Chapter 5- Chemical Kinetics

Question 1

Collision theory of chemical kinetics and reaction rate

Answer 1

Rate of a reaction is proportional to the number of collisions per second between the reacting molecules

Rate= Zf 
Z = total number of collisions per second
f = fraction of collisions that are effective

Question 2

Arrhenius equation about collision of molecules

Answer 2

Rate= Ae^(-Ea/RT)
A= frequency factor 
R= ideal gas constant
T= temp in kelvin

Question 3

+ Gibbs free energy

Answer 3

Endergonic, energy absorbed, nonspontaneous

Question 4

• Gibbs free energy

Answer 4

Exergonic, energy given off, spontaneous

Question 5

Temp for enzymes in human body

Answer 5

Between 35 and 40 Celsius (body temp)

Question 6

Rate law

Answer 6

Rate = k[A]^x[B]^y

Only reactants and k, x, and y must be found experimentally for a certain reaction at a certain temperature

Question 7

Zero order reaction

Answer 7

rate of product formation is independent of changes in concentrations

Can change with temp b/c k is dependent on temperature

Linear graph slope, -k

Question 8

Higher order reactions

Mixed order reactions

Answer 8

Higher- 3rd order rates

Mixed- noninteger orders (fractions). Reaction appears to be first order then when the reactant is low it kicks in and speeds up again

Question 9

First order reactions

Answer 9

Directly proportional to one reactant

[A]e^-kt

Nonlinear graph

Question 10

Second order reactions

Answer 10

Proportional to either concentrations of two reactants or to the square of the concentration of a single reactant

Nonlinear curved graph.