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Identifying Rates of Reactions with Different Factors

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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

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