21295607-Reaction-Rates

21295607-Reaction-Rates - REACTION RATES The reaction rate...

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REACTION RATES The reaction rate or rate of reaction for a reactant or product in a particular reaction is intuitively defined as how fast a reaction takes place. For example, the oxidation of iron (iron rusting) under the atmosphere is a slow reaction which can take many years, but the combustion of butane in a fire is a reaction that takes place in fractions of a second that is a fast reaction rate. Iron rusting – slow reaction rate Wood burning – fast reaction rate Consider a typical chemical reaction: aA + bB → pP + qQ The lowercase letters (a, b, p, and q) represent stoichiometric coefficients, while the capital letters represent the reactants (A and B) and the products (P and Q).
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Rate of a reaction is always positive. '-' sign is present in the reactant involving terms because the reactant concentration is decreasing. Factors that affect the rate of reaction: Concentration: Reaction rate increases with concentration, as described by the rate law and explained by collision theory. As reactant concentration increases, the frequency of collision
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This note was uploaded on 12/04/2009 for the course CHEM 120 taught by Professor Johnmichael during the Spring '09 term at Tennessee Martin.

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21295607-Reaction-Rates - REACTION RATES The reaction rate...

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