UNIT # 06 THERMODYNAMICS EXERCISE # 1. T i. 1. m Zn

Size: px
Start display at page:

Download "UNIT # 06 THERMODYNAMICS EXERCISE # 1. T i. 1. m Zn"

Transcription

1 UNI # 6 HERMODYNMIS EXERISE #. m Zn.S Zn.( f i + m H O.S H O.( f i (6.8 gm (.4 J/g ( f + 8 gm (4. J/g ( f [(6.8 (.4 + 8(4.] f (6.8 (.4 ( + (8 (4. ( (6.8(.4( (8(4.( f 97. (6.8(.4 (8(4.. U q + w heat absorb (q 4 joule w 7 joule since Work done by the system. ( U q + w 4 7 joule. Decrease in internal energy U ( work done by the system w U w U w q he process is adiabatic. ( 4. t constant volume w U q first law. he energy due to external field is not included in i nternal energy like gravitat ional field, ear th's magnetic field etc. ( 6. Heat and work are path dependent, or indefinite quantity. ( 7. For monoatomic ideal gas total degree of freedom ( hree translational mode of motion ( R R r + R R 8. r monoatomic ideal gas R t constant pressure q H n q (. mole.(8.4 J / K mole (6 9. Reversible process-involve infinitesimally small driving force. Hence system and surrounding remains in equilibrium. (. temperature at 'a' R at (a at (c R...(i ( (4 8 R U n ( f i R(8 R U. R. Work done in adiabataic process ( U w n w ((.(. he case of irreversible adiabatic process. w ( f i n ( ( f i n R (f i (atm(l L n (R (L atm.8 (L atm k mole. B > and B > H n ( B > w ext ( B < 6. Heat of reaction at const. pressure r H Heat of reaction at const. pressure r U r H r U + n g R n g r H r U ( R B >

2 8. Fusion and vaporisation are example of isothermal processes - ( Q f < b Q f R b 9. H O(s q H O(l H O(l 6 q H fusion (kj/mole mole 8 q 6.. kj q ms (6 gm (4.8 J/K gm (6((4.8 q NE q + q. kj. When ice liquid : the process is reversible fusion. he fusion is isothermal process. ( : dq dq d. U q + w constant since H q p.6 U + atm ( litres R U.6 (L atm (. J/L atm U. For reversible adiabatic process ( q rev S system. S n ln ln 7 S ln R ln 98 H 4. Using S transition H S surr trans S trans S surr S total transition transition X q, temperature of ice bath 7K Initial pressure R f R (.8 atm final pressure atm final volume ; f f i i i i ( R 4.6 L f S ln S R ln for spontaneous reactions S total > ( S total S system + S surr X S total S system 98 S total > S sys + X 98 X S syst > 98 Hence S syst can be negative but numerically smaller than X 98. S syst X For dissociation reactions ( H > and n g > r S > 8. G H S G [( 8] G + 8 spontaneous but less than certain temperature. 9. Formation of Fe O 4 Fe(s + O (g Fe O 4 (s ; G? G ( 9 kcal + ( 77 kcal 4. kcal/mole. H S H ( 66. S bove this temperature the process becomes spontaneous. (

3 HERMODYNMIS EXERISE #. Intensive property ( extensive property ( extensive property ph concentration mole/volume though ph is a dimensionless number and intensive property (ph EMF energy Intensive property ch arg e Boiling point( b temperature intensive property entropy (s q extensive intensive extensive property. t constant, the molecule with maximum atoms have greatest internal energy.. q U W ( + 4 K 4. Irreverssible adiabatic process ( W ext atm ext atm K (R. R( W ( atm atm atm and W ( R( R( (7 R R. B B isochoric heating ( B isothermal expansion ( isobaric cooling B ( B isochoric heating B 6. B emperature at ( D D 4 ( /. B now D : U H U n remember for ideal gas H n 7. (,, Isochoric heating H B(,, W (4 4 K H irr. adiabatic process (q R ( R W W B + W B + W D ( B B ln ( D B W ( ln 4 ( 4 W ln and q W ( U q ln (,, H overall H + H H U + ( H ( + ( H U + ( H ( + ( H H overall ( + ( + ( +

4 W q by source. H q p W by (n (q source ( kcal.8 kcal since H is state function H will remain same from both path-isobaric and non-isobaric q p isobaric path non-isobaric path q But q q p only when path was isobaric. B H q p only for isobaric path.. Greater the n g greater the value of S.. S n ln for isochoric change. S 7 R ln 47 7 S R ln 47. he net heat absorbed by hot and cold body is equal to zero. q H + q Let is the total heat capacity of hot and cold body. ( f + ( f H f H H Entropy change S otal S hot body + S cold body f S hot body.ln H f S cold body.ln f f S otal ln ln H f ln H. (f S otal ln 4 H. 4. G H S y + mx H m S from intercept > H > m < S < S >. Melting of H O(s at and atm is a reversibly procers S otal aporisation of H O(l at 7 K is a reversible process S otal Below H O(s H O(l is non spontaneous not feasible. H O(l H O(s (freezing is feasible above H O(s H O(l feasibly G ive for melting process S otal increases 9. G H + E G + 6 cal. H O(l H O(g 7 K 7 K atm S H vap atm G H f H i

