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Chapter 4 Chemical Quantities and Aqueous Reactions

Chemistry: A Molecular Approach , 1 st Ed. Nivaldo Tro. Chapter 4 Chemical Quantities and Aqueous Reactions. Roy Kennedy Massachusetts Bay Community College Wellesley Hills, MA. 2008, Prentice Hall. Reaction Stoichiometry.

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Chapter 15: Chemical Equilibrium

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Chemistry 102(001) Fall 2012

Chemistry 102(001) Fall 2012. CTH 328 10:00-11:15 am Instructor : Dr. Upali Siriwardane e-mail : upali@latech.edu Office : CTH 311 Phone 257-4941 Office Hours : M,W 8:00-9:00 & 11:00-12:00 am; Tu , Th , F 8:00 - 10:00am.. Exams: 10 :00-11:15 am, CTH 328.

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Spontaneity and Equilibrium

Spontaneity and Equilibrium. isolated system : . Isothermal process. Maximum work obtained in a process at constant temperature is equal to the decrease in Helmholtz energy of the system. Calculate the maximum work that can be obtained from the combustion of 1 mole of methane at 298 K.

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This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License

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Chapter 15

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Types of Chemical Reactions

Types of Chemical Reactions. Chemical Reactions. Chemical reactions are grouped according to patterns in the chemical formulas. Synthesis Reactions. Two reactants combine to make a larger or more complex product. Synthesis Reactions. Synthesis Reactions.

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Chemical Quantities Chapter 9

Chemical Quantities Chapter 9. Information Given by the Chemical Equation. Balanced equation provides the relationship between the relative numbers of reacting molecules and product molecules 2 CO + O 2 ? 2 CO 2 2 CO molecules react with 1 O 2 molecules to produce 2 CO 2 molecules.

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Stoichiometry Race

Stoichiometry Race . Rules . You can only work with your partner All your work must be shown on the white board First team gets 3 points Second team gets 2 points Third team gets 1 point Team with the highest score gets bubble gum!. Molar Mass. Determine the molar mass for the following:

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Equilibrium Systems and Stress

Equilibrium Systems and Stress . Chemical Equilibrium. Chemical Equilibrium When the rates of the forward and reverse reactions are equal in a chemical reaction The concentration (amount) of reactants and products of the reaction remains the same Ex: 2CO (g) + O 2(g) ? 2O 2(g).

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Combustion

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Causes of Change

Causes of Change. Order and Spontaneity . Enthalpy and Reactions. Some reactions happen easily, but some others do not. Sodium and chlorine readily react to form NaCl when brought together.

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The balanced chemical equation provides information about the beginning and end of reaction. The reaction mechanism give

Reaction Mechanisms. The balanced chemical equation provides information about the beginning and end of reaction. The reaction mechanism gives the path of the reaction. Mechanisms provide a very detailed picture of which bonds are broken and formed during the course of a reaction.

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2.0 0.5 0.20 5.0 0.012

For the reaction 2A + B {image} C + 2D at 35°C, the value of kf is 3.0 x 10-3 M-2•s-1 and the value of kr = 1.5 x 10-2 M-2•s-1. Calculate the value of Kc for this reaction. 2.0 0.5 0.20 5.0 0.012.

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Chemical Equations

Chemical Equations. These interactions are called chemical reactions . A substance that undergoes a chemical reaction is called a reactant . A substance that is formed in a chemical reaction is called a product .

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Equilibrium Constant

Equilibrium Constant. Example. H 2 + F 2 ? 2HF

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Combustion

Combustion. ____________________ ____________________ ____________________. Hydrocarbon Combustion. Hydrocarbons are molecular (covalent) compounds made ____________________ ____________________ Many are used as fuels; _______________ ________________________________

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Limiting Reagent Problems

Limiting Reagent Problems. I 2 O 5 (g) + 5 CO(g) ----> 5 CO 2 (g) + I 2 (g) 1. According to the reaction above, if 80.0 grams of iodine(V) oxide, I 2 O 5 , reacts with 28.0 grams of carbon monoxide, CO. Determine the mass of iodine I 2 , which could be produced?. Limiting Reagent Problems.

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