A study was made to determine the activation energy
EA for a chemical reaction. The rate constant k was determined as a function of temperature T, and the data in the table below obtained.
T, K | k, s21 |
599 | 0.0005 |
629 | 0.0025 |
647 | 0.0052 |
666 | 0.014 |
683 | 0.025 |
700 | 0.064 |
The data should fit a linear model of the form log k = log A ֊ EaJ(2.303RT), where A is the preexponential factor, and R is the gas constant.
(a) Fit the data to a straight line of the form log k = a ֊ 1000b/T. *(b) Find the slope, intercept, and standard error of the estimate.
*(c) Noting that EA = ֊b × 2.303R × 1000, find the activation energy and its standard deviation (Use R = 1.987 cal mol 21 K"1). *
(d) A theoretical prediction gave Ea = 41.00 kcal mol 1K 1. Test the null hypothesis that Ea is this value at the 95% confidence level.
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