'Standard enthalpy' diaporamas de présentation

Thermochemical principles includes: transfer of heat between the system and the surroundings

Thermochemical principles includes: transfer of heat between the system and the surroundings the enthalpy change for any process is the sum of the enthalpy changes for the steps into which the process can be divided

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AP Chemistry Final Exam Review

AP Chemistry Final Exam Review. Chapter 1. Matter and Measurements. Important Terms. Atom Element Law Of Definite Proportions. Mixture Solution Physical Properties Chemical Properties. Intensive Property Extensive Property SI units. Precision Accuracy Significant figures

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Phases or states of matter

Phases or states of matter:. Phases or states of matter. The physical properties of solids, liquids, and gases. LIQUIDS. The particles in a liquid are fairly well ordered over a short distance, but there is no long range order.

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PHYSICAL CHEMISTRY ERT 108 Semester II 2010/2011

PHYSICAL CHEMISTRY ERT 108 Semester II 2010/2011. Huzairy Hassan School of Bioprocess Engineering UniMAP. Standard Thermodynamic Functions of Reaction. Introduction.

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Chapter 15 - Standard enthalpy change of a reaction

Chapter 15 - Standard enthalpy change of a reaction. Standard Enthalpy Changes Hana Amir and Madeley. Any reaction that depends on temperature , pressure and state The enthalpy change happens when all reactants and products are in their standard state. Definition. Enthalpy of reaction

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Some Thermodynamic Terms

Some Thermodynamic Terms. Notice that the energy change in moving from the top to the bottom is independent of pathway but the work required may not be! Some examples of state functions are:

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Thermochemistry

Thermochemistry. AP Chemistry Seneca Valley SHS. Chapter 6. 6.1 The Nature of Energy. Kinetic and Potential Energy Energy: the capacity to do work or produce heat. Kinetic energy: energy an object has due to its motion Potential energy: energy due to position or composition.

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THERMOCHEMISTRY

THERMOCHEMISTRY. Courtesy of lab-initio.com. Definitions #1. Energy : The capacity to do work or produce heat. Potential Energy : Energy due to position or composition. Kinetic Energy : Energy due to the motion of the object. Definitions #2.

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Chemical Thermodynamics 2013/2014

Chemical Thermodynamics 2013/2014. 5 th Lecture:Thermochemistry Valentim M B Nunes, UD de Engenharia. Thermochemistry. The study oh heat required or produced by chemical transformations is called thermochemistry . Its an application of the first Law. Remember: q p = ? H and q V = ? U.

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STANDARD MOLAR ENTHALPY OF FORMATION

STANDARD MOLAR ENTHALPY OF FORMATION. Enthalpy change when 1 mol of species is formed in its Standard State at a Specified Temperature from the most stable forms of its constituent elements in their standard forms (at the same temperature). MOST STABLE FORM OF ELEMENT.

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ME 475/675 Introduction to Combustion

ME 475/675 Introduction to Combustion. Lecture 3. Thermodynamic Systems (reactors). Closed systems Open Steady State, Steady Flow (SSSF ) Systems How to find changes, and , for mixtures when temperatures and composition change due to reactions (not covered in Thermodynamics I).

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For which of the following substances does ? H 0,f298 = 0?

For which of the following substances does ? H 0,f298 = 0?. ZnO(s) H 2 O(l) Hg(l) I 2 (l) C(diamond).

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Calculating ? H using molar heats of formation

Calculating ? H using molar heats of formation. Chem 12. If 1 mol of compound is formed from its constituent elements, then the enthalpy change for the reaction is called the enthalpy of formation, ? H o f . Standard conditions (standard state): 1 atm and 25 o C (298 K).

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Enthalpies of Formation and Reaction

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Chapter 6 - Thermochemistry

Chapter 6 - Thermochemistry. Section 6.1 The Nature of Energy. Energy Law of Conservation of Energy Potential energy Kinetic energy Heat Work Pathway State function or property Chemical Energy. Chemical Energy. System Surroundings Exothermic Endothermic Thermodynamics

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Bond & Group Enthalpies

Bond & Group Enthalpies. The standard entahlpy change associated with breaking the bond in a diatomic molecule in the gas phase: N ? N (g) -------> 2 N (g) D H [N ? N] = + 946 kJ / mole of N ? N bonds

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4. free energy

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Thermochemical Stoichiometry Problems

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Example using enthalpy of combustion and formation

Example using enthalpy of combustion and formation. Construct an enthalpy cycle and calculate the value of ? H f ? (C 2 H 5 OH(l)) given the following data :. Determine enthalpy change for SO 2 ( g ) + 2H 2 S ( g ) --> 2H 2 O ( l ) + 3S ( s ) Use the following values (all in kJ )

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