5 HERMODYNMIS EXERISE # OMREHENSION #. U Here U Kinetic energy of ideal gas ( U n. U q + w J q 8J q 8 J OMREHENSION # n...(i sub. ( in (...(ii. r S S (H OH, g [S (O, g + S (H, g]. R.R w d ( (. ( / w ( ( R d ( J/K-mole. r H f H (H OH, g f H (O, g (4 87 kj/mol. rs rs ln,m (H OH,m (O,m (H 44 ( J/K-mol work done by the gas w ( (. For diatomic gas with no vibrational degree of freedom R + R rs ( 6 ( 4 ln rs. J/K-mol 4. rh rh r ( / R U w ( ( 7 J ( 7 w ( (J 8J ( ( rh ( 87 4( rh kj/mol. r G rh S 8786 (. 8.9 kj/mol

6 HERMODYNMIS.(i H O (g H O( (g > ( W ext ( ( (g W +ve (ii H O (s H O(g (g > (s W ve (iii H O ( H O(s (s > ( W ext ( (s ( ve (iv H (g + N (g NH (g W ext ( ext (n R n R n g R W +e (v ao (s ao (s + O (g W ext > ve. E 6 J w J q w 6 4 J. H glucose 88 kj mol (a Energy need to climb m Mgh 6. q 87 Joule Now useful energy from mole of glucose kj 87 No. of mole of glucose required 7.67 mole grams of glucose gm (b Energy need tp climb m will be time. wt. should be time.487 kg 4. q p q v + n g R 4.66 q v q v (8. 6. kj q v 7.8 kj. H kcal H E + EXERISE # 4[] 4.8 E +. E (48.9 Joule E.99 kcal cal NH 4 N(s + O (g N (g + O (g + H O( H 98 E + n g R H H 44 cal H E + ( 44E+. (.8.96 E E W extd (. (. W. J 9. Zn(s + H + (aq Zn + (aq + H (g H 6. kj Q E W 6. kj E +. ( 6 E 9. kj W ext (. 6 W.. W irr W irr 9. kj W rev. og W rev. 8.4 log4 W rev 7.9 kj and q E W at E H W rev q 7.9 kj

7 . n 7 7 K diabatic condition Q EWn ( W W. kj/mole. rocess reversibly adiabatic 98. K K v K. K log. log. ( log. log.6 Now n ( R ( m ( m 8.4 m.6.6. W. log W.988 kj 44.8L.4L 7K B 46K able- log State.4L State - State - atm atm atm atm 46 atm K 46K State atm Step Name of process q w E H Isochoric R(7 R(7 R(7 B Isotherm 46R ln 46R ln Isotherm R(7 R(7 R(7 R(7 overall State - (Isochoric W q E R(7 H n p d H R(7 State - B (Isothermal E H H E + is Q w log( 46 Q 46 R ln W 46 R ln E n W ( State - (Isobaric q E w E + ( or H E + R( 7. H (g + O (g H O( p p H O( p H (g reaction p O (g p reaction.9 kj H 7 H 98 + np ( kj H kj JK mol H n n p d ( d H.64 kj/mole W ( ( W 477 E E.87 kj

8 7. S 8.8 J/K H. kj 8. S H S n pd. (. 8.8 HERMODYNMIS 9 K d.. log (6 7 S.68 kj 9. Br ( + l (g Brl(g, H 9. kj S Br. S l (g. S Brl(g 9.7 J mol K S R r G H S J. l 4 ( l 4 (g atm 98 K S JK r H H p H r ( kj.6 kj/mol r G H R S r G r G 4.96 kj/mol. Step- (- Ice ( K Ice (7 K ( K (7 K S m p ln.9 ln 7 S 6. J/ Step- (- Ice (7 K Water (7 K H S f.4.44 J/ 7 7 Step- (- Water (7 K Water (7 K S 4.8 ln 7 7 Step-4 ( J/ Water (7 K Steam (7 K (7 K (7 K S 4 H v J/. H O (g + O(s H (g + O (g (i r H 98 r H (g + r H O (g r H O (s r H O(g k cal/mol (ii r G (iii (iv (v r G 6.8 r G r H r S r S rs 98 r S. cal/ mole but at constant H E + n g r H r E 98 S 98 [H O(g] 9.8 k cal/mol r S s H O(g + S O r S H r S O. r S H O(g r S H (g 4. cal/ K mole O Step- (- EXERISE # 4[B] Steam (7 K Steam (4 K (7 K (4 K S.9 ln J/ 7 S 98.4 J/., atm, K, atm (a constant ( constant ( / constant ( / ( / / 9.8 w U n v d w 9.7 J 6.L

9 (b U w. 8.4 ( R R. (. 4 K 7.4L w U. 8.4 (4 w 496. J. L, 7/, 67 K,. Ma atm,.7 Ma 7 atm n R. (i U H (ii q w ln ln 7 q 7. kj w 7. kj 7( ( (. / L K q, w U.. 8.4( w U.4 kj H ( kJ (iii q w U H (iv q, U w ( K w U ( 6 7. kj H ( kj (v U H 4.(i L w ( L-atm w J w 9.94 kj q w 9.94 kj he entropy change of the system S sys. will be same in all the three process as it is state function. (S S sys. ln 8.4 ln 9.4 J/K For reversible process ( S S surr. S sys. 9.4 J/K (ii (iii S sys. 9.4 J/K q S surr. irrev. q rev S sys S S sys. + ( S sys J/K For free expansion system doesn't absorb any heat so q ( q S sys. S S sys..87 J/K.(i S sys., S surr., S (ii U w, n v ( (( ( K 94.6 S sys. n p ln R ln ln 8.4 ln 47 S sys..97 J/K since no heat is transfered ( q S surr. S S sys..97 J/K (iii In free expansion ( q w U is constant. ( S sys. ln. 8.4 ln.8 JK S surr. S S sys.8 J/K 6. atm, L atm,.99l Let a + b On finding a, b so ( w d ( d w ( + ( w (. + (.99. L-atm w J U w J H U + ( + (.99 99J H 99. kj

