'Pure liquids' presentation slideshows

Equilibrium Basic Concepts

Equilibrium Basic Concepts. Reversible reactions do not go to completion. They can occur in either direction. Chemical equilibrium exists when two opposing reactions occur simultaneously at the same rate.

2.04k views • 139 slides

Chapter 11 Chemical Equilibrium

Chapter 11 Chemical Equilibrium. 11.1 The Equilibrium Condition 11.2 The Equilibrium Constant 11.3 Equilibrium Expressions Involving Pressures 11.4 The Concept of Activity 11.5 Heterogeneous Equilibria 11.6 Applications of the Equilibrium Constant 11.7 Solving Equilibrium Problems

1.08k views • 40 slides

Conduction and Breakdown in Liquid Dielectrics

Conduction and Breakdown in Liquid Dielectrics. Liquid as insulators. Liquid dielectrics, because of their inherent properties, appear as though they would be more useful as insulating materials than either solids or gases .

742 views • 29 slides

Chemical Equilibrium

Chemical Equilibrium. Brown, LeMay Ch 15 AP Chemistry Monta Vista High School. 15.1: Chemical Equilibrium. Occurs when opposing reactions are proceeding at the same rate Forward rate = reverse rate of reaction Ex: Vapor pressure: rate of vaporization = rate of condensation

484 views • 28 slides

Chemistry SM-1232 Week 10 Lesson 2

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Chemistry SM-1232 Week 10 Lesson 2

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Previously in Chem 104: Kinetics

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5.6 - Characteristic Physical Properties

5.6 - Characteristic Physical Properties. UNIQUE. Physical properties are used to describe substances. Most are NOT useful for identifying the substance.

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VI. The Equilibrium Constant

VI. The Equilibrium Constant. p. 57 - 60. The Equilibrium Constant, Keq. A (g) + B (g) = C (g) + D (g) Keq = [Products] = [Reactants]. 2A (g) + 3B (g) = 2C (g) + D (g) Keq =. Not Included in Keq:. solids pure liquids

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4.7 Kw and the Ionization of Water

4.7 Kw and the Ionization of Water. Chemistry 12 http://www.800mainstreet.com/acid_base/dissociation_of_water.html. 4.7. 2 H 2 O (l) + 59J ? H 3 O + (aq) + OH ? (aq) Spontaneous Not very often Affected by temperature. 4.7. 2 H 2 O (l) + 59J ? H 3 O + (aq) + OH ? (aq)

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Calculating Equilibrium Constants

Calculating Equilibrium Constants. Using the ICE method to solve for K. Heterogeneous Equilibrium. REMEMBER! p.623 Pure Solids or Pure Liquids are not included in equilibrium expressions because [Solids], [Liquids] are constant. Calculating Equilibrium Constants.

229 views • 6 slides