Chemical Kinetics (5/8) Flashcards
Chemical Kinetics graph
end of the line is below the start= products are favored and spontaneous (-G)
Arrhenius equation
K=Ae^(-E_a/RT)
Enzyme
Biological catalysts reduce the activation energy of a reaction
- stabilizes
- weakens bonds
- increases collisions
- donates electron density
- DOES NOT change enthalpy or ∆G (cannot make a reaction spontaneous)
heterogeneous and homogeneous
Heterogeneous= different phase than reactants Homogeneous= Same phase as reactants
For an endothermic reaction
The reactants are lower in energy than the products, the transition state is higher in energy than the products, the reaction has a positive ∆H
Rate law
Math expression for the relationship between [r] and rate of reaction
Rate equation
rate= K[A]^x[B]^y
Units of third order reaction
1/(M^2*s)
Units of second order reactin
1/(M*s)
Units of first order reaction
1/s
Units of 0th order reaction
M/s
Solving for activation energy
The difference in energy between the reactants and the transition state