10 7.(i S sys. n v ln R ln R ln S S surr. S sys. (Reversible process ( R ln 8.68 qh.( q H 4.4 kj v p R (ii S sys. R ln w q U R (9 q R (9 S surr. R (.9 U n v d 9.9 kj (iii w q U 9.9 kj H n p d 4.4 kj. t 98 K, S R ln R (.9 R (.4 8. G H S U + S dg du + d + d ds Sd w, d, d dq ds so dg ds + d ds Sd dg d Sd G d ( 4 4 S d d 4.6 (4/ 8. L-atm 8 J Sd (. d( +.( 9. n Sd ( +. (4 G 8 J L L & so t K G 6 kj/mole H 77 kj/mole G H S S kj/mole G kj/mole dditional non- work (- G G 4 kj/mole. r p J/K mole r S d d( r S r p H J/K mole r S 7 r S r p ln 7 r S ln J/K mole (i w ( L-atm w J 4. k q H n d p 8.68.( d ( r H r p d r H 7 r H 4.7 ( r H J/mole r G 479. ( 94. J.9 kj/mole

CHEM Thermodynamics. Entropy, S

CHEM Thermodynamics. Entropy, S hermodynamics Change in Change in Entropy, S Entropy, S Entropy is the measure of dispersal. he natural spontaneous direction of any process is toward greater dispersal of matter and of energy. Dispersal

More information

S = k log W CHEM Thermodynamics. Change in Entropy, S. Entropy, S. Entropy, S S = S 2 -S 1. Entropy is the measure of dispersal.

S = k log W CHEM Thermodynamics. Change in Entropy, S. Entropy, S. Entropy, S S = S 2 -S 1. Entropy is the measure of dispersal. , S is the measure of dispersal. The natural spontaneous direction of any process is toward greater dispersal of matter and of energy. Dispersal of matter: Thermodynamics We analyze the constraints on

More information

S = k log W 11/8/2016 CHEM Thermodynamics. Change in Entropy, S. Entropy, S. Entropy, S S = S 2 -S 1. Entropy is the measure of dispersal.

S = k log W 11/8/2016 CHEM Thermodynamics. Change in Entropy, S. Entropy, S. Entropy, S S = S 2 -S 1. Entropy is the measure of dispersal. Entropy is the measure of dispersal. The natural spontaneous direction of any process is toward greater dispersal of matter and of energy. Dispersal of matter: Thermodynamics We analyze the constraints

More information

So far changes in the state of systems that occur within the restrictions of the first law of thermodynamics were considered:

So far changes in the state of systems that occur within the restrictions of the first law of thermodynamics were considered: Entropy So far changes in the state of systems that occur within the restrictions of the first law of thermodynamics were considered: Energy is transferred from one state to another by any possible forms,

More information

(D) energy arising by gravitational pull. (A) molar internal energy (B) volume (C) w (D) q + w 7. For a monatomic gas, the value of the ratio of C p.

(D) energy arising by gravitational pull. (A) molar internal energy (B) volume (C) w (D) q + w 7. For a monatomic gas, the value of the ratio of C p. EXERCISE-01 CHECK YOUR GRASP SELEC HE CORREC ALERNAIVE (ONLY ONE CORREC ANSWER) 1. he piece of zinc at a temperature of 0.0 C weighing 65.38 g is dropped into 180 g of boiling water ( = 100 C). he specific

More information

Chpt 19: Chemical. Thermodynamics. Thermodynamics

Chpt 19: Chemical. Thermodynamics. Thermodynamics CEM 152 1 Reaction Spontaneity Can we learn anything about the probability of a reaction occurring based on reaction enthaplies? in general, a large, negative reaction enthalpy is indicative of a spontaneous

More information

What is thermodynamics? and what can it do for us?

What is thermodynamics? and what can it do for us? What is thermodynamics? and what can it do for us? The overall goal of thermodynamics is to describe what happens to a system (anything of interest) when we change the variables that characterized the

More information

Thermodynamics (XI) Assignment(Solution)

Thermodynamics (XI) Assignment(Solution) SYLLABUS CUM COM./XI/03 4 hermodynamics (XI) Assignment(Solution) Comprehension ype Questions aragraph for Question -5 For an ideal gas, an illustration of three different paths A, (B + C) and (D + E)

More information

SPONTANEOUS PROCESSES AND THERMODYNAMIC EQUILIBRIUM

SPONTANEOUS PROCESSES AND THERMODYNAMIC EQUILIBRIUM 13 CHAPER SPONANEOUS PROCESSES AND HERMODYNAMIC EQUILIBRIUM 13.1 he Nature of Spontaneous Processes 13.2 Entropy and Spontaneity: A Molecular Statistical Interpretation 13.3 Entropy and Heat: Macroscopic

More information

Ch 10 Practice Problems

Ch 10 Practice Problems Ch 10 Practice Problems 1. Which of the following result(s) in an increase in the entropy of the system? I. (See diagram.) II. Br 2(g) Br 2(l) III. NaBr(s) Na + (aq) + Br (aq) IV. O 2(298 K) O 2(373 K)

More information

10 NEET 31 Years 11. The enthalpy of fusion of water is kcal/mol. The molar entropy change for the melting of ice at

10 NEET 31 Years 11. The enthalpy of fusion of water is kcal/mol. The molar entropy change for the melting of ice at 6 Thermodynamics. A gas is allowed to expand in a well insulated container against a constant external pressure of.5 atm from an initial volume of.50 L to a final volume of 4.50 L. The change in internal

