1. 1. Calculate the moles of B (limiting reactant) consumed based on 10
1. Calculate the moles of B (limiting reactant) consumed based on 10.0 mL of M NaHSO3 being consumed in each trial. Put this value in the table.
L x mol = mol
1 L

2. Volume of A
(0.020M KIO3) (mL)
10.0
9.0
7.0
5.0
3.0
Time for Reaction (s)
2.0
Moles of B (NaHSO3)
Consumed
Reaction Rate in (molesNaHSO3/s)
Molarity of Solution A (KIO3) (M)

3. 2. Calculate the reaction rates in (moles NaHSO3/s) for each trial
2. Calculate the reaction rates in (moles NaHSO3/s) for each trial. Put these values in the table.
Rate = mol = mol/s
2.0 s

4. Volume of A
(0.020M KIO3) (mL)
10.0
9.0
7.0
5.0
3.0
Time for Reaction (s)
2.0
Moles of B (NaHSO3)
Consumed
Reaction Rate in (molesNaHSO3/s)
Molarity of Solution A (KIO3) (M)

5. Volume of A
(0.020M KIO3) (mL)
10.0
9.0
7.0
5.0
3.0
Time for Reaction (s)
2.0
2.5
4.0
6.0
Moles of B (NaHSO3)
Consumed
Reaction Rate in (molesNaHSO3/s)
Molarity of Solution A (KIO3) (M)

6. 3. Calculate the molarity (M2) of solution A (KIO3) for each trial using
M1V1 = M2V2 . M1 = 0.020M, V1 is in the table, and V2 = 20.0mL.
Put these values in the table.
M1V1 = M2V2
(0.020)(10.0) = M2(20.0)
M2 = M

7. Volume of A
(0.020M KIO3) (mL)
10.0
9.0
7.0
5.0
3.0
Time for Reaction (s)
2.0
2.5
4.0
6.0
Moles of B (NaHSO3)
Consumed
Reaction Rate in (molesNaHSO3/s)
Molarity of Solution A (KIO3) (M)
0.010

8. Volume of A
(0.020M KIO3) (mL)
10.0
9.0
7.0
5.0
3.0
Time for Reaction (s)
2.0
2.5
4.0
6.0
Moles of B (NaHSO3)
Consumed
Reaction Rate in (molesNaHSO3/s)
Molarity of Solution A (KIO3) (M)
0.010
0.0090
0.0070
0.0050
0.0030

9. Complete the rest of the table.

10. 4. What is the relationship between concentration of reactant and rate?
As the concentration decreases so does the rate.
This is a direct relationship.
5. Explain using the Collision Theory.
As the concentration decreases so does the number of reactant collisions so the rate decreases.