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Mixture 1: Initial Concentrations Mixture 1 22 Table 1: Reaction data for Mixture 1 Temp (C) Temp (K) 10 283.15 295.15 40 [acetone]initial [H+Jinitial 0.2M 0.8M 10 °C 313.15 Table 2: Calculated Values for the Arrhenius Plot Temperature (C) Ea = k Time(sec) 208 kJ/mol [12]initial 0.0005M 93 28 Fill in the next table by calculating the rate constant at each temperature using the rate from the table above, initial concentrations for Mixture 1 and this rate law: k[m]^1 [H+]^1 [l2]^0 rate=[12]initial/(ave time) In k (y-axis) (two decimal points) 1.66x10^-6 Rate= [12]initial/(time) 2.40x10^-5 5.37x10^-5 1.78x10^-6 22 °C 40 °C Construct an Arrhenius plot by graphing in k vs. 1/T. Find the slope for the best fitting (straight) line through the points. Write a Trend line equation. Slope= Trendline Equation=_ 1/T (x-axis) (Kelvin^-1) From the above equation, we can see that slope = -Ea / R where R= 8.314 x 10^-3 K^s/mol K. Use this relationship to calculate the value of Ea:

Mixture 1: Initial Concentrations Mixture 1 22 Table 1: Reaction data for Mixture 1 Temp (C) Temp (K) 10 283.15 295.15 40 [acetone]initial [H+Jinitial 0.2M 0.8M 10 °C 313.15 Table 2: Calculated Values for the Arrhenius Plot Temperature (C) Ea = k Time(sec) 208 kJ/mol [12]initial 0.0005M 93 28 Fill in the next table by calculating the rate constant at each temperature using the rate from the table above, initial concentrations for Mixture 1 and this rate law: k[m]^1 [H+]^1 [l2]^0 rate=[12]initial/(ave time) In k (y-axis) (two decimal points) 1.66x10^-6 Rate= [12]initial/(time) 2.40x10^-5 5.37x10^-5 1.78x10^-6 22 °C 40 °C Construct an Arrhenius plot by graphing in k vs. 1/T. Find the slope for the best fitting (straight) line through the points. Write a Trend line equation. Slope= Trendline Equation=_ 1/T (x-axis) (Kelvin^-1) From the above equation, we can see that slope = -Ea / R where R= 8.314 x 10^-3 K^s/mol K. Use this relationship to calculate the value of Ea:

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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Energy of Activation Determination using the information given below

Mixture 1: Initial Concentrations Mixture [acetone]initial 1 Table 1: Reaction data for Mixture 1 Temp (C) Temp (K) 10 283.15 295.15 313.15 22 40 0.8M 10 °C Table 2: Calculated Values for the Arrhenius Plot Temperature (C) 22 °C [H+]initial 0.2M Ea = k kJ/mol Time(sec) 208 [12]initial 0.0005M 93 28 Fill in the next table by calculating the rate constant at each erature using the rate from the table above, initial concentrations for Mixture 1 and this rate law: k[m]^1 [H+]^1 [12]^0 rate=[12]initial/(ave time) In k (y-axis) (two decimal points) 1.66x10^-6 Rate= [12]initial/(time) 2.40x10^-5 5.37x10^-5 1.78x10^-6 40 °C Construct an Arrhenius plot by graphing in k vs. 1/T. Find the slope for the best fitting (straight) line through the points. Write a Trend line equation. Slope= Trendline Equation=_ 1/T (x-axis) (Kelvin^-1) From the above equation, we can see that slope = -Ea / R where R= 8.314 x 10^-3 K^s/mol K. Use this relationship to calculate the value of Ea:
Transcribed Image Text:Mixture 1: Initial Concentrations Mixture [acetone]initial 1 Table 1: Reaction data for Mixture 1 Temp (C) Temp (K) 10 283.15 295.15 313.15 22 40 0.8M 10 °C Table 2: Calculated Values for the Arrhenius Plot Temperature (C) 22 °C [H+]initial 0.2M Ea = k kJ/mol Time(sec) 208 [12]initial 0.0005M 93 28 Fill in the next table by calculating the rate constant at each erature using the rate from the table above, initial concentrations for Mixture 1 and this rate law: k[m]^1 [H+]^1 [12]^0 rate=[12]initial/(ave time) In k (y-axis) (two decimal points) 1.66x10^-6 Rate= [12]initial/(time) 2.40x10^-5 5.37x10^-5 1.78x10^-6 40 °C Construct an Arrhenius plot by graphing in k vs. 1/T. Find the slope for the best fitting (straight) line through the points. Write a Trend line equation. Slope= Trendline Equation=_ 1/T (x-axis) (Kelvin^-1) From the above equation, we can see that slope = -Ea / R where R= 8.314 x 10^-3 K^s/mol K. Use this relationship to calculate the value of Ea:
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