More information

Answers to Problem Sheet (a) spontaneous (b) nonspontaneous (c) nonspontaneous (d) spontaneous (e) nonspontaneous

Answers to Problem Sheet (a) spontaneous (b) nonspontaneous (c) nonspontaneous (d) spontaneous (e) nonspontaneous Answers to Problem Sheet 5 1. (a) spontaneous (b) nonspontaneous (c) nonspontaneous (d) spontaneous (e) nonspontaneous 2. (a) Heat will flow from the warmer block of iron to the colder block of iron until

More information

Entropy Changes & Processes

Entropy Changes & Processes Entropy Changes & Processes Chapter 4 of Atkins: he Second Law: he Concepts Section 4.3, 7th edition; 3.3, 8th and 9th editions Entropy of Phase ransition at the ransition emperature Expansion of the Perfect

More information

Thermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation

Thermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation THERMOCHEMISTRY Thermochemistry Energy 1st Law of Thermodynamics Enthalpy / Calorimetry Hess' Law Enthalpy of Formation The Nature of Energy Kinetic Energy and Potential Energy Kinetic energy is the energy

More information

Thermodynamic Laws, Gibbs Free Energy & pe/ph

Thermodynamic Laws, Gibbs Free Energy & pe/ph Thermodynamic Laws, Gibbs Free Energy & pe/ph or how to predict chemical reactions without doing experiments OCN 623 Chemical Oceanography Definitions Extensive properties Depend on the amount of material

More information

Chapter 19 Chemical Thermodynamics

Chapter 19 Chemical Thermodynamics Chapter 19 Chemical Thermodynamics Spontaneous Processes Entropy and the Second Law of Thermodynamics The Molecular Interpretation of Entropy Entropy Changes in Chemical Reactions Gibbs Free Energy Free

More information

CHM 111 Dr. Kevin Moore

CHM 111 Dr. Kevin Moore CHM 111 Dr. Kevin Moore Kinetic Energy Energy of motion E k 1 2 mv 2 Potential Energy Energy of position (stored) Law of Conservation of Energy Energy cannot be created or destroyed; it can only be converted

More information

University of Washington Department of Chemistry Chemistry 452/456 Summer Quarter 2011

University of Washington Department of Chemistry Chemistry 452/456 Summer Quarter 2011 Homework Assignment #: Due at 500 pm Wednesday July 6. University of Washington Department of Chemistry Chemistry 45/456 Summer Quarter 0 ) he respiratory system uses oxygen to degrade glucose to carbon

More information

Phase Changes and Latent Heat

Phase Changes and Latent Heat Review Questions Why can a person remove a piece of dry aluminum foil from a hot oven with bare fingers without getting burned, yet will be burned doing so if the foil is wet. Equal quantities of alcohol

More information

Second law of thermodynamics

Second law of thermodynamics Second law of thermodynamics It is known from everyday life that nature does the most probable thing when nothing prevents that For example it rains at cool weather because the liquid phase has less energy

More information

I. Multiple Choice Questions (Type-I)

I. Multiple Choice Questions (Type-I) I. Multiple Choice Questions (Type-I) 1. Thermodynamics is not concerned about. (i) energy changes involved in a chemical reaction. the extent to which a chemical reaction proceeds. the rate at which a

More information

Thermodynamics 1. Thermodynamics means flow of heat. This deals with the quantitative relationship existing between heat and other forms of energy in physicochemical transformations. 2. The four laws are

More information

Review of classical thermodynamics

Review of classical thermodynamics Review of classical thermodynamics Fundamental Laws, Properties and Processes (2) Entropy and the Second Law Concepts of equilibrium Reversible and irreversible processes he direction of spontaneous change

More information

For more info visit

For more info visit Basic Terminology: Terms System Open System Closed System Isolated system Surroundings Boundary State variables State Functions Intensive properties Extensive properties Process Isothermal process Isobaric

More information

I PUC CHEMISTRY CHAPTER - 06 Thermodynamics

I PUC CHEMISTRY CHAPTER - 06 Thermodynamics I PUC CHEMISTRY CHAPTER - 06 Thermodynamics One mark questions 1. Define System. 2. Define surroundings. 3. What is an open system? Give one example. 4. What is closed system? Give one example. 5. What

More information

Entropy Changes & Processes

Entropy Changes & Processes Entropy Changes & Processes Chapter 4 of Atkins: he Second Law: he Concepts Section 4.3 Entropy of Phase ransition at the ransition emperature Expansion of the Perfect Gas Variation of Entropy with emperature

More information

Chemical Thermodynamics

Chemical Thermodynamics Quiz A 42.8 ml solution of ammonia (NH 3 ) is titrated with a solution of 0.9713 M hydrochloric acid. The initial reading on the buret containing the HCl was 47.13 ml and the final reading when the endpoint

More information

Chapter 8 Thermochemistry: Chemical Energy

Chapter 8 Thermochemistry: Chemical Energy Chapter 8 Thermochemistry: Chemical Energy 國防醫學院生化學科王明芳老師 2011-11-8 & 2011-11-15 Chapter 8/1 Energy and Its Conservation Conservation of Energy Law: Energy cannot be created or destroyed; it can only be

More information

Chemistry 1A, Spring 2008 Midterm Exam III, Version A April 14, 2008 (90 min, closed book)

Chemistry 1A, Spring 2008 Midterm Exam III, Version A April 14, 2008 (90 min, closed book) Chemistry 1A, Spring 2008 Midterm Exam III, Version A April 14, 2008 (90 min, closed book) Name: KEY SID: A Name: 1.) Write your name on every page of this exam. 2.) his exam has 15 multiple-choice questions

