Overview of Physical Properties of Gases. Gas Pressure


 Alyson Boyd
 2 years ago
 Views:
Transcription
1 Overview of Physical Properties of Gases! volume changes with pressure! volume changes with temperature! completely miscible! low density gases: < 2 g/l liquids and solids: 1000 g/l Gas Pressure force in all directions
2 Gas Pressure Pressure = force area Pascal, the SI standard F (N) P (Pa) = S (m2) kg! 9.81m/s2 = Pa 1 m2 at 0 oc, at see level Gas Pressure Pressure = force area F (N) P (Pa) = S (m2) 1 atm = Pa at 0 oc, at see level
3 >500 km of air Gas Pressure kg! 9.81m/s2 = Pa 1 m2 For mercury: 760 mm 1 atm = Pa = 760 mmhg (torr) For water: ~ 34 feet Ideal Gas Laws complete description of a sample of gas:! volume (V)! pressure (P)! temperature (T)! amount (n)
4 Ideal Gas Laws PV = nrt Ideal Gas Laws PV = nrt PV =R nt
5 Ideal Gas Laws PV =R nt R = 8.31 J mol1 K1 universal gas constant R = atm L mol1 K1 Ideal Gas Laws PV =R nt universal gas constant R = atm L mol1 K1
6 Ideal Gas Laws PV nt = R Ideal Gas Laws PV nt = R fixed n and T PV = constant Boyle s law
7 Ideal Gas Laws PV nt = R fixed n and T PV = constant Boyle s law V T fixed n and P = constant Charles law fixed n and T Ideal Gas Laws PV nt = R fixed n and P fixed P and T PV = constant Boyle s law V T = constant Charles law V n = constant Avogadro s law
8 Boyle s Law at fixed n and T P 1 V 1 = P 2 V 2 Charles Law at fixed n and P V 1 V = 2 T 1 T 2
9 Avogadro s Law at fixed P and T V 1 V = 2 n 1 n 2 Gas at Standard Conditions Standard conditions are standard temperature and pressure STP: 0 o C and 1 atm (760 torr) Volume of 1 mol of gas is 22.4 L
10 Ideal Gas molecules have mass, but no volume no attraction or repulsion between molecules move in straight lines between collisions no loss of energy during collisions, only transfer Molar Mass and Density PV = nrt and n = m M Molar mass: Density: M = d = mrt PV MP RT
11 Partial Pressure of Gases P total = P 1 + P 2 + P 3 + partial pressure is proportional to mole fraction that is, P 1 n = 1 P total n total P 1 = n 1 n total! P total Sample Problem 5.9 A small piece of zinc reacts with HCl to form H 2, which is collected over water at 16 o C into a large flask. The total pressure is adjusted to barometric pressure (752 torr), and the volume is 1495 ml. Calculate the partial pressure and mass of H 2. (P H2O at 16 o C is 13.6 torr).
12 Gas Laws and Stoichiometry P, V, T of gas A ideal gas law Amount (mol) of gas A molar ratio from balanced equation Amount (mol) of gas B ideal gas law P, V, T of gas B Sample Problem 5.10 Ammonia and hydrogen chloride gases react to form solid ammonium chloride. A 10.0 L flask contains ammonia at atm and 22 o C, and 155 ml of hydrogen chloride at 7.50 atm and 271 K is introduced. After the reaction occurs and the temperature returns to 22 o C, what is the pressure inside the flask?
13 KineticMolecular Theory molecules have mass, but no volume no attraction or repulsion between molecules move in straight lines between collisions no loss of energy during collisions, only transfer KineticMolecular Theory molecules have mass, but no volume no attraction or repulsion between molecules move in straight lines between collisions no loss of energy during collisions, only transfer The Meaning of Temperature Temperature is proportional to the average kinetic energy of molecular motion: E k = 3 2 R N A T
14 KineticMolecular Theory KineticMolecular Theory Nitrogen, N 2 : Diffusion Average molecular speed at 20 o C and 1 atm 0.47 km/s or 1100 mph Collision Frequency 7.1!10 9 collisions/s
15 Real Gases Deviation from ideal behavior are due to: 1. Intermolecular attractions 2. Molecular volume Real Gases
16 Real Gases: van der Waals equation P + n2 a V 2 b and a are (V  nb) = nrt van der Waals constants unique for each gas determined experimentally Practice Problems At 1400 mmhg and 13 o C, a diver inhales a 208 ml bubble of air that is 77% on N 2, 17% of O 2, and 6.0% of CO 2 by volume. (a) How many ml would the volume of the bubble be if it were exhaled at the surface at 1 atm and 298 K? (b) How many moles of N 2 are in the bubble?
