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24 Cards in this Set
- Front
- Back
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[X]
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concentration of substance X
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molarity
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moles of solute per liters of solution
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chemical kinetics
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area of chemistry that studies the rates at which reactions occur
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average reaction rate
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(M/sec) the change in the concentration of the products or reactants per time lapsed
change in concentration is negative for reactants and posiive for products (if for reactants take the opposite in the formula) change in time is always positive the answer is always positive |
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average reaction rate formula
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change in concentration/change in time = (final concentration - initial concentration)/ (final time - initial time)
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collision theory
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in order for an atom or particle to react it must collide with another particle
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effective collision
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a collision that leads to the formation of products
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ineffective collision
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collisions that do not form products
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factors for effective collisions
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1. orientation of particles
2. energy of colliding particles |
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activation energy
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(E subscript a) energy needed to react for effective collisions/ the difference between the energy of the activated complex and the reactants
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activated complex
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the transition state structure/ state at which the energy level is the greatest (very unstable)
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transition state
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temporary state in which reactant bonds are breaking and product bonds are forming (reasembles the reactants and products)
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reaction rate factors
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nature of reactants, temperature, concentration, surface area, catalyst
NCCTS |
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nature of reactants
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increasing the number and complexity of bonds lowers the reaction rate
physical state= gases react more rapidly because they are moving faster so they collide more |
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temperature
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higher temperatures increase the reaction rate by increasing the number of collisions
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concentration
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increasing the concentration increases the reaction rate
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surface area
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increasing the surface area increases the reaction rate
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catalyst
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lowers the activation energy and increases the rate of reaction without being used up
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inhibitors
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they raise the activation energy and slow down the rate of a reaction (preservatives, etc.)
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reaction rate law
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an equation that relates the reaction rate to the concentration of substances
rate= k [A]superscript x [B] superscript y (concentrations raised to some power) |
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reaction mechanism
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a series of steps that leads from reactants to products
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elementary step
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an individual step of a reaction mechanism
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intermediate products
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products produced in one step of a reaction that serve as reactants in later steps
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rate determining step
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the slowest elementary step of the reaction mechanism
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