More information

Outline of the Course

Outline of the Course Outline of the Course 1) Review and Definitions 2) Molecules and their Energies 3) 1 st Law of Thermodynamics 4) 2 nd Law of Thermodynamics 5) Gibbs Free Energy 6) Phase Diagrams and REAL Phenomena 7)

More information

Topic 5: Energetics. Heat & Calorimetry. Thursday, March 22, 2012

Topic 5: Energetics. Heat & Calorimetry. Thursday, March 22, 2012 Topic 5: Energetics Heat & Calorimetry 1 Heat is energy that is transferred from one object to another due to a difference in temperature Temperature is a measure of the average kinetic energy of a body

More information

Chapter 19 Chemical Thermodynamics Entropy and free energy

Chapter 19 Chemical Thermodynamics Entropy and free energy Chapter 19 Chemical Thermodynamics Entropy and free energy Learning goals and key skills: Explain and apply the terms spontaneous process, reversible process, irreversible process, and isothermal process.

More information

4/19/2016. Chapter 17 Free Energy and Thermodynamics. First Law of Thermodynamics. First Law of Thermodynamics. The Energy Tax.

4/19/2016. Chapter 17 Free Energy and Thermodynamics. First Law of Thermodynamics. First Law of Thermodynamics. The Energy Tax. Chemistry: A Molecular Approach, 2nd Ed. Nivaldo Tro First Law of Thermodynamics Chapter 17 Free Energy and Thermodynamics You can t win! First Law of Thermodynamics: Energy cannot be created or destroyed

More information

Page 1 of 11. Website: Mobile:

Page 1 of 11. Website:    Mobile: Class XI Chapter 6 Thermodynamics Chemistry Question 6.1: Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path

More information

Thermochemistry. Energy and Chemical Change

Thermochemistry. Energy and Chemical Change Thermochemistry Energy and Chemical Change Energy Energy can change for and flow, but it is always conserved. The Nature of Energy Energy the ability to do work or produce heat Potential energy Kinetic

More information

THE SECOND LAW OF THERMODYNAMICS. Professor Benjamin G. Levine CEM 182H Lecture 5

THE SECOND LAW OF THERMODYNAMICS. Professor Benjamin G. Levine CEM 182H Lecture 5 THE SECOND LAW OF THERMODYNAMICS Professor Benjamin G. Levine CEM 182H Lecture 5 Chemical Equilibrium N 2 + 3 H 2 2 NH 3 Chemical reactions go in both directions Systems started from any initial state

More information

Chapter 16. Thermodynamics. Thermochemistry Review. Calculating H o rxn. Predicting sign for H o rxn. Creative Commons License

Chapter 16. Thermodynamics. Thermochemistry Review. Calculating H o rxn. Predicting sign for H o rxn. Creative Commons License Chapter 16 Thermodynamics GCC CHM152 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution License 4.0. ChemWiki (CC

More information

CHEMICAL THERMODYNAMICS

CHEMICAL THERMODYNAMICS DEPARTMENT OF APPLIED CHEMISTRY LECTURE NOTES 6151- ENGINEERING CHEMISTRY-II UNIT II CHEMICAL THERMODYNAMICS Unit syllabus: Terminology of thermodynamics - Second law: Entropy - entropy change for an ideal

More information

Chapter 19 Chemical Thermodynamics

Chapter 19 Chemical Thermodynamics Chapter 19 Chemical Thermodynamics Kinetics How fast a rxn. proceeds Equilibrium How far a rxn proceeds towards completion Thermodynamics Study of energy relationships & changes which occur during chemical

More information

Module 5 : Electrochemistry Lecture 21 : Review Of Thermodynamics

Module 5 : Electrochemistry Lecture 21 : Review Of Thermodynamics Module 5 : Electrochemistry Lecture 21 : Review Of Thermodynamics Objectives In this Lecture you will learn the following The need for studying thermodynamics to understand chemical and biological processes.

More information

MME 2010 METALLURGICAL THERMODYNAMICS II. Fundamentals of Thermodynamics for Systems of Constant Composition

MME 2010 METALLURGICAL THERMODYNAMICS II. Fundamentals of Thermodynamics for Systems of Constant Composition MME 2010 METALLURGICAL THERMODYNAMICS II Fundamentals of Thermodynamics for Systems of Constant Composition Thermodynamics addresses two types of problems: 1- Computation of energy difference between two

More information

Thermochemistry. Energy and Chemical Change

Thermochemistry. Energy and Chemical Change Thermochemistry Energy and Chemical Change Energy Energy can change for and flow, but it is always conserved. The Nature of Energy Energy the ability to do work or produce heat Potential energy Kinetic

More information

CHEMICAL THERMODYNAMICS

CHEMICAL THERMODYNAMICS CT 1 CHEMICAL THERMODYNAMICS Syllabus : Fundamentals of thermodynamics : System and surroundings, extensive and intensive properties, state functions, types of processes. First law of thermodynamics -

More information

Thermodynamics. 1. Which of the following processes causes an entropy decrease?

Thermodynamics. 1. Which of the following processes causes an entropy decrease? Thermodynamics 1. Which of the following processes causes an entropy decrease? A. boiling water to form steam B. dissolution of solid KCl in water C. mixing of two gases in one container D. beach erosion

More information

THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system

THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system and its surroundings. a. System = That part of universe

More information

I. The Nature of Energy A. Energy

I. The Nature of Energy A. Energy I. The Nature of Energy A. Energy is the ability to do work or produce heat. It exists in 2 forms: 1. Potential energy is energy due to the composition or position of an object. 2. Kinetic energy is energy

More information

Problem: Calculate the entropy change that results from mixing 54.0 g of water at 280 K with 27.0 g of water at 360 K in a vessel whose walls are

Problem: Calculate the entropy change that results from mixing 54.0 g of water at 280 K with 27.0 g of water at 360 K in a vessel whose walls are Problem: Calculate the entropy change that results from mixing 54.0 g of water at 280 K with 27.0 g of water at 360 K in a vessel whose walls are perfectly insulated from the surroundings. Is this a spontaneous

More information

Class XI Chapter 6 Thermodynamics Question 6.1: Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii)

More information

2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.

