CHAPTER 27 SPECIFIC HEAT CAPACITIES OF GASES
|
|
- Ann Bryan
- 7 years ago
- Views:
Transcription
1 HATE 7 SEIFI HEAT AAITIES OF GASES. N mole, W g/mol, m/s K.E. of the vessel Internal energy of the gas (/) mv (/) J n r(t) 8. T T k. 8.. m g, t.7 cal/g- J. J/al. dq du + dw Now, (for a rigid body) So, dw. So dq du. Q msdt cal Joule..., w or piston kg., A of piston cm o kpa, g m/s, x cm. mg dw pdv oadx A ndt dt n. J. n dq npdt np n ( ) n.. J.. H. al/g, H. al/g M g/ Mol, 8. 7 erg/mol- We know, al/g So, difference of molar specific heats M M al/g Now, J J 8. 7 erg/mol- J. 7 erg/cal.. 7.6, n mole, T K (a) Keeping the pressure constant, dq du + dw, T K, 7/6, m mole, dq du + dw n dt du + dt du npdt dt 7 dt dt 6 dt dt 7 6 DT dt 7dT dt 6 dt J. (b) Kipping olume constant, dv n dt dt J (c) Adiabetically dq, du dw n 8. T T T T J
2 6. m.8 g, cm L T k, a nt or n N T 8. atm. T Q Now, v.6 9. n dt p + v Specific Heat apacities of Gases Q n p dt.87.8 al cm, cm a, Q J (a) Q du + dw du + ( 6 ) du + du J (b) n 8. [ U nt for monoatomic] n (c) du n v dt v dndtu p v (d) v. (roved above) 8. Q Amt of heat given.8. Work done Q, Q W + U for monoatomic gas U Q Q Q n T Q nt nt Again Q n pdt Where > Molar heat capacity at const. pressure. nt ndt nt 9. K K T K T T K U dv K. dq du + dw mcdt dt + pdv msdt dt+ ms + K + K,, b dv dt b dt + dt b + r, b + b 7. df K. onsidering two gases, in Gas() we have,, p (Sp. Heat at const. ), v (Sp. Heat at const. ), n (No. of moles) p & p v v
3 v v v ( ) v & p Specific Heat apacities of Gases In Gas() we have,, p (Sp. Heat at const. ), v (Sp. Heat at const. ), n (No. of moles) p & p v v v v ( ) v v Given n : n : du nv dt & du nv dt nvdt v v r &p v () p So, [from () & ()] v ( ) () & p. p. p. v. v. n n mol (n + n ) dt n v dt + n v dt nv nv.. n n + + p.. n mole, J/mol-k, (a) Temp at A T a, a a nt a 6 T a a a k. n Similarly temperatures at point b k at it is 8 k and at D it is k. (b) For ab process, dq npdt [since ab is isobaric] T b T a ( ) 9 J For bc, dq du + dw [dq, Isochorie process] n dq du n v dt T c T a () J (c) Heat liberated in cd n p dt n T d T c Heat liberated in da n v dt T a T d J ( ) 7 J Ka Ka a d Ta Td cm Tc c b Tb cm 7.
4 . (a) For a, b is constant So, T T For b,c is constant So, T T 6 T T T T 6 6 k 9 k Specific Heat apacities of Gases (b) Work done Area enclosed under the graph cc kpa 6 J J (c) Q Supplied n v dt Now, n considering at pt. b T v Q bc dt a, b. 6 dt T 6.67 Q supplied to be n p dt [ p ] 6.9 (.67) dt.9 T (d) Q U + w Now, U Q w Heat supplied Work done (.9 +.9) 9.8. In Joly s differential steam calorimeter v ml m ( ) m Mass of steam condensed.9 g, L al/g. J/g m Mass of gas present g,,.9. v.89.9 J/g-K ( ) 6.. Since it is an adiabatic process, So const. (a) (b) T onst. T T Given L, L,..96. T T 7.. a, cc, T k (a).....? (b) T T (). T (). T. k k 7.7 cm c cm a b Ka Ka 7.
