Rates of Reaction Flashcards
Activation Energy
the minimum amount of energy needed for a reaction to happen
Catalyst
speeds up a reaction without being used in the reaction itself, lowers the activation energy, causing a higher proportion of successful collisions
Collision Theory
explains why rate of reaction changes, states that particles must collide before a reaction takes place and if there is a collision, it might take place, but not all collisions lead to reactions because they need energy in order to react, and reactants must have the activation energy in order to react
Cocentration
increasing the particles per unit volume causes more frequent collisions
Mean Rate of Reaction
quantity of reactant used / time or quantity of reactant formed / time
Metabolism
the sum of all the reactions in the body
Pressure
increasing the particles per unit volume causes more frequent collisions