Identifying Rates of Reactions with Different Factors
Identifying Rates of Reactions with Different Factors
Objective:
To test what factors can significantly affect the efficiency of a reaction.
Reactions for the lab:
(part 1/2) = Mg + 2HCl → MgCl2 + H2
(part 3) = CaCO3 + 2HCl → CaCl2 + H2O + CO2
(part 4) = 10FeSO4 + 2KMnO4 + 8H2SO4 → 5Fe2(SO4)3 + 2MnSO4 + K2SO4 + 8H2O
2KMnO4 + 5Na2C2O4 + 8H2SO4 → K2SO4 + 2MnSO4 + 5Na2SO4 + 8H2O + 10C02
(part 5) = the sodium oxalate reaction plus MnSO4
Observations:
Part 1 = Different levels of concentration in molarity
Concentration of HCl
Reaction Time(s)
Reaction Rate (g Mg/s)
0.5M
514.2
2.917*10^-5
1.0M
120.97
1.24*10^-4
3.0M
24.32
0.000617
6.0M
21.87
0.000686
Part 2 = Different temperatures of solution
Temperature
Reaction Time(s)
Reaction Rate (g Mg/s)
100C
18.67
8.034*10^-4
50C
25.43
5.898*10^-4
20C
36.21
4.1425*10^-4
Part 3 = Difference in surface area
Reactant
Mass CaCO3 (g)
Reaction Time(s)
Reaction Rate (g CaCO3/s)
Powdered CaCO3
0.30
12.91
0.023
Solid CaCO3
0.49
600.00
0.00081
Part 4 = Natural Behaviour of reactants
Reactants
Reaction Time(s)
Reaction Rate (s-1)
FeSO4 + KMnO4 + H2SO4
instantaneous
N/A
Na2C2O4 +KMnO4 + H2SO4
slowly
N/A
Part 5 = Catalysed and uncatalysed
Reaction Time(s)
Reaction Rate (s-1)
With Mn+2 catalyst
instantaneous
N/A
Without Mn+2 catalyst
slowly
N/A
Analysis:
Part 1
Our first experiment was to compare different concentrations of hydrochloric acid and determine the rate of reaction. We dropped four pieces of magnesium which weighed 0.015 grams each into four different flasks which contained the same solution. The only difference was the molarity in each solution. The first flask had 0.5M, the second had 1.0M, the third had 3.0M and the fourth had 6.0M. Our reaction rates were 2.917*10^-5g/s, 1.24*10^-4g/s , 0.000617g/s, 0.000686g/s from first flask to fourth. From these results, we can obviously see the higher the concentration, the faster the rate of reaction. An example proving this is the first flask compared to the fourth. The first flask had a rate of 2.917*10^-5g/s whereas the fourth had a rate of 0.000686g/s. The fourth flask has a significantly faster rate of reaction due to the higher concentration of molecules