17 Practice Problems An environmental engineer submits a sample of air contaminated with sulfur dioxide to the lab analysis. To a 500. ml sample at 700 torr and 38 o C, she adds ml of M aqueous iodine, which reacts as follows: SO 2 + I 2 + H 2 O " HSO I  + H + The unreacted I 2 is titrated with ml of M of sodium thiosulfate: I 2 + S 2 O 3 2 " I  + S 4 O 6 2 What is the volume % of SO 2 in the air sample? Hg Practice Problems
Gas particles move in straight line paths. As they collide, they create a force, pressure.
#28 notes Unit 4: Gases Ch. Gases I. Pressure and Manometers Gas particles move in straight line paths. As they collide, they create a force, pressure. Pressure = Force / Area Standard Atmospheric Pressure
More informationCHAPTER 12. Gases and the KineticMolecular Theory
CHAPTER 12 Gases and the KineticMolecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids
More informationChemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10 Gases
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Gases A Gas Has neither a definite volume nor shape. Uniformly fills any container.
More informationCHE141 Chapter 10. Chapter 10 Gases
Chapter 0 Gases. A sample of gas (4.g) initially at 4.00 atm was compressed from 8.00 L to.00 L at constant temperature. After the compression, the gas pressure was atm. (a). 4.00 (b)..00 (c)..00 (d).
More informationLecture Notes: Gas Laws and Kinetic Molecular Theory (KMT).
CHEM110 Week 9 Notes (Gas Laws) Page 1 of 7 Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). Gases Are mostly empty space Occupy containers uniformly and completely Expand infinitely Diffuse
More informationGases. Gas: fluid, occupies all available volume Liquid: fluid, fixed volume Solid: fixed volume, fixed shape Others?
CHAPTER 5: Gases Chemistry of Gases Pressure and Boyle s Law Temperature and Charles Law The Ideal Gas Law Chemical Calculations of Gases Mixtures of Gases Kinetic Theory of Gases Real Gases Gases The
More informationAS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol 1
Moles 1 MOLES The mole the standard unit of amount of a substance the number of particles in a mole is known as Avogadro s constant (L) Avogadro s constant has a value of 6.023 x 10 23 mol 1. Example
More informationChapter 4 The Properties of Gases
Chapter 4 The Properties of Gases Significant Figure Convention At least one extra significant figure is displayed in all intermediate calculations. The final answer is expressed with the correct number
More informationF321 MOLES. Example If 1 atom has a mass of 1.241 x 1023 g 1 mole of atoms will have a mass of 1.241 x 1023 g x 6.02 x 10 23 = 7.
Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol 1.
More informationGas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion.
Name Period Gas Laws Kinetic energy is the energy of motion of molecules. Gas state of matter made up of tiny particles (atoms or molecules). Each atom or molecule is very far from other atoms or molecules.
More informationGases. States of Matter. Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large Chaotic (random)
Gases States of Matter States of Matter Kinetic E (motion) Potential E(interaction) Distance Between (size) Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large
More informationFigure 10.3 A mercury manometer. This device is sometimes employed in the laboratory to measure gas pressures near atmospheric pressure.
Characteristics of Gases Practice Problems A. Section 10.2 Pressure Pressure Conversions: 1 ATM = 101.3 kpa = 760 mm Hg (torr) SAMPLE EXERCISE 10.1 Converting Units of Pressure (a) Convert 0.357 atm to
More informationTutorial 6 GASES. PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg. STP: Standard Temperature and Pressure: 273 K and 1 atm (or 760 mm Hg)
T41 Tutorial 6 GASES Before working with gases some definitions are needed: PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg TEMPERATURE: Kelvin, K, which is o C + 273 STP: Standard Temperature and Pressure:
More informationCHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry
CHEMISTRY Matter and Change 13 Table Of Contents Chapter 13: Gases Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry State the relationships among pressure, temperature,
More informationKinetic Molecular Theory
Kinetic Molecular Theory Particle volume  The volume of an individual gas particle is small compaired to that of its container. Therefore, gas particles are considered to have mass, but no volume. There
More informationForce. Pressure = ; Area. Force = Mass times Acceleration;
Force Pressure = ; Area Force = Mass times Acceleration; If mass = kg, and acceleration = m/s 2, Force = kg.m/s 2 = Newton (N) If Area = m 2, Pressure = (kg.m/s 2 )/m 2 = N/m 2 = Pascal; (1 Pa = 1 N/m
More informationUse each of the terms below to complete the passage. Each term may be used more than once.
