Question

2. Calculate the molar concentration of FeCl3 and KI for each reaction and record the values in the table. Provide one example to show you how you compleated the calculation.

a. Each trial will have atotal reaction volume of 40.0 mL. Using diagrams show how each reaction will be different.

b. Using your drawings predict (relative to one another) what you expect to be the fastest and slowest reaction. Explain.

3. Suppose that the reaction X+Y-->Z has the rate law of rate= k[X][Y].

a. What is the overall order of the reaction?

b. What is the order with respect to X? To Y?

c. In a reaction, a student ixed 0.1 M X with 0.0001 M Y and found the rate law to be rate = Ks[Y]. How are K and Ks related? Explain.

TABLE:

Trial FeCl3(mL) KI (mL) H2O (mL)

1 20.0 20.0 0.0

2 20.0 10.0 10.0

3 10.0 20.0 10.0

4 15.0 10.0 15.0

5 10.0 15.0 15.0

Concentration of FeCl3= 0.020 M

Concentration of KI= 0.020 M

Concentration of HCl= 0.10 M