Chemical Kinetics CH5 Flashcards
This theory states that the rate of a reaction is proportional to the number of collisions per second between the reactivity molecules.
Collision Theory of Chemical Kinetics
What is the Arrhenius equation, which is a rate analysis?
k = Ae^(-Ea/RT)
k= rate constant Ae= frequency factor (-Ea) = activation energy R= ideal gas constant T= temp in kelvins
What is the minimum energy collision necessary for a reaction to take place called?
Activation Energy (Ea)
True/False: The transition state has greater energy than the reactants and the products?
True
The difference between the free energy change of the products and the free energy of the reactants?
Free Energy Change of the Reaction
When energy is absorbed (endergonic)?
+G (nonspontaneous)
When energy is given off (exergonic)?
-G (spontaneous)
When molecules collide with energy equal to or greater than the activation energy, they form a certain state in which the old bonds are weakened and the new bonds begin to form.
Transition State Theory
What are the factors that affect reaction rate?
- Reaction Concentrations (proportional increases)
- Temperature (increase unless denature)
- Medium (situational increase; i.e. polar solvents increase, solid, liquid, gas)
- Catalysts (increase)
A catalyst is in the same phase (solid, liquid, gas) as the reactants.
Homogenous Catalysis
The catalyst is in a different phase.
Heterogeneous Catalysis
The rate formation is independent of changes in concentrations of any of the reactants:
rate = k[A]^0[B]^0
Zero-Order Reactions
What does a zero-order graph look like on a concentration vs time graph?
Negative (-) Linear Slope
The rate is directly proportional to only one reactant, such that doubling the concentration of the reactant results in doubling of the rate of formation of the product:
rate=[A]^1 OR rate=[B]^1
First-Order Reactions
Radioactive decay equation (which is a first-order reaction)?
[A]t = [A]oe^-kt