Gases Section 13.1 The Gas Laws In your textbook, read about the basic concepts of the three gas laws. Use each of the terms below to complete the passage. Each term may be used more than once. pressure
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55
More informationBoyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P
Boyles Law At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 or k 1 Boyles Law Example ressure olume Initial 2.00 atm 100 cm 3
More informationExam 4 Practice Problems false false
Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids
More informationThe Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10
Our Atmosphere The Gas Laws 99% N 2 and O 2 78% N 2 80 70 Nitrogen Chapter 10 21% O 2 1% CO 2 and the Noble Gases 60 50 40 Oxygen 30 20 10 0 Gas Carbon dioxide and Noble Gases Pressure Pressure = Force
More informationGases and KineticMolecular Theory: Chapter 12. Chapter Outline. Chapter Outline
Gases and KineticMolecular heory: Chapter Chapter Outline Comparison of Solids, Liquids, and Gases Composition of the Atmosphere and Some Common Properties of Gases Pressure Boyle s Law: he VolumePressure
More information= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm
Chapter 13 Gases 1. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. Gases have volumes that depend on their conditions, and can be compressed or expanded by
More informationChemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10 Gases.
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 The things we will cover in this chapter: How differ from solids and liquids Pressure,
More informationThe Gas Laws. The effect of adding gas. 4 things. Pressure and the number of molecules are directly related. Page 1
The Gas Laws Describe HOW gases behave. Can be predicted by the theory. The Kinetic Theory Amount of change can be calculated with mathematical equations. The effect of adding gas. When we blow up a balloon
More informationCHM1045 Practice Test 3 v.1  Answers Name Fall 2013 & 2011 (Ch. 5, 6, 7, & part 11) Revised April 10, 2014
CHM1045 Practice Test 3 v.1  Answers Name Fall 013 & 011 (Ch. 5, 6, 7, & part 11) Revised April 10, 014 Given: Speed of light in a vacuum = 3.00 x 10 8 m/s Planck s constant = 6.66 x 10 34 J s E (.18x10
More informationAP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward
Signed in as Daniel Semenick, Instructor Help Sign Out AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward Instructor Resources
More informationHow many moles are in a breath of air whose volume is 2.32L at body temperature (37 C) and a pressure of 745 torr?
Lecture 9 State of gas described by (n,p,v,t) n # moles P pressure V volume T (absolute) temperature (K) Sample Problem A balloon filled with helium has a volume of 1.60 L at 1.00 atm and 25oC. What will
More informationChapter 5. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Class: Date: Chapter 5 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is the pressure of the sample of gas trapped in the opentube mercury manometer
More informationBloom s Taxonomy. Study Habits and Study Resources: Pause. Expectations: Develop a working knowledge of the topics.
Dr. C. Weldon Mathews Chem 1 Office: 004 Evans Lab Telephone: 91574 email: mathews.6@osu.edu web: www.chemistry.ohiostate.edu/~mathews/ Office hours: TR 1:30  :00 pm TR 4:005:00 pm or by appointment
More informationKinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check.
Chapter 6 Gases Kinetic Theory of Gases 6.1 Properties of Gases 6.2 Gas Pressure A gas consists of small particles that move rapidly in straight lines. have essentially no attractive (or repulsive) forces.
More informationGas  a substance that is characterized by widely separated molecules in rapid motion.
