I 2 (g) 2I(g) 0.12 g 254 g mol 1 = mol
|
|
- Ethelbert Sharp
- 7 years ago
- Views:
Transcription
1 hermodynamics: Examples for chapter When 0.12 g of solid iodine was vaporized at 1670 K, the resulting gas displaced 20.2 cm 3 of dry air at 298 K and 99.9 kpa pressure. How many iodine molecules were dissociated (i.e. as atomic iodine) in the gas? he gas phase equilibrium reaction is: I 2 (g) 2I(g) Assume that the gas mixture (of I 2 and I) behave according to the ideal gas law. he amount of I 2 before any dissociation takes place is: n = m M I2 = 0.12 g 254 g mol 1 = mol After the equilibrium has been reached, the amount of I 2 is (1 α)n and the amount of I is 2αn. Here the degree of dissociation is denoted by α. he ideal gas law is: PV = n tot R n tot = PV R n tot = (1 α)n + 2αn = PV R α = PV nr 1 = PV M I 2 mr 1 = (99.9 kn m 2 ) ( m 3 ) (254 g mol 1 ) (0.12 g) (8.31 J K 1 mol 1 1 = 0.72 ) (298 K) he amount of I is 2αn = ( mol) = mol. 1
2 2. What is the molar volume of n-hexane at 660 K and 91 bar according to (a) the ideal gas law and (b) the van der Waals equation? For n- hexane, c = K and P c = 30.3 bar. If you obtain an equation that you cannot solve analytically, attempt to solve it numerically. a) b) V = R P = ( L bar K 1 mol 1 )(660 K) = 0.603L mol 1 91 bar a = 27R2 c 2 = 27( L bar K 1 mol 1 ) 2 (507.7 K) 2 64P c 64(30.3 bar) b = R c = ( L bar K 1 mol 1 )(507.7 K) 8P c 30.3 bar P = R V b ā V 2 = L 2 bar mol 2 = L mol 1 est values for V and see when you get 91 bars: V = 0.39 L mol 1. his equation can also be solved by Maxima: a : 24.81; b : 0.174; R : ; : 660; P : 91; r : solve(p = R*/(V - b) - a/(v*v), V); float(r); his shows three roots of which only one is real (two are complex). he last line converts the complicated algebraic form to numerical values. 2
3 3. en grams of N 2 is mixed with 5 g of O 2 and held at 25 C and bar. (a) What are the partial pressures of N 2 and O 2? (b) What is the volume of the ideal mixture? a) n N2 = n O2 = 10 g 1 = mol g mol 5 g 1 = mol g mol mol y N2 = = mol 0.513mol mol y O2 = = mol 0.513mol P N2 = (0.750 bar) = bar P O2 = (0.750 bar) = bar b) V = nr P = (0.513 mol)( L bar K 1 mol 1 )( K) bar = L 4. Calculate dz/dp for a real gas in the limit P 0 using the virial equation. Z = 1 + B P + C P dz ( ) dz dp = B + 2C P +... = B dp P 0 3
4 5. he critical temperature of gaseous ammonia is 406 K and the critical pressure is 113 bar. Use the van der Waals equation to predict its molar volume at 273 K and 1 bar. Hint: Calculate first the coefficients a and b, then write the equation for the molar volume: V = R +b. Guess P+a/ V 2 an initial value for the molar volume and obtain a new value from the equation. Place the obtained value in the equation again to get a new value. Repeat this procedure until the value does not change anymore. his is an example of iterative methods for solving equations. Use the following equations derived in the lecture notes: a = 27R2 2 c 64P c and b = R c 8P c his gives a = 425 L 2 kpa mol 2 and b = L mol 1. Use the above equation and iterate until you get convergence: V = L mol Derive the expressions for V c, c and P c in terms of the van der Waals constants a and b. he equations in the lecture notes can be rewritten as (the definition of critical point and the equation of state): R c ( Vc b ) 2 = 2a V 3 c 2R c ( Vc b ) 3 = 6a V 4 c P c = R c V c b ā V 2 c Division of the first equation by the second (side by side) yields V c = 3b. Substitution of this expression into the first equation above gives c = 4
5 8a. Substitution of the two previous equations into the last equation 27Rb above yields P c = a. Note that the van der Waals constants a and b 27b 2 are usually calculated using the critical temperature and pressure since they are typically known more accurately than the critical volume. 7. he isothermal compressibility κ of a gas is defined as: κ = 1 V P Calculate κ for a van der Waals gas using the method of implicit differentiation (with respect to P). Show that in the limit of infinite volume, it yields 1/P (the same result as the ideal gas law). Based on the lecture notes, the van der Waals equation can be written: ( P + ā V 2 ) ( V b ) = R Expand the left hand side and substitute V = V/n to get: nr = PV npb + n2 a V n3 ab V 2 Implicit differentiation with respect to P at constant gives (i.e., side by side): 0 = V + P Solving for ( ) V gives: P ( ) ( ) ( ) V nb n2 a V P V + 2n3 ab V 2 P V 3 P P = nb V P n 2 a/v 2 + 2n 3 ab/v 3 5