2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. CHEMISTRY & YOU Chapter 17 Thermochemistry 17.1 The Flow of Energy 17. Measuring and Expressing Enthalpy Changes 17.3 Heat in Changes of State 17.4 Calculating Heats of Reaction Why does sweating help

More information

Chapter 19 Chemical Thermodynamics Entropy and free energy

Chapter 19 Chemical Thermodynamics Entropy and free energy Chapter 19 Chemical Thermodynamics Entropy and free energy Learning goals and key skills: Understand the meaning of spontaneous process, reversible process, irreversible process, and isothermal process.

More information

CHEMICAL THERMODYNAMICS. Nature of Energy. ΔE = q + w. w = PΔV

CHEMICAL THERMODYNAMICS. Nature of Energy. ΔE = q + w. w = PΔV CHEMICAL HERMODYNAMICS Nature of Energy hermodynamics hermochemistry Energy (E) Work (w) Heat (q) Some Definitions Study the transformation of energy from one form to another during physical and chemical

More information

Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat.

Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat. CHEM134- F18 Dr. Al- Qaisi Chapter 06: Thermodynamics Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat. Energy is anything that has the capacity

More information

Lecture 4. The Second Law of Thermodynamics

Lecture 4. The Second Law of Thermodynamics Lecture 4. The Second Law of Thermodynamics LIMITATION OF THE FIRST LAW: -Does not address whether a particular process is spontaneous or not. -Deals only with changes in energy. Consider this examples:

More information

OCN 623: Thermodynamic Laws & Gibbs Free Energy. or how to predict chemical reactions without doing experiments

OCN 623: Thermodynamic Laws & Gibbs Free Energy. or how to predict chemical reactions without doing experiments OCN 623: Thermodynamic Laws & Gibbs Free Energy or how to predict chemical reactions without doing experiments Definitions Extensive properties Depend on the amount of material e.g. # of moles, mass or

More information

THERMODINAMICS. Tóth Mónika

THERMODINAMICS. Tóth Mónika THERMODINAMICS Tóth Mónika 2014 monika.a.toth@aok.pte.hu Temperature Temperature: is related to the average energy of the motion of the particles of an object or system. Different temperature scales. Thermometer

More information

The Second Law of Thermodynamics (Chapter 4)

The Second Law of Thermodynamics (Chapter 4) The Second Law of Thermodynamics (Chapter 4) First Law: Energy of universe is constant: ΔE system = - ΔE surroundings Second Law: New variable, S, entropy. Changes in S, ΔS, tell us which processes made

More information

Thermodynamics- 1) Hess's law states that 1) The standard enthalpy of an overall reaction is the sum of the enthalpy changes in individual reaction. ) Enthalpy of formation of compound is same as the enthalpy

More information

= 1906J/0.872deg = 2186J/deg

= 1906J/0.872deg = 2186J/deg Physical Chemistry 2 2006 Homework assignment 2 Problem 1: he heat of combustion of caffeine was determined by first burning benzoic acid and then caffeine. In both cases the calorimeter was filled with

More information

Energy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy

Energy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy THERMOCHEMISTRY Thermodynamics Study of energy and its interconversions Energy is TRANSFORMED in a chemical reaction (POTENTIAL to KINETIC) HEAT (energy transfer) is also usually produced or absorbed -SYSTEM:

More information

Name Date Class THE FLOW OF ENERGY HEAT AND WORK

Name Date Class THE FLOW OF ENERGY HEAT AND WORK 17.1 THE FLOW OF ENERGY HEAT AND WORK Section Review Objectives Explain the relationship between energy, heat, and work Distinguish between exothermic and endothermic processes Distinguish between heat

More information

Chapter 19 Chemical Thermodynamics

Chapter 19 Chemical Thermodynamics Chapter 19 Chemical Thermodynamics Kinetics How fast a rxn. proceeds Equilibrium How far a rxn proceeds towards completion Thermodynamics Study of energy relationships & changes which occur during chemical

More information

Thermodynamics Spontaneity. 150/151 Thermochemistry Review. Spontaneity. Ch. 16: Thermodynamics 12/14/2017

Thermodynamics Spontaneity. 150/151 Thermochemistry Review. Spontaneity. Ch. 16: Thermodynamics 12/14/2017 Ch. 16: Thermodynamics Geysers are a dramatic display of thermodynamic principles in nature. As water inside the earth heats up, it rises to the surface through small channels. Pressure builds up until

More information

CHEM Thermodynamics. Work. There are two ways to change the internal energy of a system:

CHEM Thermodynamics. Work. There are two ways to change the internal energy of a system: There are two ways to change the internal energy of a system: Thermodynamics Work 1. By flow of heat, q Heat is the transfer of thermal energy between and the surroundings 2. By doing work, w Work can

More information

CHEMISTRY 109 #25 - REVIEW

CHEMISTRY 109 #25 - REVIEW CHEMISTRY 109 Help Sheet #25 - REVIEW Chapter 4 (Part I); Sections 4.1-4.6; Ch. 9, Section 9.4a-9.4c (pg 387) ** Review the appropriate topics for your lecture section ** Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc

