Chapter 13
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Kinetic energy | the energy available because of the motion of the object
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| thermodynamics | the scientific study of interconversion of heat and other forms of energy
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| reaction rate | is the change in the concentration of a reactant or a product with time (M/s).
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| Rate= | Δ[A]/Δ t or -Δ[A]/Δt
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| rate constant | a constant of proportionality between the reaction rate and the concentration of reaction (k)
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| instantaneous rate | rate for specific instance in time
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| 4 factors affecting rates of reaction | 1. reactant concentration 2. temperature 3. catalysts 4. surface area
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| what is the rate of reaction proportional to? | concentration of reactants
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| overall reaction order | the sum of the powers to which all reaction concentrations appearing in the rate law are raised. x + y
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| rate law | expressed the relationship of the rate of a reaction to the rate constant and the concentrations of the reactants raised to some powers. RATE = k[A]x[B]y
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| rate laws are: | 1. rate laws are always determined experimentally 2. reaction order is always defined in terms of reactant(not product) concentrations 3. the order of the reaction is not related to the stoichiometric coefficient of the reaction in the balanced equation
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| first-order reaction | a reaction whose rate depends on the reactant concentration raised to the first power. k=rate/[A]
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| half-life of a first order reaction | the time required for the concentration of a reaction to decrease to half of its initial concentration, independent of the initial concentration of the reactant
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| second-order reaction | a reaction whose rate depends on the concentration of one reactant raised to the second power or on the concentration of two different reactants, each raised to the first power. Inversely proportional to the initial reactant concentration
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| activated complex | a temporary species formed by the reactant molecules as a result of the collision before they form the product
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| the activation energy (Ea) | is the minimum amount of energy required to initiate a chemical reaction
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| reaction mechanism | the sequence of elementary steps that lead to the product formation
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| intermediates | are not species that appear in a reaction mechanism but not the overall balanced equation, they are always formed and consumed during the reaction
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| molecularity of a reaction | is the number of molecules reacting in an elementary step
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| unimolecular reaction | elementary step with one molecule
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| bimolecular reaction | elementary step with 2 molecules
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| termolecular reaction | elementary step with 3 molecules
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| rate-determining step | the slowest step in the sequence of steps leading to the product formation
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| heterogeneous catalyst | the reactants and the catalysts are in different phases
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| homogeneous catalyst | the reactant and the catalysts are dispersed in a singe phase, usually liquid
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| average rate | change in the concentration of A/length of time interval
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| first-order reaction equation | Ln [A]t/[A]0=-kt
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| half-life of first order reaction equation | t1/2=o,693/k
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| second-order reaction equation | rate= -Δ[A]/Δt +kt
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| half-life equation of a second order reaction | t1/2= 1/k[A]o
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| zero-order reaction | one in which the rate does not depend on the concentration of reactants
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