5 (c) Work done by the gas in the process m T T T( ) W T T 6.. [ ].7 J (, ). 8.., T 9 k, atm, p atm We know for adiabatic process, T T or (). (9). ().. T (). (9). T..78 T. T (.78) /.. K 9. Ka a, cm 6 m, T k,. (a) Suddenly compressed to cm (). (). (). 8 Ka Specific Heat apacities of Gases T T (). T ().- T 6 K (b) Even if the container is slowly compressed the walls are adiabatic so heat transferred is. Thus the values remain, 8 Ka, T 6 K.. Given (Initial ressure), (Initial olume) (a) (i) Isothermal compression, or, (ii) Adiabatic ompression or o + (b) (i) Adiabatic compression or (ii) Isothermal compression or. Initial pressure Initial olume (a) Isothermally to pressure + Adiabetically to pressure ( ) ( ) + (+)/ Final olume (+)/ 7.
6 Specific Heat apacities of Gases (b) Adiabetically to pressure to ( + ) () Isothermal to pressure / (+)/ Final olume (+)/. nt Given Ka a, cm 6 m, T k (a) n T 8. (b) ( ) moles. 6.6 J/mole (c) Given Ka a,? cm 6 m,. cm 6 m, T k, T? Since the process is adiabatic Hence ( 6 ) ( 6 ) a 78 Ka (d) Q W + U or W U [U, in adiabatic] n dt ( ) J J (e) U n dt J. A B For A, the process is isothermal A A A A A For B, the process is adiabatic, A A A A A ( B ) A ( B ) B B B B B For,, the process is isobaric T T T T T Final pressures are equal. T. B. p A B. A : B : :. : : :. Initial ressure Initial olume Final ressure Final olume Given,, Isothermal workdone nt Ln 7.6
7 Specific Heat apacities of Gases Adiabatic workdone Given that workdone in both cases is same. Hence nt Ln ( )ln nt nt nt ( ) ln ( ) ln We know T const. in adiabatic rocess. T T, or T ( ) T () ( ) Or, T - T or T T (ii) From (i) & (ii) ( ) ln T T T ( ) ln T T T nt (i) [ ].., T k, Lv l (a) The process is adiabatic as it is sudden, ( ). (). / (b) Ka n a W [T T ] T (). T (.). T.. T nt n n w [T T ] K. T ( in m ) (. ). (c) Internal Energy, dq, du dw ( 8.8)J 8.8 J 8 J. (d) Final Temp.. k k. (e) The pressure is kept constant. The process is isobaric. 8.8 J 8 J. Work done ndt ( ) Final Temp K (.). J. Initial Temp (f) Initial volume Final volume L T T T Work done in isothermal ntln ln / T ln.9 (g) Net work done W A + W B + W J. L. 7.7
8 Specific Heat apacities of Gases 6. Given. We know fro adiabatic process T onst. So, T T (eq) As, it is an adiabatic process and all the other conditions are same. Hence the above equation can be applied. So, T. T.. T T. T. T So, T :T : 7. cm,. J/mol-k, T k, 7 cm (a) No. of moles of gas in each vessel, T 8. 7 (b) Heat is supplied to the gas but dv dq du n dt.8. dt dt for (A).8. For (B) dt.8. 7 A.8. A B A [For container A] T T A. 7. cm of Hg..8. B 7 [For ontainer B] B.8. B A cm of Hg. T T Mercury moves by a distance B A.. m. 8. mhe. g,.67, g/mol, mh? 8/mol. Since it is an adiabatic surrounding He dq n dt. dt. (.67 ) dt (i) m H n dt dt m. dt [Where m is the rqd. Mass of H ] Since equal amount of heat is given to both and T is same in both. Equating (i) & (ii) we get. m dt dt m g.67 A He / / T T / / T T : B H 9. Initial pressure, Initial Temperature T Initial olume (a) For the diathermic vessel the temperature inside remains constant A B, Temperature T o For adiabatic vessel the temperature does not remains constant. The process is adiabatic T T T T ( ) T T T T 7.8
