Results of Midterm 2 0 102030405060708090 points # of students GradePoints A85-100 B+B+ 75-84 B60-74 C+C+ 50-59 C30-49 D,F<30 100 # of students Midterm.

Slides:

Advertisements

Similar presentations

Use of Steam Tables Saturated Vapor or Liquid

Advertisements

The Ideal Gas Ideal Gas Law Van der Waals Equation Distribution of Molecular Speeds.

First Law of Thermodynamics

Lecture 15. Phases of Pure Substances (Ch.5) Up to now we have dealt almost exclusively with systems consisting of a single phase. In this lecture, we.

Ch15 Thermodynamics Zeroth Law of Thermodynamics

Lecture 19 Overview Ch. 4-5 List of topics Heat engines

Chapter 16 Chemical and Phase Equilibrium Study Guide in PowerPoint to accompany Thermodynamics: An Engineering Approach, 5th edition by Yunus.

Equilibrium A state in which opposing processes of a system are occurring at the same rate. 1.Physical (a) Saturated Solution – dissolution and crystallization.

Work, Heat and Internal Energy: The First Law. System – the specific part of the universe of interest to us Surroundings – the part of the universe not.

Entropy Change Property diagrams (T-s and h-s diagrams) –From the definition of the entropy, it is known that  Q=TdS during a reversible process. –Hence.

Entropy and the Second Law of Thermodynamics

1 CHEM 212 Chapter 3 By Dr. A. Al-Saadi. 2 Introduction to The Second Law of Thermodynamics The two different pressures will be equalized upon removing.

Results of Midterm points # of students GradePoints A B+B B60-74 C+C C30-49 D,F

Results of Midterm points # of students GradePoints A B+B B46-55 C+C C26-40 D,F

Lecture 294/16/07. Changes in temperature - recap Heat = (constant) x (mass) x (change in temp)

Absolute Zero Physics 313 Professor Lee Carkner Lecture 15.

Section 4 -Phase Equilibrium Two-Phase Systems A system is a set of components that are being studied. Within a system, a phase is a region that has the.

Phy 202: General Physics II Ch 15: Thermodynamics.

PM3125 Content of Lectures 1 to 6: Heat transfer: Source of heat

Properties of Pure Substances

Chapter 3 Phase Transitions and Chemical Reactions.

Chapter 17 Thermochemistry.

Spontaneity of Chemical and Physical Processes: The Second and Third Laws of Thermodynamics 1.

Chapter 15 Thermodynamics.

Chapter 15: Thermodynamics

Q19. Second Law of Thermodynamics

Prof. Fred Remer University of North Dakota Phase Changes and Latent Heat Where’s the heat? Solid Liquid Gas.

© 2005 Pearson Prentice Hall This work is protected by United States copyright laws and is provided solely for the use of instructors in teaching their.

Spontaneity and Equilibrium isolated system : Isothermal process  Maximum work obtained in a process at constant temperature is equal to the decrease.

Thermodynamics The First Law of Thermodynamics Thermal Processes that Utilize an Ideal Gas The Second Law of Thermodynamics Heat Engines Carnot’s Principle.

Thermal contact Two systems are in thermal (diathermic) contact, if they can exchange energy without performing macroscopic work. This form of energy.

Thermodynamics. System / environment Diathermal / adiabatic Walls between the system and surroundings are called diathermal if they permit energy flow.

ENGR 2213 Thermodynamics F. C. Lai School of Aerospace and Mechanical Engineering University of Oklahoma.

The Second Law of Thermodynamics

Temperature, Heat, and the First Law of Thermodynamics

32.1 Pressure Dependence of Gibbs’ Free Energy Methods of evaluating the pressure dependence of the Gibbs’ free energy can be developed by beginning with.

Entropy Change Property diagrams (T-s and h-s diagrams) from the definition of the entropy, it is known that Q=TdS during a reversible.

Equilibrium. Reversible Reactions Able to proceed in both directions (forward and reverse) PE (kJ) Reaction coordinate Forward AE f Reverse AE r HH.

Ch15 Thermodynamics Zeroth Law of Thermodynamics If two systems are in thermal equilibrium with a third system, then they are in thermal equilibrium with.

CHAPTER 15 Thermodynamics Thermodynamic Systems and Their Surroundings Thermodynamics is the branch of physics that is built upon the fundamental.

حرارة وديناميكا حرارية

Pressure – Volume – Temperature Relationship of Pure Fluids.

A more appropriate definition of K (for the same chemical reaction discussed previously) is With this definition, each concentration term is divided by.