6 he definition of isothermal compressibility now gives (at last stage V is assumed to be large): κ = 1 V P = V nb PV n 2 a/v + 2n 3 ab/v 2 V PV = 1 P 8. he cubic expansion coefficient is defined by α = 1 V P Calculate the cubic expansion and isothermal compressibility coefficients for an ideal gas. For an ideal gas V = nr/p. he require partial derivatives are therefore: P = nr P and P = nr P 2 Using the definitions for α and κ (using PV = nr below): α = 1 V κ = 1 V P P = nr PV = nr nr = 1 = nr V P 2 = PV V P 2 = 1 P 9. A certain gas has the following equation of state: P = nr V nb 6
7 a) Calculate the following partial derivatives: ( ) P V and ( ) P V b) Show that the following relation holds for the mixed partial derivatives for this equation of state: ( ) ( ) 2 P 2 P = V V a) ( ) P V = nr (V nb) 2 and b) ( ) 2 P = nr V (V nb) 2 and ( ) P V = nr V nb ( ) 2 P = nr V (V nb) Calculate the compressibility factor Z for NH 3 (g) at 400 K and 50 bar by using the attached graph and the virial equation. By reading the value for B from the graph, using relation B = B/R, and the virial equation written in terms of P, we get: 1 + Z = 1 + B P +... = 1 + B R P +... ( L mol 1 ) ( bar L K 1 mol 1 (50 bar) = 0.85 )(400 K) 7
8 8
a) Use the following equation from the lecture notes: = ( 8.314 J K 1 mol 1) ( ) 10 L
hermodynamics: Examples for chapter 4. 1. One mole of nitrogen gas is allowed to expand from 0.5 to 10 L reversible and isothermal process at 300 K. Calculate the change in molar entropy using a the ideal
More informationProblem Set 3 Solutions
Chemistry 360 Dr Jean M Standard Problem Set 3 Solutions 1 (a) One mole of an ideal gas at 98 K is expanded reversibly and isothermally from 10 L to 10 L Determine the amount of work in Joules We start
More informationvap H = RT 1T 2 = 30.850 kj mol 1 100 kpa = 341 K
Thermodynamics: Examples for chapter 6. 1. The boiling point of hexane at 1 atm is 68.7 C. What is the boiling point at 1 bar? The vapor pressure of hexane at 49.6 C is 53.32 kpa. Assume that the vapor
More informationGases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline
Gases and Kinetic-Molecular 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 Volume-Pressure
More informationFinal Exam CHM 3410, Dr. Mebel, Fall 2005
Final Exam CHM 3410, Dr. Mebel, Fall 2005 1. At -31.2 C, pure propane and n-butane have vapor pressures of 1200 and 200 Torr, respectively. (a) Calculate the mole fraction of propane in the liquid mixture
More informationCHAPTER 12. Gases and the Kinetic-Molecular Theory
CHAPTER 12 Gases and the Kinetic-Molecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids
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 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 informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationChapter 13 - Chemical Equilibrium
Chapter 1 - Chemical Equilibrium Intro A. Chemical Equilibrium 1. The state where the concentrations of all reactants and products remain constant with time. All reactions carried out in a closed vessel
More informationProblem Set 4 Solutions
Chemistry 360 Dr Jean M Standard Problem Set 4 Solutions 1 Two moles of an ideal gas are compressed isothermally and reversibly at 98 K from 1 atm to 00 atm Calculate q, w, ΔU, and ΔH For an isothermal
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 informationk 2f, k 2r C 2 H 5 + H C 2 H 6
hemical Engineering HE 33 F pplied Reaction Kinetics Fall 04 Problem Set 4 Solution Problem. The following elementary steps are proposed for a gas phase reaction: Elementary Steps Rate constants H H f,
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 informationBoyle s law - For calculating changes in pressure or volume: P 1 V 1 = P 2 V 2. Charles law - For calculating temperature or volume changes: V 1 T 1
Common Equations Used in Chemistry Equation for density: d= m v Converting F to C: C = ( F - 32) x 5 9 Converting C to F: F = C x 9 5 + 32 Converting C to K: K = ( C + 273.15) n x molar mass of element
