Results:
Slope 1
2
3
4
0.25516 kPa
0.09496 kPa
0.010285 kPa
.69419 kPa
20.9 C
20.9
20.9
34.2 C
The following mechanism has been proposed for this reaction:
H2O2 + I- ---> IO-+ H2O (step 1, rate determining)
H2O2 + IO----> I- + H2O + O2 (step 2)
1. Identify any intermediate species and/or catalyst species in this mechanism.
2. What is the exact (not general) rate expression for the catalyzed reaction? Does your data from runs 1 â 3 support the rate expression? Explain.
3. Calculate the rate constant, k, at room temperature (average value) and room temperature + 10 °C. Hint: change your rate units into mol/L·s (using PV = nRT).
4. Determine the activation energy for the catalyzed reaction in kJ/mol using the two-point Arrhenius equation.
5. Do you expect the activation energy of the uncatalyzed reaction to be larger, smaller, or the same as the catalyzed reaction? Explain.
Results:
Slope 1 | 2 | 3 | 4 |
0.25516 kPa | 0.09496 kPa | 0.010285 kPa | .69419 kPa |
20.9 C | 20.9 | 20.9 | 34.2 C |
The following mechanism has been proposed for this reaction:
H2O2 + I- ---> IO-+ H2O (step 1, rate determining)
H2O2 + IO----> I- + H2O + O2 (step 2)
1. Identify any intermediate species and/or catalyst species in this mechanism.
2. What is the exact (not general) rate expression for the catalyzed reaction? Does your data from runs 1 â 3 support the rate expression? Explain.
3. Calculate the rate constant, k, at room temperature (average value) and room temperature + 10 °C. Hint: change your rate units into mol/L·s (using PV = nRT).
4. Determine the activation energy for the catalyzed reaction in kJ/mol using the two-point Arrhenius equation.
5. Do you expect the activation energy of the uncatalyzed reaction to be larger, smaller, or the same as the catalyzed reaction? Explain.