Entropy Rate Balance for Closed Systems

Constant volume (isochoric) process No work is done by the gas: W = 0. The P-V diagram is a vertical line, going up if heat is added, and going down if.

ENGR 2213 Thermodynamics F. C. Lai School of Aerospace and Mechanical Engineering University of Oklahoma.

Thermodynamics Thermodynamics is a branch of physics concerned with heat and temperature and their relation to energy and work.

Phase of Water and Latent Heats

Equilibrium. Equilibrium is a state in which there are no observable changes as time goes by. Although there are still changes occurring, they are not.

Chapter 9 Heat.

CHEM 112 Spring 2011 Exam 1 Review.

Chapter 15 Thermodynamics Thermodynamic Systems and Their Surroundings Thermodynamics is the branch of physics that is built upon the fundamental.

Physics 101 Lecture 11. Thermal Physics Thermodynamics.

Introduction to Thermodynamics 1. 2 Thermodynamics is the branch of physics that is built upon the fundamental laws that heat and work obey. In thermodynamics.

Lecture 24Purdue University, Physics 2201 Lecture 24 Heat PHYSICS 220.

CHANGES IN TEMPERATURE AND PHASE Holt Chapter 10, Section 3.

15.1 Thermodynamic Systems and Their Surroundings

Thermodynamic Property Relations

Lecture 17 Overview Ch. 4-5 List of topics

11.3 Some Properties of Liquids

Chemical Equilibrium.

Steam Engine Sliding valve Steam enters chamber from

Quiz #1 for GP II, MATH, Spring 2012

Reflections on the Motive Power of Fire and

Reflections on the Motive Power of Fire and

Phase Diagram Vocabulary Triple Point: Only point at which all three phases (solid, liquid, gas) exist at equilibrium Critical Point: Point at which.

Thermochemistry.

Chemical Equilibrium Mass transfer takes place from higher chemical potential to lower chemical potential. If the chemical potential of reactants are.

Presentation transcript:

Results of Midterm points # of students GradePoints A B+B B60-74 C+C C30-49 D,F< # of students Midterm 1

Problem 1 (heat engine) 1 – 2 2 – 3 3 – 1 T1T1 P T2T V (20) The heat engine uses an ideal gas as its working substance. 1-2 is an isochoric process, 2-3 – adiabatic, 1-3 – isothermal. T 1 and T 2 are given. Find  Q for each process and the efficiency of the heat engine in terms of T 1 and T 2 (  =1+2/f, C V =(f/2)Nk B ). (10) Which way of increasing the efficiency of the Carnot heat engine is better – to increase the temperature of the hot reservoir by  T (  T <<T H, T C ) or to decrease the temperature of the cold reservoir by the same  T? Explain.

Problem 2 vdW (20) Two insulated tanks with volumes V 1 and V 2 are connected by a valve. Each tank contains one mole of the same monatomic van der Waals gas (the constants a and b are known). Initially, when the valve was closed, both gases were at the same temperature T i. The valve is open and the system reaches its equilibrium state. Find the equilibrium temperature T f. Is T f higher or lower than T i ? For which value of V 1 /V 2 you expect T f to be equal to T i? the temperature will decrease V 1, T i V 2, T i if

Problem 3 (phase transformations) (25) The pressure of the saturated water vapor at T = C is bar (these T and P correspond to the triple point of water). The latent heat of the solid-liquid transformation at C is 335 kJ/kg, the latent heat of the liquid-gas transformation is 2500 kJ/kg. Find the pressure of the saturated water vapor at T = -1 0 C. Along the solid-gas phase equilibrium curve: - the latent heat of sublimation at the triple point - we neglected the volume of solid and expressed the gas volume using the ideal gas law. n – the number of moles in 1 kg.

Problem 4 (chem. equilibrium) (25) Consider the following reaction at T = 298K and P = 1bar: H 2 CO 3 (aq)  HCO 3 -- (aq) + H + (aq) (a) Using the data in the Table on p.404, calculate  G for this reaction, and the equilibrium constant K. (b) If the initial amount of H 2 CO 3 is 1 mole, what will be the amounts of each reactant and product at equilibrium? The mass action law: Thus, in equilibrium, H 2 CO 3 HCO 3 -- H+H+ initial100 change-x+ x final1-xxx H 2 CO 3 HCO 3 -- H+H+  H (kJ) S (J/K)  G (kJ) To obtain the value of  G for the reaction, subtract  G of the reactants from  G of the products: