Find the new rate constant at 310K if the rate constant is 7 M-1s-1 at 370K, and the Activation Energy is 900kJ/mol.
(Hint: Use the Arrhenius equation)
1.788X10-24 M-1s-1
The time it takes to reduce the concentration of a reactant to half of its original value.
Rate = k[Cr(H2O)6 3+] [SCN]2
k = 2.00x10-5
The main factors of Collision Theory
What are:
-Activation Energy
-Temperature
-Molecular Orientation
A certain reaction has an activation energy of 54.0 kJ/mol. As the temperature is increased from to a higher temperature, the rate constant increases by a factor of 7.00. Calculate the higher temperature
A substance that is formed in one step and used up in a subsequent step.
What is an intermediate?
Looking at the graph on the sheet of paper in front of you; name what the graph or curve is representing.
Maxwell-Boltzmann curve
Integrated- shows how the concentrations of species in a reaction depend on time.
Write the rate law expected for the mechanism given to you on the sheet of paper. What is the overall balanced equation for the reaction? What are the intermediates in the proposed mechanism?
Rate = k[C4H9Br]
Balanced equation:
C4H9Br + 2H2O → C4H9OH + Br- + H3O+
Intermediates: C4H9+ and C4H9OH2+
On the graph given to you, label the activation energy (reverse and forward), intermediate, and activated complex(s) on the graph given to you.
1.Adsorption and activation of the reactants.
2.Migration of the adsorbed reactants on the surface.
3.Reaction of the adsorbed substances.
4.Escape, or desorption, of the products
0th: [A]=-kt + [A]
1st: ln[A]=-kt + ln[A]
2nd: 1/[A] = kt + 1/[A]