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 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 informationEquations of State. Equations of State (EoS)
Equations of State (EoS) Equations of State From molecular considerations, identify which intermolecular interactions are significant (including estimating relative strengths of dipole moments, polarizability,
More informationAnswer, Key Homework 6 David McIntyre 1
Answer, Key Homework 6 David McIntyre 1 This print-out should have 0 questions, check that it is complete. Multiple-choice questions may continue on the next column or page: find all choices before making
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 informationEXERCISES. 16. What is the ionic strength in a solution containing NaCl in c=0.14 mol/dm 3 concentration and Na 3 PO 4 in 0.21 mol/dm 3 concentration?
EXERISES 1. The standard enthalpy of reaction is 512 kj/mol and the standard entropy of reaction is 1.60 kj/(k mol) for the denaturalization of a certain protein. Determine the temperature range where
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 informationFugacity, Activity, and Standard States
Fugacity, Activity, and Standard States Fugacity of gases: Since dg = VdP SdT, for an isothermal rocess, we have,g = 1 Vd. For ideal gas, we can substitute for V and obtain,g = nrt ln 1, or with reference
More informationStatistical Mechanics, Kinetic Theory Ideal Gas. 8.01t Nov 22, 2004
Statistical Mechanics, Kinetic Theory Ideal Gas 8.01t Nov 22, 2004 Statistical Mechanics and Thermodynamics Thermodynamics Old & Fundamental Understanding of Heat (I.e. Steam) Engines Part of Physics Einstein
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 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 informationPV (0.775 atm)(0.0854 L) n = = = 0.00264 mol RT -1-1
catalyst 2 5 g ¾¾¾¾ 2 4 g 2 g DH298 = rxn DS298 C H OH( ) C H ( ) + H O( ) 45.5 kj/mol ; = 126 J/(K mol ) ethanol ethene water rxn 1 atm 760 torr PV (0.775 atm)(0.0854 L) n = = = 0.00264 mol RT -1-1 (0.08206
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 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 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 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 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 informationObjectives: 1. Be able to list the assumptions and methods associated with the Virial Equation of state.
Lecture #19 1 Lecture 19 Objectives: 1. Be able to list the assumptions and methods associated with the Virial Equation of state. 2. Be able to compute the second virial coefficient from any given pair
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 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 informationReview - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008
Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid
More informationThermodynamics of Mixing
Thermodynamics of Mixing Dependence of Gibbs energy on mixture composition is G = n A µ A + n B µ B and at constant T and p, systems tend towards a lower Gibbs energy The simplest example of mixing: What
More informationCHEMISTRY GAS LAW S WORKSHEET
Boyle s Law Charles Law Guy-Lassac'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 informationSo T decreases. 1.- Does the temperature increase or decrease? For 1 mole of the vdw N2 gas:
1.- One mole of Nitrogen (N2) has been compressed at T0=273 K to the volume V0=1liter. The gas goes through the free expansion process (Q = 0, W = 0), in which the pressure drops down to the atmospheric
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 informationIdeal Gas and Real Gases
Ideal Gas and Real Gases Lectures in Physical Chemistry 1 Tamás Turányi Institute of Chemistry, ELTE State roerties state roerty: determines the macroscoic state of a hysical system state roerties of single
More information) and mass of each particle is m. We make an extremely small
Umeå Universitet, Fysik Vitaly Bychkov Prov i fysik, Thermodynamics, --6, kl 9.-5. Hjälpmedel: Students may use any book including the textbook Thermal physics. Present your solutions in details: it will
More informationChapter 10. Can You... 1. draw the Lewis structure for a given covalently bonded molecule?
