6) A particular reaction has the following rate constant at different temperatures: Temperature (°C) k (s¹) Temperature (K) 1/T (K) 6.78 x 10-4 0.134 -52 33 In (k) a. Convert the temperature to kelvin, find 1/T (K), and take the natural log of the rate constant and complete the chart above. b. Plot 1/T (K) in the x-axis and In (k) in the y-axis. This is the linear form of the Arrhenius Equation.
6) A particular reaction has the following rate constant at different temperatures: Temperature (°C) k (s¹) Temperature (K) 1/T (K) 6.78 x 10-4 0.134 -52 33 In (k) a. Convert the temperature to kelvin, find 1/T (K), and take the natural log of the rate constant and complete the chart above. b. Plot 1/T (K) in the x-axis and In (k) in the y-axis. This is the linear form of the Arrhenius Equation.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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We now the Arrhenius equation for activation energy determination.
ln(k2/k1) = Ea/R x (1/T1 - 1/T2)
where,
Ea = the activation energy of the reaction in J/mol
R = the ideal gas constant = 8.3145 J/K·mol
T1 and T2 = absolute temperatures (in Kelvin)
k1 and k2 = the reaction rate constants at T1 and T2
So it is very important equation for activation energy determination
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