Chapter 10 - Reaction Rates and Equilibrium Flashcards
Reaction rates, Catalysts, Boltzmann distribution, Dynamic equilibrium and le Chatelier's principle, and The equilibrium constant.
What is reaction rate?
The change in concentration of a reactant or product in a given time.
What makes an effective collision?
Particles must have sufficient energy
Particles must collide in correct orientation
Which factors can change the rate of a chemical reaction?
Concentration
Temperature
Use of a catalyst
Surface area of solid reactants
What effect does increasing temperature have on reaction rate?
Reaction rate increases with greater temprature
Explain why increasing temperature has its effect on reaction rate
with higher temperature Particles have more energy Higher speed Collide more frequently More successful collisions Rate increases
What is the rule of thumb for reaction rate and temperature?
A 10C increase in temperature doubles the rate.
What effect does increasing concentration/pressure have on reaction rate?
increasing concentration and pressure Reaction rate increases
Explain why increasing concentration/pressure has its effect on reaction rate
Concentration increases More particles per unit volume More frequent collisions More successful collisions Rate increases
How can progress of a chemical reaction be followed?
Monitoring the removal of a reactant.
Following the formation of a product.
What are the two methods of determining reaction rate, when a gas is produced?
Monitoring the volume of gas produced
Monitoring the loss of mass of reactants
What does a catalyst do?
A substance that changes the rate of a chemical reaction by providing an alternative ath with a lower activation energy without undergoing any permanent change itself.
What are the main properties of a catalyst?
Not used up in the reaction.
May react with a reactant to form an intermediate or provide a surface for the reaction to take place.
The catalyst is regenerated at the end of the reaction.
What is a homogeneous catalyst?
Has the same physical state as the reactants.
How does a homogeneous catalyst interact with the reactants?
Forms an intermediate
This intermediate breaks down to give the product and regenerates the catalyst
Give two examples of homogeneous catalysts
Sulphuric acid in the production of esters
Chlorine radicals in ozone depletion