Given the following data for the reaction A $\rightarrow$ B, determine the activation energy, E_a, of the reaction. k (M/s)
T (K)
2) 04 * 10^-⁴
250
6) 78* 10^-³
400

Question

Given the following data for the reaction A $\rightarrow$ B, determine the activation energy, E_a, of the reaction. k (M/s) T (K) 2)04 * 10^-⁴ 250 6)78* 10^-³ 400

Quizplus · Accepted Answer

The activation energy (Ea) can be calculated using the Arrhenius equation:k = Ae^(-Ea/RT)where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant (8.314 J/mol*K), and T is the temperature in Kelvin.Taking the natural logarithm of both sides of the equation, we get:ln(k) = ln(A) - (Ea/RT)Plotting ln(k) versus 1/T should give a straight line with a slope of -Ea/R.Using the data given, we can calculate ln(k) and 1/T:ln(k)    1/T-4.605   0.004-2.708   0.0025Plotting these values gives a straight line with a slope of -2.34 kJ/mol. Therefore, the activation energy is 2.34 kJ/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