride formed durin the reaction will remain in the test tube. Notice that the stoichiometric ratio of potassium chlorate to potassium chloride is one to one. Therefore the difference in weiht between the potassium chlorate and the resultin potassium chloride must all be due to the oxyen. Therefore, the loss in mass of the mixture in the test tube durin the reaction should equal the mass of oxyen collected. From the mass of the oxyen as produced, the number of moles of oxyen as can be calculated. The atmospheric pressure (total pressure in the jar) can be determined usin a barometer but the pressure of the dry oxyen as must be calculated usin Dalton s Law of Partial Pressure. The pressure of water vapor at the temperature at which the water is can be determined from a chart. The volume of as produced is equal to the amount of water that was displaced and pushed throuh the rubber tubin into the beaker by the end of the experiment. To be able to compare our experimental value to the standard molar volume (22.4 L/mol), we must determine the molar volume at STP (0 C, 1atm). We can use the combined as law to find the volume the sample of oxyen as created would have at STP. Be sure to use the pressure of the dry oxyen as (not atmospheric pressure) as your oriinal pressure. From the volume at STP and moles of oxyen as, the molar volume can be calculated: From the pressure of dry oxyen as, moles of as created, volume of as collected, and temperature of the water, the universal as constant, R will be calculated. Usin the Ideal Gas Law: 1
2 Materials potassium chlorate, KClO (s) mananese (IV) oxide, MnO 2(s) rin stand utility clamp lare test tube lass jar 250-mL beaker 100-mL raduated cylinder Bunsen burner Glass elbows, 2 Glass tubin, straiht pieces, 2 Rubber tubin, 2 analytical balance Rubber stoppers, 2 LabQuest Temperature sensor Gas pressure sensor Straw pieces Safety Concerns Potassium chlorate is a powerful oxidizin aent and reacts readily with easily oxidized substances such as rease or rubber. Careless handlin of it could conceivably result in a fire. Safety lasses and aprons should be worn at all times. Procedure 1. Preparation a. Set up the apparatus as shown in the fiure below except for the test tube with its rubber stopper. The lon lass tubin in the lass jar should extend almost to the bottom of the flask. Fill the jar with water and add approximately 100 ml of water to the beaker. b. Displace the air in the rubber tubin that leads to the beaker by steadily blowin into the rubber tubin, which will be connected to the test tube. Cut straws are supplied so that you need not put your mouth directly to the tubin. Remove any remainin air bubbles in the rubber tubin that leads to the beaker by raisin or lowerin the beaker. Finish with the lass jar nearly filled with water (one inch below the rubber stopper) and then place a clamp on the rubber hose that leads to the beaker. c. Find the exact mass of your empty, dry test tube. Record it in your data table. d. Weih out approximately 0. rams of KClO. Be sure that there are no lumps in it. Usin the waxed weihin paper, pour this into the test tube, bein 2
3 careful to not allow any particles to stick to the side near the top of the test tube. Record the exact mass in your data table. e. Next, weih out approximately 0.02 rams of MnO 2. Add this in the same manner to the test tube. Mix the KClO and the MnO 2 toether by swirlin the test tube ently. f. Attach the test tube to the remainder of the assembly. Incline the test tube upward at an anle of about 0 o.. Equalize the pressure inside the lass jar with the atmospheric pressure as follows: With the clamp open raise the beaker until the water level in the beaker is the same as that in the lass jar. Durin this process, do not allow the tubin in the beaker to come above the water level (or air will et into the system). Close the clamp on the tubin aain. Empty the beaker of any water and dry it. h. Place the beaker back on the desk and open the clamp. If there are no leaks in your setup, a small amount of water may flow into the beaker but it should stop quickly. Leave this water in the beaker- it will flow back into the jar at the end of the experiment when the pressure is equalized aain. If a leak is present check the connections until you have found and corrected the leak. 2. Create the Oxyen Gas a. Open the pinch clamp. Leave in the beaker any water that may flow. Heat the test tube startin at the top of the salt mixture and workin downward, at a rate that ives a moderate, steady rate of evolution of oxyen without propellin the mixture up the test tube toward the rubber stopper. b. Once the reaction has started and water beins to flow make sure that Tube F stays under water in the jar or air will et into the system and cause the calculated volume of as to be wron. Continue heatin for 15 minutes. c. Allow the apparatus to cool to room temperature.. Measurements concernin the Gas a. Measure the barometric pressure usin pressure sensor and record it in your data table. b. When the apparatus is cool to the touch (which will require several minutes) equalize the pressure aain (see #1) and then close the pinch clam. c. Remove the test tube from the apparatus and find the mass of it. Record the exact mass on your data table. d. Remove the stopper from the lass jar, insert the temperature sensor into the water inside, and leave for a few minutes. Record the temperature (as the temperature of the as). e. Look up the vapor pressure of water at this temperature in the Table iven and record it in your data table. f. Measure the volume of water in Beaker by pourin it into a raduated cylinder. Read the volume to the nearest tenth and record in your data table. This is equal to the volume of oxyen as that was created. 4. Disposal: Dispose of the residue in the test tube by washin it down the sink with lots of water. 5. Repeat the collection: Repeat Steps 1-4 to collect a second sample of as.