9 p ( ) (b) When the values are opened, the temperature remains T through out nt +, nt ( n n )T [Total value after the expt + ] nt nt. For an adiabatic process, v onst. There will be a common pressure when the equilibrium is reached Hence For left For ight () ( ) () ( ) () Equating for both left & right or () ( ) / / Similarly / / / / / / / For right () / / / Specific Heat apacities of Gases For left.() (b) Since the whole process takes place in adiabatic surroundings. The separator is adiabatic. Hence heat given to the gas in the left part Zero. (c) From () Final pressure Again from () / / / ( ) or y / / /. A cm m, M. g. kg, atm pascal, L cm. m. L 8 cm.8 m,. atm The process is adiabatic / / () () (AL). (AL).. log log.9. / / T / / T.9 m / v m/s 7.9
10 Specific Heat apacities of Gases. 8 m/s, T, oh.89 kg/m, r 8. J/mol-k, At ST, a, We know sound Again, o J/mol-k.8 (8) (8).8 Again, or J/mol-k. g kg, cm 6 m cal/mol-ki. J/mol-k J/mol-k 8. ( ) (8.) 8. Since the condition is ST, atm pa m/s. Given o.7 g/cm.7 kg/m,. a, 8. J/mol-k,. KHz. Node separation in a Kundt tube 6 cm, cm m So, - 6 m/s We know, Speed of sound o (6)..7 (6) But J/mol-k Again So, J/mol-k. Hz, T Hz,. cm 6.6 m 6.6 (66 ) m/s m [v nt t M ot m T (66 ) m v J/mol-k, J/mol-k. o m T ] (66 ) 8. (66 )
Answer, 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 informationHEAT UNIT 1.1 KINETIC THEORY OF GASES. 1.1.1 Introduction. 1.1.2 Postulates of Kinetic Theory of Gases
UNIT HEAT. KINETIC THEORY OF GASES.. Introduction Molecules have a diameter of the order of Å and the distance between them in a gas is 0 Å while the interaction distance in solids is very small. R. Clausius
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 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 informationThe final numerical answer given is correct but the math shown does not give that answer.
Note added to Homework set 7: The solution to Problem 16 has an error in it. The specific heat of water is listed as c 1 J/g K but should be c 4.186 J/g K The final numerical answer given is correct but
More informationa) 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 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 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 informationHeat and Work. First Law of Thermodynamics 9.1. Heat is a form of energy. Calorimetry. Work. First Law of Thermodynamics.
Heat and First Law of Thermodynamics 9. Heat Heat and Thermodynamic rocesses Thermodynamics is the science of heat and work Heat is a form of energy Calorimetry Mechanical equivalent of heat Mechanical
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 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 informationChapter 18 Temperature, Heat, and the First Law of Thermodynamics. Problems: 8, 11, 13, 17, 21, 27, 29, 37, 39, 41, 47, 51, 57
Chapter 18 Temperature, Heat, and the First Law of Thermodynamics Problems: 8, 11, 13, 17, 21, 27, 29, 37, 39, 41, 47, 51, 57 Thermodynamics study and application of thermal energy temperature quantity
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 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 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 informationES-7A Thermodynamics HW 1: 2-30, 32, 52, 75, 121, 125; 3-18, 24, 29, 88 Spring 2003 Page 1 of 6
Spring 2003 Page 1 of 6 2-30 Steam Tables Given: Property table for H 2 O Find: Complete the table. T ( C) P (kpa) h (kj/kg) x phase description a) 120.23 200 2046.03 0.7 saturated mixture b) 140 361.3
More information= 800 kg/m 3 (note that old units cancel out) 4.184 J 1000 g = 4184 J/kg o C
Units and Dimensions Basic properties such as length, mass, time and temperature that can be measured are called dimensions. Any quantity that can be measured has a value and a unit associated with it.