Chapter 10  Gases Gas  a substance that is characterized by widely separated molecules in rapid motion. Mixtures of gases are uniform. Gases will expand to fill containers (compare with solids and liquids
More informationCHEMISTRY GAS LAW S WORKSHEET
Boyle s Law Charles Law GuyLassac's Law Combined Gas Law For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure PV = k The volume of a fixed mass of gas is
More informationHonors Chemistry. Chapter 11: Gas Law Worksheet Answer Key Date / / Period
Honors Chemistry Name Chapter 11: Gas Law Worksheet Answer Key Date / / Period Complete the following calculation by list the given information, rewriting the formula to solve for the unknown, and plugging
More information7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.
CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,
More information2. If pressure is constant, the relationship between temperature and volume is a. direct b. Inverse
Name Unit 11 Review: Gas Laws and Intermolecular Forces Date Block 1. If temperature is constant, the relationship between pressure and volume is a. direct b. inverse 2. If pressure is constant, the relationship
More informationSubstances that are liquids or solids under ordinary conditions may also exist as gases. These are often referred to as vapors. Properties of Gases
Common Student Misconceptions Students need to be told to always use Kelvin temperatures in gas problems. Students should always use units (and unit factor analysis) in gaslaw problems to keep track of
More informationGas Laws. E k = ½ (mass)(speed) 2. v101613_10am
Gas Laws v101613_10am Objective: In this lab you will become familiar with the Ideal Gas Law and Dalton s Law of Partial Pressures. You will be able to use the information collected along with stoichiometry
More informationGases. Macroscopic Properties. Petrucci, Harwood and Herring: Chapter 6
Gases Petrucci, Harwood and Herring: Chapter 6 CHEM 1000A 3.0 Gases 1 We will be looking at Macroscopic and Microscopic properties: Macroscopic Properties of bulk gases Observable Pressure, volume, mass,
More informationGuide to Chapter 9. Gases Answers in green and red.
Guide to Chapter 9. Gases Answers in green and red. We will spend three lecture days on this chapter. Day 1. Pressure, barometers, STP, manometers, Charles Law, Boyles Law, Aogadro's Law, Combined Gas
More informationC 6 H 12 O O 2 6 CO H 2 O
Honors Chemistry Name Chapter 11: Gas Laws and Stoichiometry WS II Date / / eriod 1. Calcium hydride reacts with water to form hydrogen gas and calcium hydroxide. This reaction is sometimes used to inflate
More informationCHAPTER 12 GASES AND THEIR BEHAVIOR
Chapter 12 Gases and Their Behavior Page 1 CHAPTER 12 GASES AND THEIR BEHAVIOR 121. Which of the following represents the largest gas pressure? (a) 1.0 atm (b) 1.0 mm Hg (c) 1.0 Pa (d) 1.0 KPa 122. Nitrogen
More informationSample Exercise 10.1 Converting Pressure Units
Sample Exercise 10.1 Converting Pressure Units (a) Convert 0.357 atm to torr. (b) Convert 6.6 10 2 torr to atmospheres. (c) Convert 147.2 kpa to torr. Solution Analyze In each case we are given the pressure
More informationMolar Mass of Butane
Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures
More informationTemperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1
Answers Additional Questions 12.1 1. A gas collected over water has a total pressure equal to the pressure of the dry gas plus the pressure of the water vapor. If the partial pressure of water at 25.0
More informationPhysics Courseware Physics I Ideal Gases
Physics Courseware Physics I Ideal Gases Problem 1. How much mass of helium is contained in a 0.0 L cylinder at a pressure of.0 atm and a temperature of.0 C? [The atomic mass of helium is 4 amu] PV (
More informationThe Gas, Liquid, and Solid Phase
The Gas, Liquid, and Solid Phase When are interparticle forces important? Ron Robertson Kinetic Theory A. Principles Matter is composed of particles in constant, random, motion Particles collide elastically
More informationAbbreviations Conversions Standard Conditions Boyle s Law
Gas Law Problems Abbreviations Conversions atm  atmosphere K = C + 273 mmhg  millimeters of mercury 1 cm 3 (cubic centimeter) = 1 ml (milliliter) torr  another name for mmhg 1 dm 3 (cubic decimeter)
More informationWed Sep 12, 2007 THE GASEOUS STATE
Chapter 5: Gases Gas Stoichiometry Partial Pressure Kinetic Theory Effusion and Diffusion Wed Sep 12, 2007 Exam #1  Friday, Sep 14 Attendance is mandatory! Practice exam today in recitation Week 3 CHEM
More informationGeneral Properties of Gases. Properties of Gases. K is for Kelvin. C is for degrees Celsius. F is for degrees Fahrenheit PROPERTIES OF GASES GAS LAWS
PROPERTIES OF GASES or GAS LAWS 1 General Properties of Gases There is a lot of empty space in a gas. Gases can be expanded infinitely. Gases fill containers uniformly and completely. Gases diffuse and
More informationESSAY. Write your answer in the space provided or on a separate sheet of paper.
