'Calculating equilibrium constants' presentation slideshows

Introduction to Chemical Equilibrium

Introduction to Chemical Equilibrium. CHEM 160. Chapter 15. The Concept of Equilibrium. Consider colorless frozen N 2 O 4 . At room temperature, it decomposes to brown NO 2 : N 2 O 4 ( g ) ? 2NO 2 ( g ). At some time, the color stops changing and we have a mixture of N 2 O 4 and NO 2 .

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Equilibrium

Equilibrium. L. Scheffler Lincoln High School 2009. 1. Equilibrium Systems. Many chemical reactions are reversible. Such reactions do not go to completion. There is a state of balance between the products and the reactants

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Chemical Equilibrium

Chemical Equilibrium. Chapter 15. The Equilibrium Condition Section 13.1. Consider the following reversible reaction: N 2 O 4 ( g ) 2NO 2 ( g ) Because the reaction is reversible, it has a rate for both the forward and backward reaction. Achieving Equilibrium.

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Chemical Equilibrium

Chemical Equilibrium. Recognizing Rxn Equilibrium. 1. The system is closed. Opposite rxns occur at the same rate. Equilibrium is reached by either starting w/ reactants or products. Temp is constant.

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Applications of the equilibrium constant

Applications of the equilibrium constant. The Extent of a Reaction The tendency for a reaction to occur is indicated by the magnitude of the equilibrium constant.

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Chapter 15

Chapter 15. Chemical Equilibrium. Overview. 15.1 The Concept of Equilibrium

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Based on CaCO 3 (s) CaO(s) + CO 2 (g), which

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