More information18 Q0 a speed of 45.0 m/s away from a moving car. If the car is 8 Q0 moving towards the ambulance with a speed of 15.0 m/s, what Q0 frequency does a
First Major T-042 1 A transverse sinusoidal wave is traveling on a string with a 17 speed of 300 m/s. If the wave has a frequency of 100 Hz, what 9 is the phase difference between two particles on the
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 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 informationChapter 10 Temperature and Heat
Chapter 10 Temperature and Heat What are temperature and heat? Are they the same? What causes heat? What Is Temperature? How do we measure temperature? What are we actually measuring? Temperature and Its
More informationLecture 14 Chapter 19 Ideal Gas Law and Kinetic Theory of Gases. Chapter 20 Entropy and the Second Law of Thermodynamics
Lecture 14 Chapter 19 Ideal Gas Law and Kinetic Theory of Gases Now we to look at temperature, pressure, and internal energy in terms of the motion of molecules and atoms? Relate to the 1st Law of Thermodynamics
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 informationThermochemistry. r2 d:\files\courses\1110-20\99heat&thermorans.doc. Ron Robertson
Thermochemistry r2 d:\files\courses\1110-20\99heat&thermorans.doc Ron Robertson I. What is Energy? A. Energy is a property of matter that allows work to be done B. Potential and Kinetic Potential energy
More informationChapter 6 Thermodynamics: The First Law
Key Concepts 6.1 Systems Chapter 6 Thermodynamics: The First Law Systems, States, and Energy (Sections 6.1 6.8) thermodynamics, statistical thermodynamics, system, surroundings, open system, closed system,
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 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 informationexplain your reasoning
I. A mechanical device shakes a ball-spring system vertically at its natural frequency. The ball is attached to a string, sending a harmonic wave in the positive x-direction. +x a) The ball, of mass M,
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 informationState Newton's second law of motion for a particle, defining carefully each term used.
5 Question 1. [Marks 20] An unmarked police car P is, travelling at the legal speed limit, v P, on a straight section of highway. At time t = 0, the police car is overtaken by a car C, which is speeding
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. 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 information39th International Physics Olympiad - Hanoi - Vietnam - 2008. Theoretical Problem No. 3
CHANGE OF AIR TEMPERATURE WITH ALTITUDE, ATMOSPHERIC STABILITY AND AIR POLLUTION Vertical motion of air governs many atmospheric processes, such as the formation of clouds and precipitation and the dispersal
More informationmomentum change per impact The average rate of change of momentum = Time interval between successive impacts 2m x 2l / x m x m x 2 / l P = l 2 P = l 3
Kinetic Molecular Theory This explains the Ideal Gas Pressure olume and Temperature behavior It s based on following ideas:. Any ordinary sized or macroscopic sample of gas contains large number of molecules.
More informationThermodynamics AP Physics B. Multiple Choice Questions
Thermodynamics AP Physics B Name Multiple Choice Questions 1. What is the name of the following statement: When two systems are in thermal equilibrium with a third system, then they are in thermal equilibrium
More informationThe First Law of Thermodynamics
Thermodynamics The First Law of Thermodynamics Thermodynamic Processes (isobaric, isochoric, isothermal, adiabatic) Reversible and Irreversible Processes Heat Engines Refrigerators and Heat Pumps The Carnot
More informationEnergy Matters Heat. Changes of State
Energy Matters Heat Changes of State Fusion If we supply heat to a lid, such as a piece of copper, the energy supplied is given to the molecules. These start to vibrate more rapidly and with larger vibrations
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 informationKINETIC THEORY OF GASES AND THERMODYNAMICS SECTION I Kinetic theory of gases
KINETIC THEORY OF GASES AND THERMODYNAMICS SECTION I Kinetic theory of gases Some important terms in kinetic theory of gases Macroscopic quantities: Physical quantities like pressure, temperature, volume,
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 informationChem 338 Homework Set #5 solutions October 10, 2001 From Atkins: 5.2, 5.9, 5.12, 5.13, 5.15, 5.17, 5.21
Chem 8 Homework Set #5 solutions October 10, 2001 From Atkins: 5.2, 5.9, 5.12, 5.1, 5.15, 5.17, 5.21 5.2) The density of rhombic sulfur is 2.070 g cm - and that of monoclinic sulfur is 1.957 g cm -. Can
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 informationState Newton's second law of motion for a particle, defining carefully each term used.