Test 1 General Chemistry CH116 Summer, 2012 University of Massachusetts, Boston Name ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Sodium hydride reacts with excess
More informationCHEM 1411, chapter 5 exercises
CHEM 1411, chapter 5 exercises 1. A gasfilled balloon with a volume of 12.5 L at 0.90 atm and 21 C is allowed to rise to the stratosphere where the temperature is 5 C and the pressure is 1.0 millibar.
More informationLiquid phase. Balance equation Moles A Stoic. coefficient. Aqueous phase
STOICHIOMETRY Objective The purpose of this exercise is to give you some practice on some Stoichiometry calculations. Discussion The molecular mass of a compound is the sum of the atomic masses of all
More informationAn increase in temperature causes an increase in pressure due to more collisions.
SESSION 7: KINETIC THEORY OF GASES Key Concepts In this session we will focus on summarising what you need to know about: Kinetic molecular theory Pressure, volume and temperature relationships Properties
More informationMolar Mass of Butane
Suggested reading: Chang 10 th edition text pages 175201 Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine
More information87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X
HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below
More informationChapter 13 Gases. An Introduction to Chemistry by Mark Bishop
Chapter 13 Gases An Introduction to Chemistry by Mark Bishop Chapter Map Gas Gas Model Gases are composed of tiny, widelyspaced particles. For a typical gas, the average distance between particles is
More informationExploring Gas Laws. Chapter 12. Solutions for Practice Problems. Student Textbook page 477
Chapter 12 Exploring Gas Laws Solutions for Practice Problems Student Textbook page 477 1. Problem At 19 C and 100 kpa, 0.021 mol of oxygen gas, O 2(g), occupy a volume of 0.50 L. What is the molar volume
More informationCHEMISTRY. Stoichiometry
Stoichiometry 1gram molecular mass 6.022 x 10 23 molecules Avagadro No of particles 6.022 x 10 23 particles MOLE 1 gram atomic mass 6.022 x 10 23 atoms Molar volume 22.4dm 3 at STP Equivalent mass of an
More informationGas Laws. vacuum. 760 mm. air pressure. mercury
Gas Laws Some chemical reactions take place in the gas phase and others produce products that are gases. We need a way to measure the quantity of compounds in a given volume of gas and relate that to moles.
More information1.23 Gas Calculations
1.23 Gas Calculations Gas calculations at Alevel are done in two different ways although both link the volumes of a gas to the amount in moles of the gas. The same amount in moles of any gas will have
More informationREVIEW QUESTIONS Chapter 5. 1. Determine the pressure of the gas (in mmhg) in the diagram below, given atmospheric pressure= 0.975 atm.
Chemistry 101 ANSWER KEY REVIEW QUESTIONS Chapter 5 1. Determine the pressure of the gas (in mmhg) in the diagram below, given atmospheric pressure= 0.975 atm. atm = 0.975 atm h = 5 cmhg gas atm 760 mmhg
More informationPhysics Notes Class 11 CHAPTER 13 KINETIC THEORY
1 P a g e Physics Notes Class 11 CHAPTER 13 KINETIC THEORY Assumptions of Kinetic Theory of Gases 1. Every gas consists of extremely small particles known as molecules. The molecules of a given gas are
More informationName Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.
Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kineticmolecular
More informationGas Density. Lift GOODYEAR. Goodyear blimp filled with He gas BADYEAR. Weight. Badyear blimp filled with Cl 2 gas
Gas Density Lift GOODYEAR Goodyear blimp filled with He gas BADYEAR Weight Badyear blimp filled with Cl 2 gas At STP( 1.00 atm, 273 K) 1.00 mole gas = 22.4 L Gas density: d = mass/volume = molar mass/molar
More information**VII1 C NC *VII2 C NC I2 C NC I3 C NC I4 C NC II1 C NC II2 C NC II3 C NC IV1 C NC IV2 C NC VIII1 C NC
**VII1 N *VII2 N I2 N I3 N I4 N II1 N II2 N II3 N IV1 N IV2 N VIII1 N EMISTRY 13101 Quiz 5 Spring 2013 Form B NAME: Key hapter 11: States of Matter A. (2 pts) onsider the structures of the
More informationThe Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon12? Molar Mass of Atoms 3/1/2015
The Mole Chapter 10 1 Objectives Use the mole and molar mass to make conversions among moles, mass, and number of particles Determine the percent composition of the components of a compound Calculate empirical
More informationEXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor
EXPERIMENT 15: 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 informationb. As you draw a vacuum in your mouth, atmospheric pressure pushing on the surface of the liquid forces the liquid up the straw.
CHAPTER FIVE Questions 16. a. Heating the can will increase the pressure of the gas inside the can, P T, V and n constant. As the pressure increases, it may be enough to rupture the can. b. As you draw
More informationVersion 001 HW03Non Ideal, Gas Mixtures & KMT vandenbout (52130) 1. = torr
Version 001 HW03Non Ideal, Gas Mixtures & KMT vandenbout (52130) 1 This printout should have 20 questions. Multiplechoice questions may continue on the next column or page find all choices before answering.
More informationStoichiometry V = 9.98 L CO2. 34.0 ml H 2 SO 4 soln 6.0 mol H 2 SO. 1000 ml H 2 SO 4 soln. 2 mol CO = 0.408 mol CO 2 1 mol H 2 SO 4
Stoichiometry We cannot count molecules so instead we weigh them; however, it is etremely inconvenient to weigh gases. So, when adding gases to a reaction how do we measure the amount of gas? We use the
More informationStoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.
Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven
More informationSTOICHIOMETRY STOICHIOMETRY. Measurements in Chemical Reactions. MoleMole Relationships. MassMass Problem. MoleMole Relationships
STOICHIOMETRY STOICHIOMETRY The analysis of the quantities of substances in a chemical reaction. Stoichiometric calculations depend on the MOLE MOLE relationships of substances. Measurements in Chemical
More informationChapter 5 Gases. August 2, 2009 [PROBLEM SET FROM R. CHANG TEST BANK] Student:
Chapter 5 Gases Student: 1. A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm 3 ; the density of water
More informationChemistry Final Exam Review
Name: Date: Block: Chemistry Final Exam Review 20122013 Unit 1: Measurement, Numbers, Scientific Notation, Conversions, Dimensional Analysis 1. Write 0.000008732 in scientific notation 8.732x106 2. Write
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
General Chemistry PHS 1015 Practice Exam 4 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following statements about pressure
More informationTemperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero 273 o C 0 K
Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero 273 o C 0 K Kinetic Molecular Theory of Gases 1. Large number of atoms/molecules in random motion 2.
More information10. Gases. P= g h Pressure. Pressure is defined as the force across a unit area. Force N
0. Gases 0. ressure ressure is defined as the force across a unit area. Force N ascal, a Area m In chemistry, the SI unit for pressure, the ascal (a), is typically too small to be of practical use. Typically
More information6 Evaluation of the Gas Law Constant
6 Evaluation of the Gas Law Constant Name: Date: Section: Objectives Measure the value of the gas constant R Use Dalton s Law to calculate the partial pressure of hydrogen in a closed container Learn to
More informationChemistry 110 Lecture Unit 5 Chapter 11GASES
Chemistry 110 Lecture Unit 5 Chapter 11GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all
More information4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.
1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.
More information1. Balance the following equation. What is the sum of the coefficients of the reactants and products?
