'Endothermic reactions' presentation slideshows

General Chemistry

General Chemistry. 1 st Semester Review. Chapter 2. Qualitative observation : describes matter without using numbers Ex: Quantitative observation : describes matter using measurements Ex:. Classifying Matter by Composition.

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Chemistry 112

Chemistry 112. Overview of Chapters 5, 8, 16, & 9. Chapter 5 Highlights. Chemical reactions involve energy. There are two types of energy: potential (stored) and kinetic (energy of motion).

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Fire Behavior

5. Fire Behavior. Objectives (1 of 4). Describe the chemistry of fire. Define the three states of matter. Describe how energy and work are interrelated. Describe the conditions needed for a fire. Explain the chemistry of combustion. Describe the products of combustion.

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Chemical Reactions

Chemical Reactions. Chapter 14 Material on Midterm. A model formula. Chemicals react in very precise ways. In this activity, you will model a chemical reaction and will predict how chemicals react. Section 1: Forming New Substances. Objectives:

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Chemical Reactions

Chemical Reactions. Energy and Reaction Rates. Chemical Reactions. Chemical reactions require energy to start Activation E nergy - Energy needed to start a chemical reaction Endothermic reactions take in energy Exothermic reactions give off energy. Chemical Reactions. Chemical Reactions.

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Chemical Reactions

Chemical Reactions. And Enzymes. A chemical reaction is a process that changes, or transforms, one set of chemicals into another. Mass and energy are conserved Reactants become products Always involve changes in the chemical bonds that join the atoms of the compounds.

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Chapter 7:

Chapter 7:. Chemical Reactions. 7.1: Chemical reactions alter arrangements of atoms. Atoms interact in chemical reactions: Chemical reaction: produces new substances by changing the way in which atoms are arranged. Bonds between atoms are broken New bonds are formed.

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Forensic Aspects of Fire Investigation

Forensic Aspects of Fire Investigation. Objectives: Define oxidation. Define energy and give examples of its different forms. Describe the role of heat energy in chemical reactions. Define heat of combustion and ignition temperature.

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7.3 Exothermic and Endothermic Reactions

7.3 Exothermic and Endothermic Reactions. Review Stuff from 7.1. Chemical reactions involve the breaking of chemical bonds in the reactants and the formation of chemical bonds in the products . Reactants are on the left side Products are on the right side. Law? What law?.

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Chemical Engineering and Sustainability

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Thermochemistry

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Enthalpy

Enthalpy. Calorimetry of Chemistry. Enthalpy. During a chemical reactions bonds are broken and/or made . When this occurs we can gain or lose chemical potential energy.

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Changes in matter

Changes in matter. Physical and Chemical Properties Physical and Chemical Changes Observable Features of Chemical Reactions. Physical properties. used to identify substances used to classify substances used to determine effective building materials. Examples of physical properties.

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Reaction Energy and Reaction Kinetics

Reaction Energy and Reaction Kinetics. Driving Force of Reactions. Objectives. Explain the relationship between enthalpy change and the tendency of a reaction to occur. Explain the relationship between entropy and the tendency of a reaction to occur.

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Reactions and Corrosion

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Chemical equilibrium

Finding a balance (between reactants & products). Chemical equilibrium. Has been reached when the concentration of reactants and products are constant Dynamic equilibrium : The rate of formation of reactants = the rate of formation of products.

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Reaction Spontaneity and Entropy

Reaction Spontaneity and Entropy. Thermochemical Reactions Lecture 3. Spontaneous Processes. A spontaneous process is a physical or chemical change that occurs with no outside intervention. However, for many spontaneous processes, some energy must be supplied to get the process started.

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RATES OF REACTION

RATES OF REACTION. Rates of Reaction. The rate of a chemical reaction is the speed at which the reaction occurs (i.e. speed at which the reactants are used or products are produced). Rate can be measured by the: 1) change in mass of reactants or products . 2) change in pH

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Energy Changes

Section D3.3. Energy Changes. Bond Energy. Energy associated with bonds Exothermic reactions: Energy is released Produces an increase in temperature May produce light Reactants ? Products and Energy. Endothermic Reaction. A reaction in which energy is absorbed

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