Chemistry: Rate of Reaction Flashcards
What is meant by the rate of reaction?
rate at which a chemical reaction takes place, the change in an amount of reactants and products over time
What is necessary for a reaction to take place?
two particles must collide with enough energy (activation energy) to break bonds
What is collision theory?
states a reaction will not take place unless two particles collide successfully at the right orientation and with at least a certain amount of kinetic energy (activation energy)
What do successful collisions require?
-right orientation -minimum amount of kinetic energy
What is activation energy?
minimum amount of energy to start a reaction, enough to break bonds
What symbol represents activation energy?
Ea
What factors affect the rate of a chemical reaction?
-increasing temperature -increasing solution concentration -increasing gas pressure
-increasing surface area of solid reactants -using a catalyst
How does increasing temperature increase the rate of reaction?
-molecules have more kinetic energy -more likely to have activation energy -increases successful collisions
How does increasing solution concentration increase the rate of reaction?
-more particles in given volume -closer together, increases contact -likelihood of successful collisions higher
How does increasing gas pressure increase the rate of reaction?
-more particles in given volume -closer together, increases contact -increases likelihood of successful collisions
How does increasing surface area of solid reactants increase the rate of reaction?
-more particles available to collide with molecules in gas or liquid -greater likelihood of successful collisions
How does using a catalyst increase rate of reaction?
-a catalyst is a substance that can lower the activation of a chemical reaction without being chemically changed itself -particles more likely to have activation energy -increased likelihood of successful collisions
