Factors Affecting Reaction Rates
Objective:
To determine the affect that concentration, nature of reactants, temperature and the use of a catalyst can have on reaction rates.
Materials:
See each part of procedure in lab text pg.1
Procedure:
As in lab text pg.1
Data and Observations:
Table 1: Concentration
[HCl] | Volume H2 produced (mL) | Time (s) | Rate (mL H2/s) |
2.0 | 54.8 | 91 | 0.60 |
3.0 | 49.8 | 35 | 1.4 |
6.0 | 51.4 | 15 | 3.4 |
Table 2: Nature of Reactants
Metal | Mass Loss(g) | Time (s) | Rate (g/s) |
Mg | 0.12 | 36 | 0.0033 |
Zn | 0.11 | 719 | 0.00015 |
Table 3: Temperature
Temperature of HCl | Mass of Alkaseltzer(g) | Time (s) | Rate (g/s) |
Hot | 3.25 | 69.67 | 0.0466 |
Warm | 3.23 | 59.92 | 0.0539 |
Cold | 3.24 | 53.07 | 0.0611 |
Table 4: Catalyst
Reaction | Before | During | After |
H2O2 solution | Transparent and nothing happened. | Transparent and nothing happened. | Transparent and nothing happened. |
H2O2 solution with MnO2 | Transparent and nothing happened. | It began to bubble with increased temperature and get darker. | It turned to black and opaque. |
Sample calculations:
Part1: For [HCl]2.0
[pic 1]
Part2: For Metal Mg
[pic 2]
Part3: For cold temperature
[pic 3]
Questions:
1. Concentration:
a) The reaction rate increases as the concentration of the reaction increases, same as lab result. Because particles have to collide to react successfully, so an increase in concentration of produces makes more collisions. Therefore The chances of an effective collision goes up with the increase in concentration.
b)
0.60mLH2 | 1 mol H2 | 1 mol Mg | 24.3g Mg | 91s |
1s | 22400mL H2 | 1 mol H2 | 1 mol Mg |
=0.059g Mg
So, 0.059g of Mg was used.
2. Nature of Reactants:
a) The independent variable in the reaction was the type of metal used.