CHEM /27/11 III. A. 1st Law of Thermodynamics (Chapter 2)

Slides:

Advertisements

Similar presentations

Chapter 10 Thermodynamics

Advertisements

Chem Ch 19/#1 Today’s To Do List l Start Chapter 19: 1st Law P-V work State Functions 1st Law Adiabatic Processes.

Chapter 7: Thermochemistry

Thermodynamics: The First Law 자연과학대학 화학과 박영동 교수 Classical thermodynamics.

Mechanical equivalent of heat Joule (1843) Under adiabatic conditions 1 °F increase when 772 lb dropped 1 foot J = 1 cal 1 J ≡ amount of work required.

Thermodynamic Property Relations

Lecture 334/25/05. 1 st Law of Thermodynamics revisited ∆E = q + w Change in Energy content heat work.

Chem. 412 – Phys. Chem. I. Sign Convention System Surroundings  ΔU = Internal Energy.  q = heat flow; transfer of energy between two objects.  w =

Fig The net work done by the system in the process aba is –500 J.

Prentice-Hall © 2007 General Chemistry: Chapter 7 Slide 1 of 58 CHEMISTRY Ninth Edition GENERAL Principles and Modern Applications Petrucci Harwood Herring.

Chapter 51 Chapter 6 Thermochemistry Jozsef Devenyi Department of Chemistry, UTM.

Thermodynamics Thermodynamics is the study of systems involving energy in the form of heat and work.

Chapter 6 THERMOCHEMISTRY West Valley High School AP Chemistry Mr. Mata.

Chapter 21 Basic Concepts of Thermodynamics Thermodynamics is the study of transformations of energy System and surroundings –the system is the part of.

Atkins’ Physical Chemistry Eighth Edition Chapter 2 The First Law Copyright © 2006 by Peter Atkins and Julio de Paula Peter Atkins Julio de Paula.

A 3.51 g sample of benzene, C 6 H 6, was burned in a bomb calorimeter in an excess of oxygen. The initial temperature was o C and rose to

Thermodynamics. Thermodynamic Process in which energy is transferred as heat and work.

Chapter 5 Thermochemistry

50 mL 100 o 100 mL 25 o 150 mL (4.184 J/ o C g) q = C x  T x mass q 2 = (4.184 J/ o C g) x q 1 = - q 2 (T f - 100) x (50) = T f = 50 o C q 1 =x (T f -

Thermodynamics Chapter 15. Figure 15-1 An ideal gas in a cylinder fitted with a movable piston.

Thermochem Quick review

Chapter 5 - Thermochemistry Heat changes in chemical reactions.

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

Spontaneity, Entropy & Free Energy.  1 st Law of Thermodynamics  Spontaneous processes  Entropy (S)  Position probability  States of matter  Page.

Prentice-Hall © 2002General Chemistry: Chapter 7Slide 1 of 50 Chapter 7: Thermochemistry Philip Dutton University of Windsor, Canada Prentice-Hall © 2002.

Marzena Dzida, Mirosław Chorążewski University of Silesia, Institute of Chemistry, Szkolna 9, Katowice The effect of temperature and pressure on the thermodynamic.

Thermochemistry Chapter 6. The Nature of Energy Energy is the capacity to do work or produce heat. Energy is the capacity to do work or produce heat.

when system is subdivided? Intensive variables: T, P Extensive variables: V, E, H, heat capacity C.

CHEM 433 – 9/22/11 II. Gases – finish van der Waals Equation. (1.4) III. 1st Law of Thermodynamics (Chapter 2) - Introduction & Definitions (2.1) - Internal.

THERMOCHEMISTRY.

THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:

By Miss Anis Atikah Ahmad

Thermodynamics Chapter 15. Part I Measuring Energy Changes.

THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:

AgNO 3 + HCl  When 50.0 mL of M AgNO 3 and 50.0 mL of M HCl are mixed in a coffee-cup calorimeter, the mixture’s temperature increases from.

THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:

First Law of Thermodynamics

The first law of Thermodynamics. Conservation of energy 2.

B2 Thermodynamics Ideal gas Law Review PV=nRT P = pressure in Pa V = volume in m3 n = # of moles T= temperature in Kelvin R = 8.31 J K -1 mol -1 m = mass.

THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:

CALORIMETRY HEAT OF COMBUSTION RESONANCE ENERGY OF BENZENE.

Chapter 51 Thermochemistry. 2 The Nature of Energy From Physics: Force – a kind of push or pull on an object. Energy – the capacity to do work. Work –

Energy The capacity to do work or to produce heat.

Prentice Hall © 2003Chapter 5 Chapter 5 Thermochemistry CHEMISTRY The Central Science 9th Edition David P. White.

© 2009, Prentice-Hall, Inc. Bomb Calorimetry Reactions can be carried out in a sealed “bomb” such as this one. The heat absorbed (or released) by the water.

THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:

ERT 108/3 PHYSICAL CHEMISTRY FIRST LAW OF THERMODYNAMICS Prepared by: Pn. Hairul Nazirah Abdul Halim.

Chapter 6 Energy Law of Conservation of Energy Potential vs Kinetic Heat – transfer of Energy because of temp. difference.

THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:

Monday 13 October 2014 Read: –Section 3.3. Problems: –3.16, 3.18, 3.22, 3.36.

Thermochemistry 3 Calorimetry & Heat of Formation.

Chapter 5 Thermochemistry

ERT 108/3 PHYSICAL CHEMISTRY EXERCISES FIRST LAW OF THERMODYNAMICS

1st law of thermodynamic

Chapter 2 The First Law Unit 3 adiabatic process

Chapter 18 Temperature, Heat, and the First Law of Thermodynamics

The Laws of Thermodynamics

Studies energy changes and the direction of flow of energy

University of North Carolina, Wilmington

Chapter 3 The 2nd law of thermodynamics

CHEM 433 – 10/11/11 III. 1st Law: “Machinery” ( )

Thermochemistry Chapter 6.

Thermodynamics tutorhour 1

CHEM 433 – 10/4/11 III. 1st Law: Adiabatic changes (2.6)

Pressure - Volume Graph

Thermodynamics tutorhour 2

CHEM /23/10 III. A. 1st Law of Thermodynamics (Chapter 2)

Chapter 19 The kinetic theory of gases

Consider an isothermal reversible expansion of an ideal gas

Presentation transcript:

CHEM 433 - 9/27/11 III. A. 1st Law of Thermodynamics (Chapter 2) - expansion work (Rev isothermal) - Heat Transactions (2.4) —> Heat Capacity • READ: Chapter #2 (1 – 4)

Constant Pressure Expansion… w = –pextV

Isothermal Reversible Expansion… w = –nRTln(V2/V1) More work in this case: reversible system is pushing against maximum possible pressure…

A constant volume a.k.a. “Bomb” Calorimeter…

How much energy is needed to heat 1 mol of CO2 (g) from 298K to 348K (at constant volume)? What does this process look like on a plot of p vs. V? 1.0 kJ p T2 T1 V