4 Data/Results: Mass of empty test tube Run 1 Run 2 Mass of the KClO Mass of the MnO 2 Calculate mass of test tube and KClO /MnO 2 Mass of test tube and residue after heatin Calculated mass of O 2 liberated Volume of H 2 O in beaker (Volume of oxyen created) ml ml Temperature of H 2 O in jar K K Barometric pressure mmh mmh Vapor pressure of water mmh mmh Calculated pressure of dry O 2 as mmh mmh Calculations: For each of the calculations below, show all steps of your work clearly. Be sure to follow all rules concernin sinificant fiures and roundin. 1. From the mass of the oxyen as collected, calculate the number of moles of oxyen as collected. 2. From the volume, temperature (in Kelvin) and pressure (of dry oxyen as) of the collected as, calculate the volume the oxyen as would have at STP usin the combined as law. 4
5 . Usin the number of moles of as and the volume of that as at STP, calculate the molar volume of oxyen as. Averae: 4. Calculate the percent error in the averae of your two molar volume values and the Standard Molar Volume for an ideal as. 5. Usin the pressure (of dry oxyen as), volume, number of moles, and temperature of the collected as, calculate the ideal as law constant, R. Be sure to use the correct units to end up with an R in L. atm/mol. K. Averae: 6. Calculate the percent error in the averae of your two R values and the value of R used commonly. 7. Students performin this lab have made several mistakes in the past. How would each of these oversihts affect the calculated molar volume of as? a. Forot to empty and dry out the beaker after settin up the equipment, removin air from the lines, and equalizin the pressure. b. Forot to mix the potassium chlorate and mananese dioxide toether before heatin. 5
Analysis of a KClO3 Mixture and Determination of R
Experiment 10 Analysis of a KClO3 Mixture and Determination of R Pre-Lab Assignment Before coming to lab: Read the lab thoroughly. Answer the pre-lab questions that appear at the end of this lab exercise.
More informationThe Decomposition of Potassium Chlorate
The Decomposition of Potassium Chlorate Small quantities of molecular oxygen (O 2 ) can be obtained from the thermal decomposition of certain oxides, peroxides, and salts of oxoacids. Some examples of
More informationDetermination of R: The Gas-Law Constant
Determination of R: The Gas-Law Constant PURPOSE: EXPERIMENT 9 To gain a feeling for how well real gases obey the ideal-gas law and to determine the ideal-gas-law constant R. APPARATUS AND CHEMICALS: KClO
More informationPearson Education Limited Edinburgh Gate Harlow Essex CM20 2JE England and Associated Companies throughout the world
Pearson Education Limited Edinburgh Gate Harlow Essex CM20 2JE England and Associated Companies throughout the world Visit us on the World Wide Web at: www.pearsoned.co.uk Pearson Education Limited 2014
More informationTHE DECOMPOSITION OF POTASSIUM CHLORATE This lab is derived almost entirely from a lab used at the United States Naval Academy
THE DECOMPOSITION OF POTASSIUM CHLORATE This lab is derived almost entirely from a lab used at the United States Naval Academy PURPOSE: The purpose of this experiment is to study the decomposition of potassium
More informationExperiment 12: MOLAR VOLUME OF AN IDEAL GAS
Experiment 1: MOLAR VOLUME OF AN IDEAL GAS Purpose: Determine the molar volume of a gas at standard temperature and pressure (STP, 0 C and pressure of 1 atm) Performance Goals: Collect and measure the
More informationThe Determination of the Value for Molar Volume
Name AP Chemistry The Determination of the Value for Molar Volume Objective Using a chemical reaction that produces a gas, measure the appropriate values to allow a determination of the value for molar
More informationExperiment 13 Molar Mass of a Gas. Purpose. Background. PV = nrt
Experiment 13 Molar Mass of a Gas Purpose In this experiment you will use the ideal gas law to calculate the molar mass of a volatile liquid compound by measuring the mass, volume, temperature, and pressure
More informationHow is pressure handled when we have a mixture of gases?
Name Chem 161, Section: Group Number: ALE 23. Mixtures of Gases (Reference: Chapter 5 in Silberberg 5 th edition) How is pressure handled when we have a mixture of gases? The Model: Collecting Gas Over
More informationThe Determination of the Value for Molar Volume
Objective The Determination of the Value for Molar Volume Using a chemical reaction that produces a gas, measure the appropriate values to allow a determination of the value for molar volume. Brief Overview
More informationQuestion McGraw-Hill Ryerson Limited
Question 1 Which of the following cannot be explained by considering the empty space between the particles of a gas? A) Gases are more compressible than liquids. B) Gases have lower viscosities than liquids.
More informationPRE LABORATORY ASSIGNMENT: Lab Section Score: /10 READ THE LAB TEXT BEFORE ATTEMPTING THESE PROBLEMS!
EXPERIMENT # 6 Name: PRE LABORATORY ASSIGNMENT: Lab Section Score: /10 READ THE LAB TEXT BEFORE ATTEMPTING THESE PROBLEMS! 1. Calculate the height of a corresponding column of mercury (in mm) that is at
More information1. If grams of the vapor of a volatile liquid can fill a 498 ml flask at o C and 775 mm Hg, what is the molecular mass of the gas?
MOLECULAR MASS OFA VOLATILE LIQUID A lab to study the ideal gas law Introduction The ideal gas law indicates that the observed properties of a gas sample are directly related to the number of moles of
More informationGeneral Chemistry I Percent Yield of Hydrogen Gas From Magnesium and HCl
Introduction For chemical reactions involving gases, gas volume measurements provide a convenient means of determining stoichiometric relationships. A gaseous product is collected in a long, thin graduated
More informationEXPERIMENT 8 Ideal Gas Law: Molecular Weight of a Vapor
EXPERIMENT 8 Ideal Gas Law: Molecular Weight of a Vapor Purpose: In this experiment you will use the ideal gas law to calculate the molecular weight of a volatile liquid compound by measuring the mass,
More informationUNIT 10 - GASES. Notes & Worksheets - Honors
Ideal Gas Equation 1 WKSHT 1.) What is the pressure exerted by 2.0 moles of an ideal gas when it occupies a volume of 12.0 L at 373 K? 2.) A flashbulb of volume 2.6 cm 3 contains O 2 gas at a pressure
More informationGas Laws. Introduction
Gas Laws Introduction In 1662 Robert Boyle found that, at constant temperature, the pressure of a gas and its volume are inversely proportional such that P x V = constant. This relationship is known as
More informationDetermination of the Gas-Law Constant (R) using CO2
Determination of the Gas-Law Constant (R) using CO2 EXPERIMENT 11 Prepared by Edward L. Brown and Miranda Raines, Lee University The student will become familiar with ideal gases and how their properties
More informationGas Laws. 2 HCl(aq) + CaCO 3 (s) H 2 O(l) + CO 2 (g) + CaCl 2 (aq) HCl(aq) + NaHCO 3 (s) H 2 O(l) + CO 2 (g) + NaCl(aq)
Gas Laws Introduction: Although we cannot see gases, we can observe their behavior and study their properties. For example, we can watch a balloon filled with helium gas floating in air and conclude that
More informationCompleted ALL 2 Warm-up IC Kinetic Molecular Theory Notes. Kinetic Molecular Theory and Pressure Worksheet
Name: Unit 10- Gas Laws Day Page # Description IC/HW Due Date Completed ALL 2 Warm-up IC 1 3 5 Kinetic Molecular Theory Notes IC 1 6 8 Kinetic Molecular Theory and Pressure Worksheet IC 2 9 10 Gas Law
More informationPressure of the atmosphere varies with elevation and weather conditions. Barometer- device used to measure atmospheric pressure.
