Chapter 14 Flashcards
Chemical kinetics
Study of reaction rate
Reaction rate
Speed at which reactions take place
Mechanism
Step by step view of the change of reactants to product
Rate
Change in concentration over time
Instantaneous rate
Slope at curve at one point
Initial rate
Instantaneous rate at time 0
How is reaction rate measured
Using concentration change for a reactant or a product over time
Reaction order
The exponent of the rate with respect to each reactant
How to find overall reaction order
Add individual reaction order
What is k in rate law
The rate constant dependent on temperature
First order reactions
Rate that depends only on reactant to the 1st power
T or F : reactions with k>=10^9 are fast
True
Activation energy
Minimum energy needed fir a reaction to occur
Transition state
Organization of atoms at its highest energy state
Unimolecularity elementary reaction and rate law
A -> products / Rate= k[A]
Bimolecularity elementary reaction and rate law
A+A➡️products / Rate= k[A]^2
A+B➡️products / Rate= k[A][B]
Termolecularity elementary reaction and rate law
A+A+A➡️products / Rate=k[A]^3
A+A+B➡️products / Rate= k[A]^2[B]
A+B+C➡️products / Rate= k[A][B][C]
Rate determining step
The slowest step in a reaction
What does catalyst do
Increase the rate of reaction by decreasing activation energy
Homogenous catalyst
Reactant and catalysts are in the same phase
Heterogenous catalysts
Catalyst is in a different phase than the reactants
