Lecture 8 - Chemical Kinetic Flashcards
What happens when the concentration of reactants increase
The reactant molecules will collide
What happens when the tempeture increases
Molecules go faster and collide more often
Greater energy
What is a catalyst
Speed up reactions by changing the mechanism of reaction
Increase the rate of reaction by decreasing activation energy
What are the two types of catalysts
Homogeneous -mine is present in the same phase as the reacting molecules
Heterogenous - exists in the different phase from the reacting molecules
What is the collision model
Bonds are broken and new ones are formed
Molecules only react. If they collide with each other and need enough energy for bonds to break
What is activation energy
Minimum amount of energy required for reaction
What is the Arrhenius equation
K - rate constant
A- frequency factor
e-mathematical quantity
T-kelvin temperature
R - gas constant (8.314 j/mol)
E - activation energy
What affects rate of reaction
Temperature
Surface area
Concentration
Etc
Another way of doing Arrhenius equation
In k = ln A - E power of a/ RT
What is the equation for rate of reaction
Ra = change in conc of species / change in time
What is reaction order
Relationship between the concentrations of species and the rate of reaction
