Rate Determination and Activation Energy

LABORATORY REPORT
Experiment 6 Rate Determination and Activation Energy
Name: ____________________________________________ Date: ___________________
Lab Partner’s Name: _________________________________ Score: _________________
I. Introduction
II. Results Analysis
A. Data
B. Discussion
III. Conclusion
References (APA Style)
ATTACHMENT 1
DATA AND CALCULATIONS
Trial Temperature
(°C)
Rate constant, k
(s–1)
1
2
3
4
Slope, m: ________________________________________________
Activation Energy, Ea (kJ/mol) : ______________________________
CALCULATIONS:
DATA ANALYSIS
1. Plot a graph of your data above, using temperature (°C) as the x-axis, and the rate constant,
k, as the y-axis. Describe the relationship between rate constant (k) and temperature.
2. Determine the activation energy, Ea, by plotting the natural log of k (ln k) vs. the reciprocal
of absolute temperature (1/T). Absolute temperature (T) = o
C + 273) Describe the
relationship between ln k vs. 1/Temperature.
3. Calculate the activation energy, Ea, for the reaction. To do this, first calculate the best fit line
equation for the data in Step 2. Use the slope, m, of the linear fit to calculate the activation
energy, Ea, in units of kJ/mol. Note: On a plot of ln k vs. 1/absolute temperature, Ea = m × R.
4. A well-known approximation in chemistry states that the rate of a reaction often doubles
for every 10°C increase in temperature. Use your data to test this rule. (Note: It is not
necessarily equal to 2.00; this is just an approximate value, and depends on the activation
energy for the reaction.)