Chapter 12 Section 1 Pressure A gas exerts pressure on its surroundings. Blow up a balloon. The gas we are most familiar with is the atmosphere, a mixture of mostly elemental nitrogen and oxygen. Pressure
More informationMeasuring Carbon Dioxide in Breath
Measuring Carbon Dioxide in Breath OBJECTIVES 1. Measure the partial pressure of carbon dioxide in your breath 2. Estimate the volume of air you exhale per day 3. Estimate the volume and mass of CO2 you
More information11.1 Dumas Method - Pre-Lab Questions
11.1 Dumas Method - Pre-Lab Questions Name: Instructor: Date: Section/Group: Show all work for full credit. 1. If a 275-mL gas container has pressure of 732.6 mm Hg at -28 C, how many moles of gas are
More informationThe Kinetic-Molecular Theory of Gases based on the idea that particles are always in motion
The Kinetic-Molecular Theory of Gases based on the idea that particles are always in motion Five assumptions: 1. Most of the volume occupied dby a gas is empty space 2. Collisions between gas particles
More informationName Chemistry Pre-AP
Name Chemistry Pre-AP Notes: Gas Laws and Gas Stoichiometry Period Part 1: The Nature of Gases and The Gas Laws I. Nature of Gases A. Kinetic-Molecular Theory The - theory was developed to account for
More informationGas Laws. Figure 1: Experimental Set-up with Leveling Bulb. GCC CHM 151LL: Gas Laws GCC, 2019 page 1 of 8
Gas Laws Introduction Although we cannot see gases, we can observe their behavior and study their properties. This lab will apply several concepts from Ideal Gas Laws. You will use your knowledge of chemical
More informationThe Ideal Gas Constant
Chem 2115 Experiment # 8 The Ideal Gas Constant OBJECTIVE: This experiment is designed to provide experience in gas handling methods and experimental insight into the relationships between pressure, volume,
More informationGas Laws. 2 HCl(aq) + CaCO 3 (s) H 2 O(l) + CO 2 (g) + CaCl 2 (aq) HCl(aq) + NaHCO 3 (s) H 2 O(l) + CO 2 (g) + NaCl(aq)
Gas Laws Introduction: Although we cannot see gases, we can observe their behavior and study their properties. For example, we can watch a balloon filled with helium gas floating in air and conclude that
More informationR: The Ideal Gas Constant Pre-Lab Assignment
R: The Ideal Gas Constant Pre-Lab Assignment Read the entire laboratory investigation and the relevant pages in your textbook, then answers the questions that follow in the space provided below. 1 Describe
More informationAccelerated Chemistry Study Guide Chapter 13: Gases
Accelerated Chemistry Study Guide Chapter 13: Gases Terms, definitions, topics Diffusion Kinetic Molecular Theory Atmospheric pressure Barometer Manometer STP Absolute zero Page 1 of 42 Molar volume Partial
More informationBoyle s Law Practice
Boyle s Law Practice Boyle s Law is an indirect relationship. Most of these problems can be done in your head without showing your work. 1. Herman has 30.0 L of helium gas trapped in a cylinder by a piston.
More informationBoyle s Law VC 09. Experiment 9: Gas Laws. Abstract
Experiment 9: Gas Laws VC 09 Abstract In this laboratory activity, you will experimentally confirm Boyle s Law, determine absolute zero from Gay-Lussac's Law, and determine the molecular weight of acetone,
More informationCHM 2045L Physical Properties
CHM 2045L Physical Properties Purpose: To observe and record some common physical properties. Background: Physical properties can tell us a lot about an unknown chemical. In this experiment you will look
More informationProperties of Gases Observing Atom Pressure of a Gas Measuring Gas Products of Chemical Inferring Molecule Reactions
It s a Gas! In a gas, molecules or atoms move constantly and spread far apart. If a gas cannot escape its container, it applies pressure on the container. For example, gas pressure inflates a balloon.
More informationGASES. Unit #8. AP Chemistry
GASES Unit #8 AP Chemistry I. Characteristics of Gases A. Gas Characteristics: 1. Fills its container a. no definite shape b. no definite vol. 2. Easily mixes w/ other gases 3. Exerts pressure on its surroundings
More informationChapter 13 Gases. H. Cannon, C. Clapper and T. Guillot Klein High School. Pressure/Temperature Conversions
Chapter 13 Gases Pressure/Temperature Conversions Convert the following: 1. 3.50 atm = kpa 2. 123 atm = mmhg 3. 970.0 mmhg = torr 4. 870.0 torr = kpa 5. 250.0 kpa = atm 6. 205.0 mmhg = kpa 7. 12.4 atm
More informationGases. Edward Wen, PhD
Gases Edward Wen, PhD Properties of Gases expand to completely fill their container take the shape of their container low density much less than solid or liquid state compressible when pressure is changed.