Chapter 10 Can You... 1. draw the Lewis structure for a given covalently bonded molecule? e.g. SF 6 and CH 3 Cl 2. identify and count the number of non-bonding and bonding domains within a given covalently
More informationFUNDAMENTALS OF ENGINEERING THERMODYNAMICS
FUNDAMENTALS OF ENGINEERING THERMODYNAMICS System: Quantity of matter (constant mass) or region in space (constant volume) chosen for study. Closed system: Can exchange energy but not mass; mass is constant
More informationINTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e
CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum
More informationProblem Solving. Stoichiometry of Gases
Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.
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 informationGuide to Chapter 13. Chemical Equilibrium
Guide to Chapter 13. Chemical Equilibrium We will spend five lecture days on this chapter. During the first class meeting we will focus on how kinetics makes a segue into equilibrium. We will learn how
More informationChapter 8: Quantities in Chemical Reactions
Ch 8 Page 1 Chapter 8: Quantities in Chemical Reactions Stoichiometry: the numerical relationship between chemical quantities in a balanced chemical equation. Ex. 4NH 3 + 5O 2 4NO + 6H 2 O The reaction
More informationF321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 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 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 kinetic-molecular
More information10 Cl atoms. 10 H2O molecules. 8.3 mol HCN = 8.3 mol N atoms 1 mol HCN. 2 mol H atoms 2.63 mol CH2O = 5.26 mol H atoms 1 mol CH O
Chem 100 Mole conversions and stoichiometry worksheet 1. How many Ag atoms are in.4 mol Ag atoms? 6.0 10 Ag atoms 4.4 mol Ag atoms = 1.46 10 Ag atoms 1 mol Ag atoms. How many Br molecules are in 18. mol
More informationChemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
More informationPhysics 5D - Nov 18, 2013
Physics 5D - Nov 18, 2013 30 Midterm Scores B } Number of Scores 25 20 15 10 5 F D C } A- A A + 0 0-59.9 60-64.9 65-69.9 70-74.9 75-79.9 80-84.9 Percent Range (%) The two problems with the fewest correct
More informationGibbs Free Energy and Chemical Potential. NC State University
Chemistry 433 Lecture 14 Gibbs Free Energy and Chemical Potential NC State University The internal energy expressed in terms of its natural variables We can use the combination of the first and second
More informationUnit 19 Practice. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: Unit 19 Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The first law of thermodynamics can be given as. A) E = q + w B) =
More informationProblem Set 1 3.20 MIT Professor Gerbrand Ceder Fall 2003
LEVEL 1 PROBLEMS Problem Set 1 3.0 MIT Professor Gerbrand Ceder Fall 003 Problem 1.1 The internal energy per kg for a certain gas is given by U = 0. 17 T + C where U is in kj/kg, T is in Kelvin, and C
More informationIB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
More informationPhase Equilibrium: Fugacity and Equilibrium Calculations. Fugacity
Phase Equilibrium: Fugacity and Equilibrium Calculations (FEC) Phase Equilibrium: Fugacity and Equilibrium Calculations Relate the fugacity and the chemical potential (or the partial molar Gibbs free energy)
More informationCHAPTER 14 CHEMICAL EQUILIBRIUM
CHATER 14 CHEMICAL EQUILIBRIUM roblem Categories Biological: 14.98. Conceptual: 14.1, 14., 14.9, 14.5, 14.54, 14.55, 14.56, 14.57, 14.58, 14.59, 14.60, 14.61, 14.6, 14.66, 14.67, 14.68, 14.69, 14.81, 14.91,
More informationStates of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided.
CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. ideal gas
More informationReporting: one report / group. The results of the carryover load calculations will also be reported to Metsä Fibre, Rauma.
