1. April 21, 2010 CHEM 112- General Chemistry 2
Exam #3 Review
April 21, 2010
CHEM 112- General Chemistry 2

2. Osmotic Pressure =cRT
= osmotic pressure in atm
c= concentration in mol/L
R= Latm/Kmol
T= temperature in Kelvin
An aqueous solution containing 1.0g of bovine insulin per liter has an osmotic pressure of 3.2mmHg at 25°C. Calculate the molar mass of bovine insulin.

3. Determining Rate Law- Initial Rate Method
Reaction: CO(g) + NO2(g) → CO2(g) + NO(g)
Determine the rate law, including the value of the rate constant.
Experiment
[CO], mol/L
[NO2], mol/L
Initial Rate 1
5.10 x 10 -4
0.350 x 10 -4
3.4 x 10-8 2
0.700 x 10 -4
6.8 x 10-8 3
0.175 x 10 -4
1.7 x 10-8 4
1.02 x 10 -3 5
1.53 x 10 -3
10.2 x 10-8

4. Summary of rate laws and graphical method
Reaction Order
Integrated Rate Law
Characteristic Kinetic Plot
Slope of Kinetic Plot
Units of Rate Constant
Zero
[R]0 - [R]t = kt
[R] vs. t -k
mole L-1 sec-1
First
[R]t = [R]0e-kt
ln([R]t/[R]0)= -kt
ln[R] vs. t
sec-1
Second
1/[R]t – 1/ [R]0 = kt
1/[R] vs. t k
L mole -1 sec-1

5. Determining rate law- graphical method

6. Determine the half-life equation for a zero order process
First order
Zero order
[R]0 - [R]t = kt

7. Determining remaining amount given half-life data

8. The Arrhenius equation is used to determine the activation energy (Ea) from experimental data
Graphical Form
Two point form

9. The rate law for an elementary step is given by the equation for that step
Molecularity
Rate Equation
A → product
Unimolecular
Rate= k[A]
A + B → product
Biomolecular
Rate= k[A][B]
A + A → product
Bimolecular
Rate= k[A]2
2A + B → product
Termolecular
Rate= k[A]2[B]

10. Elementary steps- determining rate equation and molecularity

11. Writing and evaluating Equilibrium expressions