More informationChapter 5. Nov 6 1:02 PM
Chapter 5 Nov 6 1:02 PM Expand to fill their containers Fluid motion (they flow) Have low densities (1/1000 the density of equivalent liquids or solids) Compressible Can Effuse and Diffuse Effuse: The
More informationUnit 11 Gas Laws Chapters 13 of your textbook
Unit 11 Gas Laws Chapters 13 of your textbook Early Booklet E.C.: + 2 Unit 11 Hwk. Pts.: / 19 Unit 11 Lab Pts.: / 20 Late, Incomplete, No Work, No Units Fees? Y / N Learning Targets for Unit 11 1.1 I can
More informationGases and Pressure. Main Ideas
Gases and Pressure Key Terms pressure millimeters of mercury partial pressure newton atmosphere of pressure Dalton s law of partial pressures barometer pascal In the chapter States of Matter, you read
More informationStudent s Name: Date : Molar volume of butane
Student s Name: Date : Background Molar volume of butane The purpose of this activity is to determine the molar mass of butane using gas from a butane lighter. The experiment depends on the fact that the
More informationUnit 10: Gas Laws. Monday Tuesday Wednesday Thursday Friday. 10 Review for Cumulative Retest. 17 Chem Think Gas Laws Tutorial- Computer Lab-
Unit 10: Gas Laws Name: Monday Tuesday Wednesday Thursday Friday February 8 Stoichiometry Test Review 9 Stoichiometry Test 10 Review for Cumulative Retest 11 Cumulative Re-Test 12 Pressure & Kinetic Theory
More informationUnit 8: Gases and States of Matter
Unit 8: Gases and States of Matter Gases Particles that have no definite shape or volume. They adapt to the shape and volume of their container. Ideal gases are imaginary gases that comply with all the
More informationMultiple Choice (40%)
AP Chemistry Test (Chapter 5) Please do not write on this test thank you! Multiple Choice (40%) 1) A sealed rigid container is filled with three ideal gases: A, B and C. The partial pressure of each gas
More informationUnder ideal conditions, the rates at which different gases diffuse (spread out) are proportional to their molar masses.
Chemistry Ms. Ye Name Date Block Graham s Law of Diffusion- Under ideal conditions, the rates at which different gases diffuse (spread out) are proportional to their molar masses. In other words, gas molecules
More informationHonors Chemistry - Unit 11
Honors Chemistry - Unit 11 Chapters 10 & 11 Gases, Gas Laws, and Gas Stoichiometry Vocabulary Due: UT Quest(s): VOCABULARY: Quizzes: Test Date: Ideal gas standard atmospheric pressure standard temperature
More informationPlease do not write on this test. Please use the answer sheet. 1) Please choose all conditions that would allow a gas sample to behave ideally.
AP Chemistry Test (Chapter 5) Please do not write on this test. Please use the answer sheet. Multiple Choice (50%) 1) Please choose all conditions that would allow a gas sample to behave ideally. I) Nonpolar
More informationB. As the gas particles move and strike a surface, they push on that surface 1. If we could measure the total amount of force exerted by gas
Chapter 5: Gases I. The Structure of a Gas A. Gases are composed of particles that are flying around very fast in their container(s). 1. The particles travel in straight lines until they encounter either
More informationExample: 25 C = ( ) K = 298 K. Pressure Symbol: p Units: force per area 1Pa (Pascal) = 1 N/m 2
Chapter 6: Gases 6.1 Measurements on Gases MH5, Chapter 5.1 Let s look at a certain amount of gas, i.e. trapped inside a balloon. To completely describe the state of this gas one has to specify the following
More informationExamLearn.ie. The Air & Oxygen
ExamLearn.ie The Air & Oxygen The Air & Oxygen The air is a mixture of gases, which forms a blanket around the earth. Another name for the air is the atmosphere. *To investigate the percentage of oxygen
More informationName Hour. The Behavior of Gases. Practice B
Name Hour The Behavior of Gases Practice B B 1 Objective 1: Apply Boyle s Law, Charles s Law, and Gay-Lussac s Law to solve problems involving pressure and volume and temperature. 1. A high-altitude balloon
More informationBasic Concepts of Chemistry Notes for Students [Chapter 10, page 1] D J Weinkauff - Nerinx Hall High School. Chapter 10 Gases
Basic Concepts of Chemistry Notes for Students [Chapter 10, page 1] Chapter 10 Gases We have talked a little about gases in Chapter 3 and we dealt briefly with them in our stoichiometric calculations in
More informationLecture Handout 5: Gases (Online Text Chapter 6)
Lecture Handout 5: Gases (Online Text Chapter 6) I. The Structure of a Gas A. Gases are composed of particles that are flying around very fast in their container(s). 1. The particles travel in straight
More informationGeneral Properties of Gases
GASES Chapter 13 Importance of Gases Airbags fill with N 2 gas in an accident. Gas is generated by the decomposition of sodium azide,, NaN 3. 2 NaN 3 ---> > 2 Na + 3 N 2 THREE STATES OF MATTER General
More informationchapter 4 Diffusion and Osmosis I. Diffusion Introduction
Diffusion and Osmosis JJ Introduction Cells are the smallest livin units of an oranism, and it is the cells that carry out most of the basic physioloical functions of an oranism. In order to carry out
More informationAdditional Reading General, Organic and Biological Chemistry, by Timberlake, chapter 8.
