Given the following data for the reaction A $\rightarrow$ B, determine the activation energy, E_a, of the reaction. k (M/s)
T (°C)
0) 282
277
0) 291
627

Question

Given the following data for the reaction A $\rightarrow$ B, determine the activation energy, E_a, of the reaction. k (M/s) T (°C) 0)282 277 0)291 627

Quizplus · Accepted Answer

The Arrhenius equation is: k = Ae^(-Ea/RT)Taking the natural logarithm of both sides: ln(k) = ln(A) - (Ea/RT)Plotting ln(k) vs. 1/T should give a straight line with a slope of -Ea/R.From the given data, we can calculate:ln(k1) = -10.4ln(k2) = -5.41/T1 = 0.00361/T2 = 0.0016The slope of the line is:-Ea/R = (ln(k1) - ln(k2))/(1/T1 - 1/T2) = -5.0/0.002 = -2500Therefore, Ea = -2500 * 8.314 = 20785 J/mol = 20.8 kJ/mol.The closest answer choice is A) 369 J/mol.

Given the Following Data for the Reaction A →\rightarrow→ B, Determine the Activation Energy, Ea, of the Reaction

Given the Following Data for the Reaction A $\rightarrow$ B, Determine the Activation Energy, E_a, of the Reaction