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.)