More information

Energy is the capacity to do work

Energy is the capacity to do work 1 of 10 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly

More information

Thermodynamics: Entropy, Free Energy, and Equilibrium

Thermodynamics: Entropy, Free Energy, and Equilibrium Chapter 16 Thermodynamics: Entropy, Free Energy, and Equilibrium spontaneous nonspontaneous In this chapter we will determine the direction of a chemical reaction and calculate equilibrium constant using

More information

CHAPTER THERMODYNAMICS

CHAPTER THERMODYNAMICS 54 CHAPTER THERMODYNAMICS 1. If ΔH is the change in enthalpy and ΔE the change in internal energy accompanying a gaseous reaction, then ΔHis always greater than ΔE ΔH< ΔE only if the number of moles of

More information

Entropy, Free Energy, and Equilibrium

Entropy, Free Energy, and Equilibrium Entropy, Free Energy, and Equilibrium Chapter 17 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs

More information

Chapter 16. Spontaneity, Entropy and Free energy

Chapter 16. Spontaneity, Entropy and Free energy Chapter 16 Spontaneity, Entropy and Free energy Contents Spontaneous Process and Entropy Entropy and the second law of thermodynamics The effect of temperature on spontaneity Free energy Entropy changes

More information

, is placed in thermal contact with object B, with mass m, specific heat c B. and initially at temperature T B

, is placed in thermal contact with object B, with mass m, specific heat c B. and initially at temperature T B 4C_PLC http://www.cabrillo.edu/~jmccullough/physics4c/files/4c_plc/4c_plc.htm Page 1 of 8 /6/201 1. The heat capacity at constant volume and the heat capacity at constant pressure have different values

More information

Energy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy

Energy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy THERMOCHEMISTRY Thermodynamics Study of energy and its interconversions Energy is TRANSFORMED in a chemical reaction (POTENTIAL to KINETIC) HEAT (energy transfer) is also usually produced or absorbed -SYSTEM:

More information

THE ZEROTH AND FISRT LAW OF THERMODYNAMICS. Saeda Al-Mhyawi secend Tearm 1435H

THE ZEROTH AND FISRT LAW OF THERMODYNAMICS. Saeda Al-Mhyawi secend Tearm 1435H H ZROH AND FISR LAW OF HRMODYNAMIS Saeda Al-Mhyawi secend earm 435H HAR II H ZROH AND FISR LAW OF HRMODYNAMIS Lecture () Outline Introduction he Zeroth Law of hermodynamics he First Law of hermodynamics

More information

Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes

Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes Thermochemistry Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes heat flows from high to low (hot cool) endothermic reactions: absorb energy

More information

Thermochemistry: Heat and Chemical Change

Thermochemistry: Heat and Chemical Change Thermochemistry: Heat and Chemical Change 1 Heat or Thermal Energy (q) Heat is a form of energy Is heat the same as temperature? Heat flows between two objects at different temperatures. Hot Cold 2 Chemical

More information

Chemistry 123: Physical and Organic Chemistry Topic 2: Thermochemistry

Chemistry 123: Physical and Organic Chemistry Topic 2: Thermochemistry Recall the equation. w = -PΔV = -(1.20 atm)(1.02 L)( = -1.24 10 2 J -101 J 1 L atm Where did the conversion factor come from? Compare two versions of the gas constant and calculate. 8.3145 J/mol K 0.082057

More information

OPEN CLOSED ISOLATED. Only energy can be exchanged between system & surrounding. eg. closed vessel

OPEN CLOSED ISOLATED. Only energy can be exchanged between system & surrounding. eg. closed vessel THERMODYNAMICS Limitations :- (1) Not applicable on microscopic system like, change inside an atoms. Or system having few molecules only. (2) deals only with initial & final state (does not deal with path

More information

Homework Problem Set 8 Solutions

Homework Problem Set 8 Solutions Chemistry 360 Dr. Jean M. Standard Homework roblem Set 8 Solutions. Starting from G = H S, derive the fundamental equation for G. o begin, we take the differential of G, dg = dh d( S) = dh ds Sd. Next,

More information

Chapter 11 part 2. Properties of Liquids Viscosity Surface Tension Capillary Action. Phase Changes (energy of phase changes)

Chapter 11 part 2. Properties of Liquids Viscosity Surface Tension Capillary Action. Phase Changes (energy of phase changes) Chapter 11 part 2 Properties of Liquids Viscosity Surface Tension Capillary Action Phase Changes (energy of phase changes) Dynamic Equilibrium Vapor pressure Phase diagram 1 Structure Affects Function

More information

Chemical Thermodynamics

Chemical Thermodynamics Chemical Thermodynamics Overview Everything in the world is a balance of energy, in various forms from biological processes to the rusting of a nail. Two of the most important questions chemists ask are:

More information

Chapter 19. Chemical Thermodynamics

Chapter 19. Chemical Thermodynamics Chapter 19. Chemical Thermodynamics 19.1 Spontaneous Processes Chemical thermodynamics is concerned with energy relationships in chemical reactions. We consider enthalpy and we also consider entropy in

More information

THERMODYNAMICS READ THE INSTRUCTIONS CAREFULLY

THERMODYNAMICS READ THE INSTRUCTIONS CAREFULLY TERMOYNMIS RE TE INSTRUTIONS REFULLY. The test is of hours duration.. The maximum marks are 60.. This test consists of 47 questions. 4. For each question in Section, & you will be awarded marks if you

More information

δs > 0 predicts spontaneous processes. U A + U B = constant U A = U B ds = ds A + ds B Case 1: TB > TA (-) (-) (+)(+) ds = C v(t )