1. Balance the following equation. What is the sum of the coefficients of the reactants and products? 1 Fe 2 O 3 (s) + _3 C(s) 2 Fe(s) + _3 CO(g) a) 5 b) 6 c) 7 d) 8 e) 9 2. Which of the following equations
More informationAP CHEMISTRY 2009 SCORING GUIDELINES (Form B)
AP CHEMISTRY 2009 SCORING GUIDELINES (Form B) Question 3 (10 points) 2 H 2 O 2 (aq) 2 H 2 O(l) + O 2 (g) The mass of an aqueous solution of H 2 O 2 is 6.951 g. The H 2 O 2 in the solution decomposes completely
More informationExample Problems. PV nt =R so P i. V i n i T i. = P f V f n f T f. (since V and n are constant) = P f T f. T i
The temperature of 2.5 L of a gas initially at STP is raised to 250 o C at constant volume. Calculate the final pressure of the gas in atm. PV nt =R so P i V i n i T i = P f V f n f T f or P i T i = P
More informationCHAPTER 25 IDEAL GAS LAWS
EXERCISE 139, Page 303 CHAPTER 5 IDEAL GAS LAWS 1. The pressure of a mass of gas is increased from 150 kpa to 750 kpa at constant temperature. Determine the final volume of the gas, if its initial volume
More informationProblem Set 2 Solutions
Chemistry 360 Dr. Jean M. Standard roblem Set Solutions 1. The atmospheric surface pressure on Venus is 90 bar. The atmosphere near the surface is composed of 96% carbon dioxide and 4% other gases. Given
More informationVersion 001 HW04Ideal Gas Laws, Gas Mixtures and KMT sparks (52100) 1
Version 001 HW04Ideal Gas Laws, Gas Mixtures and KMT sparks (52100) 1 This printout should have 15 questions. Multiplechoice questions may continue on the next column or page find all choices before
More informationEXPERIMENT 9 Evaluation of the Universal Gas Constant, R
Outcomes EXPERIMENT 9 Evaluation of the Universal Gas Constant, R After completing this experiment, the student should be able to: 1. Determine universal gas constant using reaction of an acid with a metal.
More informationCHEM 120 Online Chapter 7
CHEM 120 Online Chapter 7 Date: 1. Which of the following statements is not a part of kinetic molecular theory? A) Matter is composed of particles that are in constant motion. B) Particle velocity increases
More informationChemical Equilibrium. Rate Forward Reaction = Rate Reverse Reaction. Chapter 14. Hill, Petrucci, McCreary & Perry 4 th. Ed.
Chapter 14 Chemical Equilibrium Hill, Petrucci, McCreary & Perry 4 th Ed. Chemical Equilibrium Many Reactions seem to STOP before all the reactants are used up. The Concentrations of Reactants and Products
More informationChemistry 13: States of Matter
Chemistry 13: States of Matter Name: Period: Date: Chemistry Content Standard: Gases and Their Properties The kinetic molecular theory describes the motion of atoms and molecules and explains the properties
More informationThe gas laws Equations of state The state of any sample of substance is specified by giving the values of the following properties: V the volume the
The gas laws Equations of state The state of any sample of substance is specified by giving the values of the following properties: V the volume the sample occupies p the pressure of the sample T the temperature
More information5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C
1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )
More informationCHEMICAL EQUILIBRIUM (ICE METHOD)
CHEMICAL EQUILIBRIUM (ICE METHOD) Introduction Chemical equilibrium occurs when opposing reactions are proceeding at equal rates. The rate at which the products are formed from the reactants equals the
More informationMole Notes.notebook. October 29, 2014
1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the
More informationEXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES
Name Section EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES PRELABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to
More information1. Which graph shows the pressuretemperature relationship expected for an ideal gas? 1) 3)
1. Which graph shows the pressuretemperature relationship expected for an ideal gas? 2. Under which conditions does a real gas behave most like an ideal gas? 1) at low temperatures and high pressures
More informationDETERMINING THE MOLAR MASS OF CARBON DIOXIDE
DETERMINING THE MOLAR MASS OF CARBON DIOXIDE PURPOSE: The goal of the experiment is to determine the molar mass of carbon dioxide and compare the experimentally determined value to the theoretical value.
More informationThermal Properties of Matter
Chapter 18 Thermal Properties of Matter PowerPoint Lectures for University Physics, Thirteenth Edition Hugh D. Young and Roger A. Freedman Lectures by Wayne Anderson Goals for Chapter 18 To relate the
More informationK + Cl  Metal M. Zinc 1.0 M M(NO
Redox and Electrochemistry This section should be fresh in your minds because we just did this section in the text. Closely related to electrochemistry is redox chemistry. Count on at least one question
More information