Carryover load Your task is to use the obtained experimental result from the probe measurement in combination with the information given in this handout to calculate the carryover load (g/nm 3 dry flue
More information10.7 Kinetic Molecular Theory. 10.7 Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory
The first scheduled quiz will be given next Tuesday during Lecture. It will last 5 minutes. Bring pencil, calculator, and your book. The coverage will be pp 364-44, i.e. Sections 0.0 through.4. 0.7 Theory
More information1.4.6-1.4.8 Gas Laws. Heat and Temperature
1.4.6-1.4.8 Gas Laws Heat and Temperature Often the concepts of heat and temperature are thought to be the same, but they are not. Perhaps the reason the two are incorrectly thought to be the same is because
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 informationThermodynamics. Chapter 13 Phase Diagrams. NC State University
Thermodynamics Chapter 13 Phase Diagrams NC State University Pressure (atm) Definition of a phase diagram A phase diagram is a representation of the states of matter, solid, liquid, or gas as a function
More information3.3. Solving Polynomial Equations. Introduction. Prerequisites. Learning Outcomes
Solving Polynomial Equations 3.3 Introduction Linear and quadratic equations, dealt within Sections 3.1 and 3.2, are members of a class of equations, called polynomial equations. These have the general
More informationCalculating Atoms, Ions, or Molecules Using Moles
TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary
More informationTHE IDEAL GAS LAW AND KINETIC THEORY
Chapter 14 he Ideal Gas Law and Kinetic heory Chapter 14 HE IDEAL GAS LAW AND KINEIC HEORY REIEW Kinetic molecular theory involves the study of matter, particularly gases, as very small particles in constant
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More informationCHAPTER 14 THE CLAUSIUS-CLAPEYRON EQUATION
CHAPTER 4 THE CAUIU-CAPEYRON EQUATION Before starting this chapter, it would probably be a good idea to re-read ections 9. and 9.3 of Chapter 9. The Clausius-Clapeyron equation relates the latent heat
More informationSample Problem: STOICHIOMETRY and percent yield calculations. How much H 2 O will be formed if 454 g of. decomposes? NH 4 NO 3 N 2 O + 2 H 2 O
STOICHIOMETRY and percent yield calculations 1 Steps for solving Stoichiometric Problems 2 Step 1 Write the balanced equation for the reaction. Step 2 Identify your known and unknown quantities. Step 3
More informationStoichiometry. What is the atomic mass for carbon? For zinc?
Stoichiometry Atomic Mass (atomic weight) Atoms are so small, it is difficult to discuss how much they weigh in grams We use atomic mass units an atomic mass unit (AMU) is one twelfth the mass of the catbon-12
More informationExergy: the quality of energy N. Woudstra
Exergy: the quality of energy N. Woudstra Introduction Characteristic for our society is a massive consumption of goods and energy. Continuation of this way of life in the long term is only possible if
More informationChapter 4: Chemical and Solution Stoichiometry
Chapter 4: Chemical and Solution Stoichiometry (Sections 4.1-4.4) 1 Reaction Stoichiometry The coefficients in a balanced chemical equation specify the relative amounts in moles of each of the substances
More informationHow To Calculate Mass In Chemical Reactions
We have used the mole concept to calculate mass relationships in chemical formulas Molar mass of ethanol (C 2 H 5 OH)? Molar mass = 2 x 12.011 + 6 x 1.008 + 1 x15.999 = 46.069 g/mol Mass percentage of
More information11 Thermodynamics and Thermochemistry
Copyright ç 1996 Richard Hochstim. All rights reserved. Terms of use.» 37 11 Thermodynamics and Thermochemistry Thermodynamics is the study of heat, and how heat can be interconverted into other energy
More informationChemistry 101 Generating Hydrogen Gas
Chemistry 101 Generating Hydrogen Gas Objectives To experimentally verify the molar volume of hydrogen gas at STP To gain experience in collecting gas over water Discussion The molar volume of a gas is
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
More informationIDEAL AND NON-IDEAL GASES
2/2016 ideal gas 1/8 IDEAL AND NON-IDEAL GASES PURPOSE: To measure how the pressure of a low-density gas varies with temperature, to determine the absolute zero of temperature by making a linear fit to
More informationCLASS TEST GRADE 11. PHYSICAL SCIENCES: CHEMISTRY Test 6: Chemical change
CLASS TEST GRADE PHYSICAL SCIENCES: CHEMISTRY Test 6: Chemical change MARKS: 45 TIME: hour INSTRUCTIONS AND INFORMATION. Answer ALL the questions. 2. You may use non-programmable calculators. 3. You may
More informationChapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass
More informationName Class Date. F 2 2269 N A 1 88.12 cm 2 A 2 1221 cm 2 Unknown: Step 2: Write the equations for Pascal s principle and pressure, force, and area.
