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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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Jeopardy

Jeopardy. 100: Stoichiometry , Atomic/Molecular Structure. How many atoms are in 23 g of potassium? Answer. 200: Stoichiometry , Atomic/Molecular Structure.

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Combined and ideal gas laws

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Chapter 11

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Chapter 16 Kinetics

Chapter 16 Kinetics. Dinosaurs generated enough heat to sustain its biochemical reactions at high rates . Reaction rate = f(temperature). What is chemical kinetics?. Deals with the speed (rate) of a chemical reaction and its reaction mechanism .

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Chapter 2

Chapter 2. Answer Key. Section 2.1, Page. Section 2.2, Page 68 .

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Final Grade for CHE 103

Final Grade for CHE 103. Calculated as stated in syllabus: EXAM1 + EXAM2 + EXAM 3 + QUIZZES 350. Outline. I. Gases & Gas Laws - Kinetic Molecular Theory - Simple variable relationships - Ideal/Combined Gas Law.

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GAS LAWS!

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Ideal Gas Law

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Applications of Equilibrium Constants

Applications of Equilibrium Constants. Example. For the reaction below 2A + 3B ? 2C A 1.5L container is initially charged with 2.3 mole of A and 3.0 mole of B. At equilibrium, .75 mole of A is present. Calculate the value of the equilibrium constant. Example.

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Equilibrium Calculations Lesson 2

Equilibrium Calculations Lesson 2. How can we describe an equilibrium system mathematically? Keq = = 2.5 The Keq is the equilibrium constant - a number that does not change. Providing the temperature is kept constant. products. reactants. products. reactants.

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Gas Laws Practice

Gas Laws Practice. How many grams of carbon dioxide gas are there in a 62.3 L container at 37 ?C and 1.12 atm.

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