5 Question 1. [Marks 28] An unmarked police car P is, travelling at the legal speed limit, v P, on a straight section of highway. At time t = 0, the police car is overtaken by a car C, which is speeding
More informationAP Chemistry 2009 Free-Response Questions Form B
AP Chemistry 009 Free-Response Questions Form B The College Board The College Board is a not-for-profit membership association whose mission is to connect students to college success and opportunity. Founded
More informationPHYS-2010: General Physics I Course Lecture Notes Section XIII
PHYS-2010: General Physics I Course Lecture Notes Section XIII Dr. Donald G. Luttermoser East Tennessee State University Edition 2.5 Abstract These class notes are designed for use of the instructor and
More information10.7 Kinetic Molecular Theory. 10.7 Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory
Week lectures--tentative 0.7 Kinetic-Molecular Theory 40 Application to the Gas Laws 0.8 Molecular Effusion and Diffusion 43 Graham's Law of Effusion Diffusion and Mean Free Path 0.9 Real Gases: Deviations
More informationThe first law: transformation of energy into heat and work. Chemical reactions can be used to provide heat and for doing work.
The first law: transformation of energy into heat and work Chemical reactions can be used to provide heat and for doing work. Compare fuel value of different compounds. What drives these reactions to proceed
More informationUnit 5 Practice Test. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: Unit 5 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The internal energy of a system is always increased by. A) adding
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 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 informationChapter 18 Homework Answers
Chapter 18 Homework Answers 18.22. 18.24. 18.26. a. Since G RT lnk, as long as the temperature remains constant, the value of G also remains constant. b. In this case, G G + RT lnq. Since the reaction
More informationDefine the notations you are using properly. Present your arguments in details. Good luck!
Umeå Universitet, Fysik Vitaly Bychkov Prov i fysik, Thermodynamics, 0-0-4, kl 9.00-5.00 jälpmedel: Students may use any book(s) including the textbook Thermal physics. Minor notes in the books are also
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 information01 The Nature of Fluids
01 The Nature of Fluids WRI 1/17 01 The Nature of Fluids (Water Resources I) Dave Morgan Prepared using Lyx, and the Beamer class in L A TEX 2ε, on September 12, 2007 Recommended Text 01 The Nature of
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 informationAP Chemistry 2009 Free-Response Questions
AP Chemistry 009 Free-Response Questions The College Board The College Board is a not-for-profit membership association whose mission is to connect students to college success and opportunity. Founded
More informationCHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)
CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26
More informationDetermination of the enthalpy of combustion using a bomb calorimeter TEC
Determination of the enthalpy of TEC Related concepts First law of thermodynamics, Hess s law of constant heat summation, enthalpy of combustion, enthalpy of formation, heat capacity. Principle The bomb
More informationChapter 28 Fluid Dynamics
Chapter 28 Fluid Dynamics 28.1 Ideal Fluids... 1 28.2 Velocity Vector Field... 1 28.3 Mass Continuity Equation... 3 28.4 Bernoulli s Principle... 4 28.5 Worked Examples: Bernoulli s Equation... 7 Example
More informationChapter 1 Classical Thermodynamics: The First Law. 1.2 The first law of thermodynamics. 1.3 Real and ideal gases: a review
Chapter 1 Classical Thermodynamics: The First Law 1.1 Introduction 1.2 The first law of thermodynamics 1.3 Real and ideal gases: a review 1.4 First law for cycles 1.5 Reversible processes 1.6 Work 1.7
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 informationJust another. Fuel Cell Formulary. by Dr. Alexander Kabza
Just another by Dr. Alexander Kabza This version is from July 16, 2015 and optimized for Smartphones. Latest version see www.kabza.de. Don t hesitate to send me any comments or failures or ideas by email!
