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DATA AND CALCULATIONS Rate constant, k (54) Trial Temperature (*C) 1 25 0.005144 20 0.004020 3 15 0.003562 4 10 0.003255 DATA ANALYSIS 1. Determine the activation energy, Ea, by plotting the natural log of k (In k) vs. the reciprocal of absolute temperature (1/T). Note: Absolute temperature, T= °C + 273. a. Choose New Calculated Column from the Data menu. b. Create a column, In rate constant, k. c. Create a second column, reciprocal of absolute temperature, 1/(Temperature (°C) + 273). d. On the displayed graph, plot In rate constants (In k) on the y-axis and the reciprocal of absolute temperature (1/T) on the x-axis by clicking on the respective axes labels. Autoscale the graph if necessary. Note: Attach this graph you created in your lab report as Figure 6 (title the graph properly). Describe the relationship between In k vs. 1/T. 2. Calculate the activation energy, Eo, for the reaction. To do this, first calculate the best fit line equation (linear fit) for the data in Step 2. Record the slope, m, of the linear fit below and use it to calculate the activation energy, Eo, in units of kJ/mol. Note: On a plot of In k vs. 1/T, Eg = m x R. 3. 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.) CALCULATIONS: Slope, m : Activation Energy, Ea (kJ/mol) :,

DATA AND CALCULATIONS Rate constant, k (54) Trial Temperature (*C) 1 25 0.005144 20 0.004020 3 15 0.003562 4 10 0.003255 DATA ANALYSIS 1. Determine the activation energy, Ea, by plotting the natural log of k (In k) vs. the reciprocal of absolute temperature (1/T). Note: Absolute temperature, T= °C + 273. a. Choose New Calculated Column from the Data menu. b. Create a column, In rate constant, k. c. Create a second column, reciprocal of absolute temperature, 1/(Temperature (°C) + 273). d. On the displayed graph, plot In rate constants (In k) on the y-axis and the reciprocal of absolute temperature (1/T) on the x-axis by clicking on the respective axes labels. Autoscale the graph if necessary. Note: Attach this graph you created in your lab report as Figure 6 (title the graph properly). Describe the relationship between In k vs. 1/T. 2. Calculate the activation energy, Eo, for the reaction. To do this, first calculate the best fit line equation (linear fit) for the data in Step 2. Record the slope, m, of the linear fit below and use it to calculate the activation energy, Eo, in units of kJ/mol. Note: On a plot of In k vs. 1/T, Eg = m x R. 3. 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.) CALCULATIONS: Slope, m : Activation Energy, Ea (kJ/mol) :,

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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DATA AND CALCULATIONS Rate constant, k (s-4) Trial Temperature (°C) 1 25 0.005144 20 0.004020 15 0.003562 4 10 0.003255 DATA ANALYSIS 1. Determine the activation energy, Ea, by plotting the natural log of k (In k) vs. the reciprocal of absolute temperature (1/T). Note: Absolute temperature, T= °C + 273. a. Choose New Calculated Column from the Data menu. b. Create a column, In rate constant, k. c. Create a second column, reciprocal of absolute temperature, 1/(Temperature (°C) + 273). d. On the displayed graph, plot In rate constants (In k) on the y-axis and the reciprocal of absolute temperature (1/T) on the x-axis by clicking on the respective axes labels. Autoscale the graph if necessary. Note: Attach this graph you created in your lab report as Figure 6 (title the graph properly). Describe the relationship between In k vs. 1/T. 2. Calculate the activation energy, Eo, for the reaction. To do this, first calculate the best fit line equation (linear fit) for the data in Step 2. Record the slope, m, of the linear fit below and use it to calculate the activation energy, Eo, in units of kJ/mol. Note: On a plot of In k vs. 1/T, Ea = m x R. 3. 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.) CALCULATIONS: Slope, m : Activation Energy, Ea (kJ/mol) : 8
Transcribed Image Text:DATA AND CALCULATIONS Rate constant, k (s-4) Trial Temperature (°C) 1 25 0.005144 20 0.004020 15 0.003562 4 10 0.003255 DATA ANALYSIS 1. Determine the activation energy, Ea, by plotting the natural log of k (In k) vs. the reciprocal of absolute temperature (1/T). Note: Absolute temperature, T= °C + 273. a. Choose New Calculated Column from the Data menu. b. Create a column, In rate constant, k. c. Create a second column, reciprocal of absolute temperature, 1/(Temperature (°C) + 273). d. On the displayed graph, plot In rate constants (In k) on the y-axis and the reciprocal of absolute temperature (1/T) on the x-axis by clicking on the respective axes labels. Autoscale the graph if necessary. Note: Attach this graph you created in your lab report as Figure 6 (title the graph properly). Describe the relationship between In k vs. 1/T. 2. Calculate the activation energy, Eo, for the reaction. To do this, first calculate the best fit line equation (linear fit) for the data in Step 2. Record the slope, m, of the linear fit below and use it to calculate the activation energy, Eo, in units of kJ/mol. Note: On a plot of In k vs. 1/T, Ea = m x R. 3. 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.) CALCULATIONS: Slope, m : Activation Energy, Ea (kJ/mol) : 8
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