Skills Worksheet Math Skills Pascal s Principle After you study each sample problem and solution, work out the practice problems on a separate sheet of paper. Write your answers in the spaces provided.
More informationChapter 8 Maxwell relations and measurable properties
Chapter 8 Maxwell relations and measurable properties 8.1 Maxwell relations Other thermodynamic potentials emerging from Legendre transforms allow us to switch independent variables and give rise to alternate
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 informationCH3 Stoichiometry. The violent chemical reaction of bromine and phosphorus. P.76
CH3 Stoichiometry The violent chemical reaction of bromine and phosphorus. P.76 Contents 3.1 Counting by Weighing 3.2 Atomic Masses 3.3 The Mole 3.4 Molar Mass 3.5 Percent Composition of Compounds 3.6
More informationPhys222 W11 Quiz 1: Chapters 19-21 Keys. Name:
Name:. In order for two objects to have the same temperature, they must a. be in thermal equilibrium.
More informationneutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
More informationChem 420/523 Chemical Thermodynamics Homework Assignment # 6
Chem 420/523 Chemical hermodynamics Homework Assignment # 6 1. * Solid monoclinic sulfur (S α ) spontaneously converts to solid rhombic sulfur (S β ) at 298.15 K and 0.101 MPa pressure. For the conversion
More informationEquilibrium. Ron Robertson
Equilibrium Ron Robertson Basic Ideas A. Extent of Reaction Many reactions do not go to completion. Those that do not are reversible with a forward reaction and reverse reaction. To be really correct we
More informationKeystone Exams: Chemistry Assessment Anchors and Eligible Content. Pennsylvania Department of Education www.education.state.pa.
Assessment Anchors and Pennsylvania Department of Education www.education.state.pa.us 2010 PENNSYLVANIA DEPARTMENT OF EDUCATION General Introduction to the Keystone Exam Assessment Anchors Introduction
More informationTHE KINETIC THEORY OF GASES
Chapter 19: THE KINETIC THEORY OF GASES 1. Evidence that a gas consists mostly of empty space is the fact that: A. the density of a gas becomes much greater when it is liquefied B. gases exert pressure
More informationStoichiometry and Aqueous Reactions (Chapter 4)
Stoichiometry and Aqueous Reactions (Chapter 4) Chemical Equations 1. Balancing Chemical Equations (from Chapter 3) Adjust coefficients to get equal numbers of each kind of element on both sides of arrow.
More informationb. Calculate the value of the equilibrium constant at 127ºC for the reaction 2NH 3 (g) N 2 (g) + 3H 2 (g)
1. Write the equilibrium expression for the following reaction: 4NH 3 (g) + 7O 2 (g) 4NO 2 (g) + 6H 2 O(g) 2. The following equilibrium concentrations were observed for this reaction at 127ºC: N 2 (g)
More informationGive all answers in MKS units: energy in Joules, pressure in Pascals, volume in m 3, etc. Only work the number of problems required. Chose wisely.
Chemistry 45/456 0 July, 007 Midterm Examination Professor G. Drobny Universal gas constant=r=8.3j/mole-k=0.08l-atm/mole-k Joule=J= Nt-m=kg-m /s 0J= L-atm. Pa=J/m 3 =N/m. atm=.0x0 5 Pa=.0 bar L=0-3 m 3.
More informationCalorimetry: Heat of Vaporization
Calorimetry: Heat of Vaporization OBJECTIVES INTRODUCTION - Learn what is meant by the heat of vaporization of a liquid or solid. - Discuss the connection between heat of vaporization and intermolecular
More informationIntermolecular Forces
Intermolecular Forces: Introduction Intermolecular Forces Forces between separate molecules and dissolved ions (not bonds) Van der Waals Forces 15% as strong as covalent or ionic bonds Chapter 11 Intermolecular
More informationCalculations with Chemical Formulas and Equations
Chapter 3 Calculations with Chemical Formulas and Equations Concept Check 3.1 You have 1.5 moles of tricycles. a. How many moles of seats do you have? b. How many moles of tires do you have? c. How could
More informationChapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)
Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H
More information