More informationIntroduction to the Ideal Gas Law
Course PHYSICS260 Assignment 5 Consider ten grams of nitrogen gas at an initial pressure of 6.0 atm and at room temperature. It undergoes an isobaric expansion resulting in a quadrupling of its volume.
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 informationThermodynamics worked examples
An Introduction to Mechanical Engineering Part hermodynamics worked examles. What is the absolute ressure, in SI units, of a fluid at a gauge ressure of. bar if atmosheric ressure is.0 bar? Absolute ressure
More informationCLASSICAL CONCEPT REVIEW 8
CLASSICAL CONCEPT REVIEW 8 Kinetic Theory Information concerning the initial motions of each of the atoms of macroscopic systems is not accessible, nor do we have the computational capability even with
More informationDesign of heat exchangers
Design of heat exchangers Exchanger Design Methodology The problem of heat exchanger design is complex and multidisciplinary. The major design considerations for a new heat exchanger include: process/design
More informationME 201 Thermodynamics
ME 0 Thermodynamics Second Law Practice Problems. Ideally, which fluid can do more work: air at 600 psia and 600 F or steam at 600 psia and 600 F The maximum work a substance can do is given by its availablity.
More information13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects
Week 3 Sections 13.3-13.5 13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects 13.4 Ways of Expressing Concentration Mass Percentage, ppm, and ppb Mole Fraction,
More informationIntroductory Laboratory EST - Experiment 9 Calorimetry - 1 - Introductory Laboratory Energy Science and Technology. Experiment 9. Physical Chemistry
Introductory Laboratory EST - Experiment 9 Calorimetry - 1 - Introductory Laboratory Energy Science and Technology Experiment 9 Physical Chemistry Calorimetry Abstract The heat of combustion of Naphthalene
More informationWorksheet #17. 2. How much heat is released when 143 g of ice is cooled from 14 C to 75 C, if the specific heat capacity of ice is 2.087 J/(g C).
Worksheet #17 Calculating Heat 1. How much heat is needed to bring 12.0 g of water from 28.3 C to 43.87 C, if the specific heat capacity of water is 4.184 /(g? 2. How much heat is released when 143 g of
More informationAvailability. Second Law Analysis of Systems. Reading Problems 10.1 10.4 10.59, 10.65, 10.66, 10.67 10.69, 10.75, 10.81, 10.
Availability Readg Problems 10.1 10.4 10.59, 10.65, 10.66, 10.67 10.69, 10.75, 10.81, 10.88 Second Law Analysis of Systems AVAILABILITY: the theoretical maximum amount of reversible work that can be obtaed
More informationChem 1A Exam 2 Review Problems
Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?