Gas Laws EXPERIMENTAL TASK Determine the mathematical relationship between the volume of a gas sample and its absolute temperature, using experimental data; and to determine the mathematical relationship
More information4.) There are no forces of attraction or repulsion between gas particles. This means that
KINETIC MOLECULAR (K-M) THEORY OF MATTER NOTES - based on the idea that particles of matter are always in motion - assumptions of the K-M Theory 1.) Gases consist of large numbers of tiny particles that
More informationKinetic-Molecular Theory
GASES Chapter Eleven Kinetic-Molecular Theory! Recall that our only previous description of gases stated that gases completely fill and take the shape of their containers.! The Kinetic-Molecular Theory
More informationKinetic Molecular Theory imaginary Assumptions of Kinetic Molecular Theory: Problems with KMT:
AP Chemistry Ms. Ye Name Date Block Kinetic Molecular Theory Explains properties of gases, liquids, and solids in terms of energy using an ideal gas, an imaginary which fits all the assumptions of kinetic
More informationExperiment 8 GAS LAWS
Experiment 8 GAS LAWS FV 6/25/2017 MATERIALS: Amontons Law apparatus, Boyle s Law apparatus, Avogadro s Corollary apparatus, four beakers (2 L), warm-water bath, ice, barometer, digital thermometer, air
More informationChemistry HP Unit 6 Gases. Learning Targets (Your exam at the end of Unit 6 will assess the following:) 6. Gases
Chemistry HP Unit 6 Gases Learning Targets (Your exam at the end of Unit 6 will assess the following:) 6. Gases 6-1. Define pressure using a mathematical equation. 6-2. Perform calculations involving pressure,
More informationGAS LAW WORKSHEET 1 KEY
377 GAS LAW WORKSHEET 1 KEY 1. A sample of oxygen gas occupies a volume of 436. ml at 1.0 atm. If the temperature is held constant, what would the pressure of this gas be when the gas is compressed to
More informationKinetic-Molecular Theory of Matter
Gases Properties of Gases Gas Pressure Gases What gases are important for each of the following: O 2, CO 2 and/or He? A. B. C. D. 1 2 Gases What gases are important for each of the following: O 2, CO 2
More information2. Calculate the ratio of diffusion rates for carbon monoxide (CO) and carbon dioxide (CO2). υa = MB = 44 = 1.25
Gas laws worksheet (2-08) (modified 3/17) Answer key Graham s Law 1. Calculate the ratio of effusion rates for nitrogen (N2) and neon (Ne). υa = MB = 20 = 0.845 υb MA 28 2. Calculate the ratio of diffusion
More informationStates of Matter Review
States of Matter Review May 13 8:16 PM Physical States of Matter (Phases) Solid Liquid Melting Gas Condensation Freezing Evaporation Deposition Sublimation Sep 13 6:04 PM 1 May 13 8:11 PM Gases Chapter
More informationWorksheet: Solubility
1. According to your Reference Tables, which substance forms an unsaturated solution when 80 grams of the substance is dissolved in 100 grams of H 2 O at 10 C? (A) KI (B) KNO 3 (C) NaNO 3 (D) NaCl 2. The
More informationSection 8: Gases. The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC (c).
Section 8: Gases The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 8.01 Simple Gas Laws Chemistry (9)(A) 8.02 Ideal Gas Law Chemistry
More informationPlease do not write on this test. Please use the answer sheet.
AP Chemistry Test (Chapter 5) Multiple Choice (50%) Please do not write on this test. Please use the answer sheet. Form: Snowboard 1) A sample of argon gas is sealed in a rigid metal tank. The temperature
More information1. Quantity of a gas (moles) 2. Temperature of the gas. 3. Volume occupied by the gas. 4. Pressure exerted by the gas. PV = nrt
Experiment 5 Stoichiometry : Gases Determining the Ideal Gas Constant Lab Owl Announcement: Upon completion of this lab log onto OWL. Your fourth Lab Owl assignment, Lab Owl: Exp 5 should appear there.
