'Standard enthalpy change' presentation slideshows

Energetics

Energetics. Exothermic and Endothermic reactions. Energy = force x distance (Joules). In chemical reactions, we need energy usually in the form of heat. Energy is absorbed to break the bonds of the reactants and energy is given out when new bonds are formed in the products.

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Standard Thermodynamic Functions of Reaction

Standard Thermodynamic Functions of Reaction. Miss Anis Atikah binti Ahmad Email: hakitasina@gmail.com. Subtopics. Standard states of pure substance Standard Enthalpy of Reaction Standard Enthalpy of Formation Determination of Standard Enthalpies of Formation and Reaction. Introduction.

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Energetics

Energetics. IB Topics 5 & 15 PART 1: Heat and Calorimetry. Above: thermit rxn. Energy: a measure of the ability to do work. Work: to move an object against an opposing force. Energy (J) = Force (N) x Distance (m)

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Energetics

Energetics. IB. Exothermic and Endothermic. Chemical reactions involves the breaking and the making of bonds. Energy is needed to break down a bond. Energy is released when a bond is formed. If more energy is released than is absorbed, the reaction will be Exothermic.

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Stoichiometry

Stoichiometry. Chemistry 6.0. The Mathematics of Chemical Reactions: STOICHIOMETRY. I. Balanced Chemical Equations A. Provide qualitative and quantitative information B. Supports the Law of Conservation of Matter 2H 2 + O 2 ? 2H 2 O

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5.1 Exothermic reactions

Topic 5- energetics SL 5.1 Exothermic and endothermic reactions 5.2 Calculation of Energy/Enthalpy Changes 5.3 Hess law 5.4 Bond enthalpy. 5.1 Exothermic reactions. Heat is produced and transferred to surroundings NaOH (s ) + H 2 O ? NaOH ( aq ) + heat

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Thermochemistry

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Thermochemistry

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Tutorial 5: Question 11

Tutorial 5: Question 11. Presented by 12S7F Yu Tian :D. Problem statement >.<. Aluminium fluoride is made industrially by reacting aluminium oxide with hydrogen fluoride at a high temperature . Al 2 O 3 (s) + 6HF (g) ? 2A l F 3 (s) + 3H 2 O (g). Problem statement >.<. UNIT:

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THE REPORT RESULT OF EXPERIMENT HESS LAW

THE REPORT RESULT OF EXPERIMENT HESS LAW. BY MARCIA SRI PURWANTININGSIH. Hess Law. Aim Observe the enthalpy of reaction between NaOH solid and HCl solution with two ways . APPRATUS /CHEMICALS Apparatus: Beaker Glass 250 mL Thermometer Materials: NaOH solid

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15.2 Born-Haber Cycle

15.2 Born-Haber Cycle. 15.2.1 Define and apply the terms lattice enthalpy, and electron affinity 15.2.2 Explain how the relative sizes and the charges of ions affect the lattice enthalpies of different ionic compounds

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Spontaneity

Spontaneity. IB Chemistry HL. In this part of Energetics we learn: Predict whether a reaction or process will be spontaneous by using the sign of ?G o

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Molar Enthalpies of Formation

Molar Enthalpies of Formation. When comparing enthalpy changes for formation reactions of different compounds, we must choose a reference energy state . It is convenient to set the enthalpies of elements in their most stable form at SATP to be zero. .

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Heat & Enthalpy Changes

Heat & Enthalpy Changes. Objectives: 1. Define the terms enthalpy and enthalpy changes. 2. Explain what information is given by the standard enthalpy change of a reaction. 3. Explain how a calorimeter is used to determine the quantity of heat transferred in a chemical reaction. Key Terms:

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More enthalpy changes

More enthalpy changes. L.O.: Define and apply the terms enthalpy of hydration and enthalpy of solution. Calculate enthalpies of solution for ionic compounds from lattice enthalpies and enthalpies of hydration.

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Heats of Formation

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Born Haber Cycles and Enthalpy

Born Haber Cycles and Enthalpy. 24/10/13. Energy Changes. First Law of Thermodynamics states that energy is always conserved. For a chemical reaction, the reaction mixture is referred to as the System. Everything else (test tube, surrounding air etc ) is referred to as the Surroundings.

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Thermit Reaction

What happened when the thermit black mixture was ignited? A great deal of sparks, flames, and smoke were produced almost as soon as the thermit was lit. Molten iron could also be seen. The reaction was quick and did not last very long.

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