More informationTechnical Thermodynamics
Technical Thermodynamics Chapter 2: Basic ideas and some definitions Prof. Dr.-Ing. habil. Egon Hassel University of Rostock, Germany Faculty of Mechanical Engineering and Ship Building Institute of Technical
More informationAP Chemistry 2010 Free-Response Questions Form B
AP Chemistry 010 Free-Response Questions Form B The College Board The College Board is a not-for-profit membership association whose mission is to connect students to college success and opportunity. Founded
More informationChemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES
Chemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES The learning objectives of this experiment are to explore the relationship between the temperature and vapor pressure of water. determine the molar
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 informationModule 5: Combustion Technology. Lecture 34: Calculation of calorific value of fuels
1 P age Module 5: Combustion Technology Lecture 34: Calculation of calorific value of fuels 2 P age Keywords : Gross calorific value, Net calorific value, enthalpy change, bomb calorimeter 5.3 Calculation
More informationAP Physics Course 1 Summer Assignment. Teachers: Mr. Finn, Mrs. Kelly, Mr. Simowitz, Mr. Slesinski
AP Physics Course 1 Summer Assignment Teachers: Mr. Finn, Mrs. Kelly, Mr. Simowitz, Mr. Slesinski On the following pages, there are six sections that use the basic skills that will be used throughout the
More informationCHEM 36 General Chemistry EXAM #1 February 13, 2002
CHEM 36 General Chemistry EXAM #1 February 13, 2002 Name: Serkey, Anne INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show
More informationwww.mathsbox.org.uk Displacement (x) Velocity (v) Acceleration (a) x = f(t) differentiate v = dx Acceleration Velocity (v) Displacement x
Mechanics 2 : Revision Notes 1. Kinematics and variable acceleration Displacement (x) Velocity (v) Acceleration (a) x = f(t) differentiate v = dx differentiate a = dv = d2 x dt dt dt 2 Acceleration Velocity
More informationHeat Exchangers - Introduction
Heat Exchangers - Introduction Concentric Pipe Heat Exchange T h1 T c1 T c2 T h1 Energy Balance on Cold Stream (differential) dq C = wc p C dt C = C C dt C Energy Balance on Hot Stream (differential) dq
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 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 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 informationStirling heat engine Internal combustion engine (Otto cycle) Diesel engine Steam engine (Rankine cycle) Kitchen Refrigerator
Lecture. Real eat Engines and refrigerators (Ch. ) Stirling heat engine Internal combustion engine (Otto cycle) Diesel engine Steam engine (Rankine cycle) Kitchen Refrigerator Carnot Cycle - is not very
More informationAP Chemistry 2008 Free-Response Questions
AP Chemistry 008 Free-Response Questions The College Board: Connecting Students to College Success The College Board is a not-for-profit membership association whose mission is to connect students to college
More informationUnit 3: States of Matter Practice Exam
Page 1 Unit 3: States of Matter Practice Exam Multiple Choice. Identify the choice that best completes the statement or answers the question. 1. Two gases with unequal masses are injected into opposite
More informationHomework 9. Problems: 12.31, 12.32, 14.4, 14.21
Homework 9 Problems: 1.31, 1.3, 14.4, 14.1 Problem 1.31 Assume that if the shear stress exceeds about 4 10 N/m steel ruptures. Determine the shearing force necessary (a) to shear a steel bolt 1.00 cm in
More informationChapter 13. Properties of Solutions
Sample Exercise 13.1 (p. 534) By the process illustrated below, water vapor reacts with excess solid sodium sulfate to form the hydrated form of the salt. The chemical reaction is Na 2 SO 4(s) + 10 H 2
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 informationStandard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K
1 Thermodynamics There always seems to be at least one free response question that involves thermodynamics. These types of question also show up in the multiple choice questions. G, S, and H. Know what
More informationEnthalpy of Combustion via Calorimetry
Enthalpy of Combustion via Calorimetry Introduction This experiment measures the enthalpy change when a system consisting of a known amount of a substance in the presence of excess oxygen is quantitatively
More informationChemistry 110 Lecture Unit 5 Chapter 11-GASES
Chemistry 110 Lecture Unit 5 Chapter 11-GASES 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 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 informationA. Kinetic Molecular Theory (KMT) = the idea that particles of matter are always in motion and that this motion has consequences.
I. MOLECULES IN MOTION: A. Kinetic Molecular Theory (KMT) = the idea that particles of matter are always in motion and that this motion has consequences. 1) theory developed in the late 19 th century to
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 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 informationCarbon Dioxide and an Argon + Nitrogen Mixture. Measurement of C p /C v for Argon, Nitrogen, Stephen Lucas 05/11/10
Carbon Dioxide and an Argon + Nitrogen Mixture Measurement of C p /C v for Argon, Nitrogen, Stephen Lucas 05/11/10 Measurement of C p /C v for Argon, Nitrogen, Carbon Dioxide and an Argon + Nitrogen Mixture
More information