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Thermochemistry

AP Chemistry Zumdahl 7E Chapter 16 Notes

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Chemistry
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State functions
Thermodynamic entropy
Chemical thermodynamics
thermodynamics
Thermochemistry
Spontaneous process
Entropy
Hess's law
Standard molar entropy
gibbs free energy
Enthalpy
Chemical reaction

1 Chapter 16 - Spontaneity, Entropy, and Free Energy 16.1 Spontaneous Processes and Entropy A. First Law 1. "Energy can neither be created nor destroyed" 2. The energy of the universe is constant B. Spontaneous Processes 1. Processes that occur without outside intervention 2. Spontaneous processes may be fast or slow a. Many forms of combustion are fast b. Conversion of diamond to graphite is slow C. Entropy (S) 1. A measure of the randomness or disorder 2. The driving force for a spontaneous process is an increase in the entropy of the universe 3. Entropy is a thermodynamic function describing the number of arrangements that are available to a system a. Nature proceeds toward the states that have the highest probabilities of existing D. Positional Entropy

AP Chemistry Zumdahl 7E Chapter 6 Notes

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Chemistry
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Thermochemistry
Chemical thermodynamics
Thermodynamic processes
Physical chemistry
Chemistry
Enthalpy
Standard enthalpy of formation
Exothermic reaction
Hess's law
Exothermic process
Calorimeter
Endothermic process

AP Chemistry A. Allan Chapter Six Notes - Thermochemistry 6.1 The Nature of Energy A. Definition 1. Energy is the capacity to do work (or to produce heat*) a. Work is a force acting over a distance (moving an object) b. *Heat is actually a form of energy. (1) chemicals may store potential energy in their bonds that can be released as heat energy B. Law of Conservation of Energy 1. Energy can be converted from one form to another, but cannot be created or destroyed a. Potential energy (1) energy due to position or composition b. Kinetic energy (1) energy due to the motion of an object (2) vmKE 22 1= C. Heat and Temperature 1. Temperature reflects random motion of particles in a substance 2. Temperature indicates the direction in which heat energy will flow

AP Bio Chp. 8

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Biology
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metabolism
Catalysis
Thermochemistry
cellular respiration
Thermodynamic processes
Enzyme
Adenosine triphosphate
Endergonic reaction
Chemical reaction
Product
Endergonic
Metabolic pathway

AP Biology Reading Guide Chapter 8: An Introduction to Metabolism Fred and Theresa Holtzclaw Copyright ? 2010 Pearson Education, Inc. - 7 - AP Biology Reading Guide Chapter 8: An Introduction to Metabolism Fred and Theresa Holtzclaw Copyright ? 2010 Pearson Education, Inc. - 1 - Name _________________________________________________ MOD____________ Date ________ Chapter 8: An Introduction to Metabolism Concept 8.1 An organism?s metabolism transforms matter and energy, subject to the laws of thermodynamics 1. Define metabolism. 2. There are two types of reactions in metabolic pathways: anabolic and catabolic. a. Which reactions release energy? b. Which reactions consume energy?

Chapter 7

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Chemistry
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Chemistry
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thermodynamics
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Chemical engineering
Thermochemistry
Chemical properties
Calorimeter
Heat
Exothermic
Enthalpy
energy
Environment
behavior
Human development
Interpersonal relationships
Love
Psychoanalysis
Human behavior
Attachment theory
Evolutionary biology
Personal life
Technology

Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 18 October 2012 Brady, Jespersen, Hyslop Chapter 7 Energy & Chemical Change Thermochemistry: the study of energy flow during a chemical reaction Ch. 7.1 Energy: the ability to do work; often measured as heat Kinetic Energy: the energy of motion; KE = ?mv2 Potential Energy: stored or positional energy; chemical energy (no simple eqn.) Conservation of Energy: 1. Energy cannot be created or destroyed 2. Energy is only converted from one form to another (KE ? PE) 3. Total energy of the universe (or an isolated system) is constant Thermochemistry: Basic Definitions Units of Energy 1 Joule (J) ? the KE possessed by a 2 kg object moving at a velocity of 1 m/s 1 cal = 4.184 J (exactly) 1 kcal = 4.184 kJ

AP Chemistry Chapter 6 Outline

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Chemistry
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Chemistry
thermodynamics
Physics
Thermochemistry
State functions
Chemical thermodynamics
Physical chemistry
Standard enthalpy of formation
Exothermic reaction
Calorimeter
Chemical energy
Exothermic
Environment

Daniel Seo 10/10/13 Period 5 Chapter 6 Thermochemistry Outline 6.1 The Nature of Energy 1. Energy ? capacity to do work (or to produce heat) i. Work ? force acting over a distance (moving an object) ii. Heat ? form of energy. ? chemicals may store potential energy in their bonds that can be released as heat energy 2. The law of conservation of mass ? energy can be converted from one form to another, but cannot be created or destroyed ? is also the first law of thermodynamics. i. Potential energy ? energy due to position or composition ii. Kinetic energy ? energy due to the motion of an object ? K? = 1/2mv2 3. Temperature reflects random motion of particles in a substance 4. Temperature indicates the direction in which heat energy will flow

Chapter 5 Thermochemistry

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Chemistry
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Physics
thermodynamics
Chemistry
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Thermochemistry
Enthalpy
energy
Heat
Exothermic
internal energy
Thermal energy
Thermodynamic system
Environment

Chapter 5: Thermochemistry ?Introduction- Energy is defined as the capacity or the ability the to do work i.e. in order to do work energy must be involved Mathematically Represented- Work or Energy = Force x Distance The view of energy can be thought of as physical in nature and contact via the exerted force Chemistry, however, must view energy differently. The study of energy and its transformation, as it applies to chemistry, is know as THERMOCHEMISTRY, along with spontaneity, the two are referred to as THERMODYNAMICS Section 5.1- Nature of Energy The study of chemistry and thermodynamics will involve the concepts of energy, work, and heat KINETIC and POTENTIAL Energy Kinetic ? energy due to an objects motion

Hess's Law

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Notes Enthalpy / Hess?s Law 2/13/13 CH 4(g) + 2O 2(g) ? CO 2(g) + 2H 2 O (g) ?H? rxn =? ?H? rxn = ??H? f products - ??H? f reactants Electron Affinity: Energy change associated with adding electrons to atoms (anions) Ionization Energy: Energy change associated with removing electrons from atoms (cations) Methods for calculating ?H rxn Hess?s Law: if a reaction can be written as the sum of two or more steps the overall enthalpy of reaction is equal to the sums of the enthalpies of reaction for each of the steps A + B ? G + H ? ?H rxn =? A + B ? C + D ? ?H rxn = x KJ C + D ? E + F ? ?H rxn = y KJ E + F ? G + H ? ?H rxn = z KJ +___________ A + B ? G + H ? ?H rxn = x + y + z KJ
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