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Plot a graph of your data above, using Temperature (°C) as the x-axis, and the rate constant, k, as the y-axis. Determine the activation energy, Ea, by plotting the natural log of k vs. the reciprocal of absolute temperature. 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 In k vs. 1/absolute temperature, Ea= -m × R.

Plot a graph of your data above, using Temperature (°C) as the x-axis, and the rate constant, k, as the y-axis. Determine the activation energy, Ea, by plotting the natural log of k vs. the reciprocal of absolute temperature. 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 In k vs. 1/absolute temperature, Ea= -m × R.

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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Tral tempenative ( | Rate constant 25°€ 0.03 20.7°€ 0.011 0.009 0.007
Transcribed Image Text:Tral tempenative ( | Rate constant 25°€ 0.03 20.7°€ 0.011 0.009 0.007
1. Plot a graph of your data above, using Temperature (°C) as the x-axis, and the rate constant, k, as the y-axis. 2. Determine the activation energy, Ea, by plotting the natural log of k vs. the reciprocal of absolute 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 In 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.) 5. Using the rate constant and precise temperature value for the trial that was done at room temperature (~20°C), as well as the Ea value you obtained in Step 3 above, calculate the value of the rate constant at 40°C.
Transcribed Image Text:1. Plot a graph of your data above, using Temperature (°C) as the x-axis, and the rate constant, k, as the y-axis. 2. Determine the activation energy, Ea, by plotting the natural log of k vs. the reciprocal of absolute 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 In 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.) 5. Using the rate constant and precise temperature value for the trial that was done at room temperature (~20°C), as well as the Ea value you obtained in Step 3 above, calculate the value of the rate constant at 40°C.
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