Chapter 4 - Chapter 4 To work with chemical reactions...

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Chapter 4 To work with chemical reactions requires knowing the correct formula of each reactant and products and the relative molar amounts of each involved in the reaction Many of the very large number of known chemical reactions can be assigned to a few categories: Combination, Decomposition, Displacement and Exchange 4.1 Combustion reactions – Reactions in which elements of compound burns in air or oxygen Balanced chemical equation – Indicates the relative amounts of reactants and products required so that the number of atoms of each element in the reactants equals the number of atoms of the same element in the products Aqueous solution – A substance dissolved in water In the 18 th century, the great French scientist Antoine Lavoisier introduced the law of conservation of mass which showed that mass is neither created nor destroyed in chemical reactions Stoichiometry – Relations among the masses of chemical reactants and products Stoichiometric coefficients – The coefficients (the multiplying numbers) in a balanced equation 4.2 Combination reaction – Two or more substance react to form a single product Oxygen and Group 7A elements usually go through combination reactions because they are very reactive Decomposition reaction – One substance decomposes to form two or more products
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This note was uploaded on 09/21/2011 for the course CHE 131 taught by Professor Kerber during the Fall '08 term at SUNY Stony Brook.

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Chapter 4 - Chapter 4 To work with chemical reactions...

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