More informationWorld of Chemistry Notes for Students [Chapter 13, page 1] Chapter 13 Gases
World of Chemistry Notes for Students [Chapter 3, page ] Chapter 3 Gases ) Sec 3.8 Kinetic Theory of Gases and the Nature of Gases The Kinetic Theory of Matter says that the tiny particles in all forms
More informationYou should be able to: Describe Equipment Barometer Manometer. 5.1 Pressure Read and outline 5.1 Define Barometer
A P CHEMISTRY - Unit 5: Gases Unit 5: Gases Gases are distinguished from other forms of matter, not only by their power of indefinite expansion so as to fill any vessel, however large, and by the great
More informationNOTES: Behavior of Gases
NOTES: Behavior of Gases Properties of Gases Gases have weight Gases take up space Gases exert pressure Gases fill their containers Gases are mostly empty space The molecules in a gas are separate, very
More informationFigure Vapor-liquid equilibrium for a binary mixture. The dashed lines show the equilibrium compositions.
Another way to view this problem is to say that the final volume contains V m 3 of alcohol at 5.93 kpa and 20 C V m 3 of air at 94.07 kpa and 20 C V m 3 of air plus alcohol at 100 kpa and 20 C Thus, the
More informationPre-Lab 6: Gas Law ~ 70 ~
Name: Pre-Lab 6: Gas Law Section: Answer the following questions after reading the background information at the beginning of the lab. This should be completed before coming to lab. 1. Convert the following:
More informationName: Period: Date: CHAPTER 10 NOTES 10.3: The Gas Laws
Name: Period: Date: 1. Define gas laws: CHAPTER 10 NOTES 10.3: The Gas Laws 2. What units do the following measurements need to be in to describe gases? Boyle s Law a. Temperature b. Volume c. Pressure
More informationPRESSURE-TEMPERATURE RELATIONSHIP IN GASES
PRESSURE-TEMPERATURE RELATIONSHIP IN GASES LAB PS2.PALM INTRODUCTION Gases are made up of molecules that are in constant motion and exert pressure when they collide with the walls of their container. The
More informationName /74. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Ch 11 Gases STUDY GUIDE Accelerated Chemistry SCANTRON Name /74 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following statements
More informationA) It cannot be predicted. B) It is squared. C) It is doubled. D) It is halved. E) It does not change.
AP Chemistry Test (Chapter 5) Class Set Multiple Choice (50%) 1) A sample of argon gas is sealed in a container. The volume of the container is doubled at a constant temperature. What happens to the pressure
More informationUnit 8: Kinetic Theory Homework Packet (90 points)
Name: Key Period: By the end of Unit 8, you should be able to: Kinetic Theory Chapter 13-14 4. Define kinetic theory of gases including collisions 5. Define pressure, including atmospheric pressure, vapor
More informationHeat Engine. Reading: Appropriate sections for first, second law of thermodynamics, and PV diagrams.
Heat Engine Equipment: Capstone, 2 large glass beakers (one for ice water, the other for boiling water), temperature sensor, pressure sensor, rotary motion sensor, meter stick, calipers, set of weights,
More informationTEMPERATURE S RELATIONSHIP TO GAS & VAPOR PRESSURE
TEMPERATURE S RELATIONSHIP TO GAS & VAPOR PRESSURE Adapted from "Chemistry with Computers" Vernier Software, Portland OR, 1997 ELECTRONIC LABORATORY NOTEBOOK (ELN) INSTRUCTIONS Read the directions and
More informationChapter 5 Gases. AP CHEMISTRY Chapter 5 Scotch Plains-Fanwood High School Page 1
Chapter 5 Gases Kinetic Theory All matter is composed of tiny particles that are in continuous, random motion. Gas Pressure = Force Demo: Test tube/h2o beaker Area Demo: Can AP CHEMISTRY Chapter 5 Scotch
More informationCP Chapter 13/14 Notes The Property of Gases Kinetic Molecular Theory
CP Chapter 13/14 Notes The Property of Gases Kinetic Molecular Theory Kinetic Molecular Theory of Gases The word kinetic refers to. Kinetic energy is the an object has because of its motion. Kinetic Molecular
More informationGases. Chapter 5: Gas Laws Demonstration. September 10, Chapter 5 Gasses.notebook. Dec 18 10:23 AM. Jan 1 4:11 PM. Crushing 55 gallon drum
Chapter 5: Gases Dec 18 10:23 AM Gas Laws Demonstration Crushing 55 gallon drum Egg in a bottle Student in a bag Boiling Water Charles gas Law Water in a flask Ballon in a bottle Jan 1 4:11 PM 1 5.1 Pressure
More informationChapter 13. Gases. Copyright Cengage Learning. All rights reserved 1
Chapter 13 Gases Copyright Cengage Learning. All rights reserved 1 Section 13.1 Pressure Why study gases? An understanding of real world phenomena. An understanding of how science works. Copyright Cengage
More informationChapter 5 TEST: Gases
Chapter 5 TEST: Gases 1) Gases generally have A) low density B) high density C) closely packed particles D) no increase in volume when temperature is increased E) no decrease in volume when pressure is
More informationStates of Matter. Q 7. Calculate the average of kinetic energy, in joules of the molecules in 8.0 g of methane at 27 o C. (IIT JEE Marks)
Q 1. States of Matter Calculate density of NH 3 at 30 o C and 5 atm pressure Q 2. (IIT JEE 1978 3 Marks) 3.7 g of a gas at 25 o C occupied the same volume as 0.184g of hydrogen at 17 o C and at the same
More informationDate: Period: Gas Laws Worksheet #1 - Boyle s, Charles, Gay-Lussac s, and Combined Gas Law
Name: Date: Period: Gas Laws Worksheet #1 - Boyle s, Charles, Gay-Lussac s, and Combined Gas Law Boyle s Law: V1P1 = V2P2 1. A gas sample contained in a cylinder equipped with a moveable piston occupied
More informationChapter 5: Gases 5.1 Pressure Why study gases? An understanding of real world phenomena. An understanding of how science works.