δs > 0 predicts spontaneous processes. U A + U B = constant U A = U B ds = ds A + ds B Case 1: TB > TA (-) (-) (+)(+) ds = C v(t ) ---onight: Lecture 5 July 23 δs > 0 predicts spontaneous processes. ---Assignment 2 (do not include 1-3 done in-class): Due Friday July 30: Class time ---Assignment 3 posted ater class tonight. Whatever

More information

Chapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics

Chapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics Chapter 8 Thermochemistry: Chemical Energy Chapter 8 1 Chemical Thermodynamics Chemical Thermodynamics is the study of the energetics of a chemical reaction. Thermodynamics deals with the absorption or

More information

Chemical Thermodynamics

Chemical Thermodynamics Page III-16-1 / Chapter Sixteen Lecture Notes Chemical Thermodynamics Thermodynamics and Kinetics Chapter 16 Chemistry 223 Professor Michael Russell How to predict if a reaction can occur, given enough

More information

Chapter 17. Free Energy and Thermodynamics. Chapter 17 Lecture Lecture Presentation. Sherril Soman Grand Valley State University

Chapter 17. Free Energy and Thermodynamics. Chapter 17 Lecture Lecture Presentation. Sherril Soman Grand Valley State University Chapter 17 Lecture Lecture Presentation Chapter 17 Free Energy and Thermodynamics Sherril Soman Grand Valley State University First Law of Thermodynamics You can t win! The first law of thermodynamics

More information

Lecture 3 Evaluation of Entropy

Lecture 3 Evaluation of Entropy Lecture 3 Evaluation of Entropy If we wish to designate S by a proper name we can say of it that it is the transformation content of the body, in the same way that we say of the quantity U that it is the

More information

1. III only 2. II, III. 3. II only. 4. I only 5. I, III. 6. I, II, III correct

1. III only 2. II, III. 3. II only. 4. I only 5. I, III. 6. I, II, III correct Version 001 EXAM 8 PRACTICE PROBLEMS chemistry (78712) 1 This print-out should have 20 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001

More information

Remember Chapter 12.1 Introduction to Kinetic Molecular Theory and Intermolecular forces

Remember Chapter 12.1 Introduction to Kinetic Molecular Theory and Intermolecular forces Remember Chapter 12.1 Introduction to Kinetic Molecular Theory and Intermolecular forces 1 To understand properties, we want to connect what we see to what is happening on a molecular level. Start with

More information

Chapter 17: Spontaneity, Entropy, and Free Energy

Chapter 17: Spontaneity, Entropy, and Free Energy Chapter 17: Spontaneity, Entropy, and Free Energy Review of Chemical Thermodynamics System: the matter of interest Surroundings: everything in the universe which is not part of the system Closed System:

More information

Class work on Calorimetry. January 11 and 12, 2011

Class work on Calorimetry. January 11 and 12, 2011 Class work on Calorimetry January 11 and 12, 2011 Name 1. The number of calories needed to raise the temperature of 100 grams of water 10 degrees Celsius is the same as the number of calories needed to

More information

Handout 12: Thermodynamics. Zeroth law of thermodynamics

Handout 12: Thermodynamics. Zeroth law of thermodynamics 1 Handout 12: Thermodynamics Zeroth law of thermodynamics When two objects with different temperature are brought into contact, heat flows from the hotter body to a cooler one Heat flows until the temperatures

More information

Classes at: - Topic: Thermodynamics. = E v. = G f T 1

Classes at: - Topic: Thermodynamics. = E v. = G f T 1 PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna Topic:

More information

Temperature C. Heat Added (Joules)

Temperature C. Heat Added (Joules) Now let s apply the heat stuff to real-world stuff like phase changes and the energy or cost it takes to carry it out. A heating curve...a plot of temperature of a substance vs heat added to a substance.

More information

Identify the intensive quantities from the following: (a) enthalpy (b) volume (c) refractive index (d) none of these

Identify the intensive quantities from the following: (a) enthalpy (b) volume (c) refractive index (d) none of these Q 1. Q 2. Q 3. Q 4. Q 5. Q 6. Q 7. The incorrect option in the following table is: H S Nature of reaction (a) negative positive spontaneous at all temperatures (b) positive negative non-spontaneous regardless

More information

The First Law of Thermodynamics

The 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 information

Physics 202 Homework 5

Physics 202 Homework 5 Physics 202 Homework 5 Apr 29, 2013 1. A nuclear-fueled electric power plant utilizes a so-called boiling water reac- 5.8 C tor. In this type of reactor, nuclear energy causes water under pressure to boil

More information

b. Free energy changes provide a good indication of which reactions are favorable and fast, as well as those that are unfavorable and slow.

b. Free energy changes provide a good indication of which reactions are favorable and fast, as well as those that are unfavorable and slow. Chem 130 Name Exam 3, Ch 7, 19, 14 November 9, 2018 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct

More information

Chem 75 Winter, 2017 Practice Exam 1

Chem 75 Winter, 2017 Practice Exam 1 This was Exam 1 last year. It is presented here with, first, just the problems and then with the problems and their solutions. YOU WILL BENEFIT MOST if you attempt first just the problems as if you were

More information

Chapter Eighteen. Thermodynamics

Chapter Eighteen. Thermodynamics Chapter Eighteen Thermodynamics 1 Thermodynamics Study of energy changes during observed processes Purpose: To predict spontaneity of a process Spontaneity: Will process go without assistance? Depends

More information

Heating and Cooling Curves

Heating and Cooling Curves Heating and Cooling Curves $ Under normal circumstances, particles will undergo more than one type of change when heated or cooled $ During a phase change, the temperature will not change $ Parts of the

More information