Chemical kinetics describes the rates of chemical reactions. The three factors that affect reaction rates are concentration of reactants, temperature, and presence of a catalyst. An instantaneous rate is the rate of reaction at a specific moment in time. Beer's law relates the absorption of light to the concentration of an absorbing substance in a solution. First and second order reactions have rates dependent on the first or second power of the concentration of a reactant. Half-life is the time required for half of the reactants to be converted to products at a given reaction rate. Activation energy is the minimum energy that reactant molecules must possess for a reaction to occur.

1. GENERAL CHEMISTRY-II (1412)
S.I. # 12
1. Define chemical kinetics:
2. What three factors affect chemical reactions?
1.________________________
2.________________________
3.________________________
3. Define instantaneous rate:
4. What is Beer’s Law?
5. What is the 1st order of reaction?
6. What is the 2nd order of reaction?
7. What is half-life?
8. What is activation energy?

2. 9. What is the Arrhenius Equation?
10. What is an intermediate step?
11. What is a rate determining step?
12. What is the difference between homogeneous catalysts and heterogeneous
catalysts?
13. A reaction obeys the following rate law: Rate = k[B]2
A+B C
a) if [A] is doubled, how will the rate change? Explain
b) what are reaction orders for A and B? What is the overall reaction order?
c) what are the units of k for this reaction?
14. The gas phase decomposition of SO2Cl2, SO2Cl2  SO2 (g) + Cl2 (g) is 1st
order in SO2Cl2. At 600K the half life for this process is 2.3x105s. A. What is the
rate constant at this temperature? B. Calculate the half life if the rate constant is
2.2x10-5s-1 at 320°C.