Chemistry - Kinetics Flashcards
The branch of chemistry that studies the rate of chemical reactions and the factors that affect them
Kinetics
The speed at which reactants are converted into products
Reaction rate
Basic rate equation
(Delta) Quantity divided by (Delta) time
For a reaction to occur particles must collide with sufficient energy to overcome the activation energy
collision theory
A temporary high energy state during a reaction when bonds are breaking and forming
activated complex
a short lived substance formed during thee reaction but not part of the final products
reaction intermediate
lowers activation energy by providing an alternative pathway with a lower energy barrier, stabilizing the transition state and speeding up the reaction without being consumed
catalyst
the minimum energy required for a reaction to occur
activation energy
A type of reaction where energy is absorbed, the products have a higher energy than the reactants
Endothermic reaction
a type of reaction where energy is released, the products have a lower amount of energy than the reactants
Exothermic reaction
the total heat content of a system
(related to energy changes during a reaction)
Enthalpy
a step-by-step sequence of reactions by which the overall chemical change occurs
reaction mechanism
type of reaction where all the reactant and products are in the same phase (solid, liquid, gas, etc.)
homogeneous reaction
type of reaction where the reactants and products are in different phases
heterogeneous reaction
explain the difference between the activated complex and a reaction intermediate
the activated complex is apart of the final reaction while the reaction intermediate is not
why does increasing temp. speed up a reaction?
it makes the particles move faster resulting in more collisions which then leads to a faster reaction
how does a catalyst lower activation energy
it provides an alternative pathway while stabilizing the transition state resulting in a lower activation energy