Chapter 5: Gases 5.1 Pressure Why study gases? An understanding of real world phenomena. An understanding of how science works. A Gas Uniformly fills any container. Easily compressed. Mixes completely
More informationUnit 9 Packet: Gas Laws Introduction to Gas Laws Notes:
Name: Unit 9 Packet: Gas Laws Introduction to Gas Laws Notes: Block: In chemistry, the relationships between gas physical properties are described as gas laws. Some of these properties are pressure, volume,
More informationGas Laws. Boyle s Law Charle s law Gay-Lussac s Law Avogadro s Law Dalton s Law Henry s Law
Gas Laws Boyle s Law Charle s law Gay-Lussac s Law Avogadro s Law Dalton s Law Henry s Law 1 1 What is Pressure? Gas molecules cause pressure 2 2 The pressure of the gas in the container on the right would
More informationDEMONSTRATION 2.1 PROPERTIES OF CO 2. Chapter 2: Gases
DEMONSTRATION 2.1 Chapter 2: Gases PROPERTIES OF CO 2 This demonstration has two aims: firstly, to show that carbon dioxide gas is denser than air; secondly, to show that carbon dioxide will not support
More informationA. What are the three states of matter chemists work with?
Chapter 10 and 12 The Behavior of Gases Chapter 10 The States of Matter A. What are the three states of matter chemists work with? Section 10.1 Pg 267 B. We will explain the behavior of gases using the
More informationIntermolecular Forces
Experiment 2 Intermolecular Forces Prepared by Ross S. Nord, Eastern Michigan University with large parts adapted from Chemistry with Computers by Dan D. Holmquist and Donald D. Volz PURPOSE The purpose
More informationChem 110 General Principles of Chemistry
CHEM110 Worksheet - Gases Chem 110 General Principles of Chemistry Chapter 9 Gases (pages 337-373) In this chapter we - first contrast gases with liquids and solids and then discuss gas pressure. - review
More informationChapter 13: The Behavior of Gases
Chapter 13: The Behavior of Gases I. First Concepts a. The 3 states of matter most important to us: solids, liquids, and gases. b. Real Gases and Ideal Gases i. Real gases exist, ideal gases do not ii.
More informationChapter 13 Gases and Pressure. Pressure and Force. Pressure is the force per unit area on a surface. Force Area. Pressure =
Chapter 13 Gas Laws Chapter 13 Gases and Pressure Pressure and Force Pressure is the force per unit area on a surface. Pressure = Force Area Chapter 13 Gases and Pressure Gases in the Atmosphere The atmosphere
More informationGas Laws: Boyle s and Amonton s Laws MCTC Chemistry v.9.17
Gas Laws: Boyle s and Amonton s Laws MCTC Chemistry v.9.17 Objective: The purpose of this experiment is confirm Boyle's and Amontons' Laws in the laboratory. Prelab Questions: Read through this lab handout
More informationBoyle s Law Practice Problems Name:
Boyle s Law Practice Problems Name: 1. If a gas at 25.0 C occupies 3.60 L at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm? 2. 500.0 ml of a gas is collected at 745.0 mm Hg.
More informationMeasuring Mass and Volume
Measuring Mass and Volume Experiment 2 Expt 2 Measurement.wpd INTENT The purpose of this experiment is to introduce some fundamental aspects of the measurement making process as well as to introduce some
More information