Question

Maeve plotted her data from Experiment CLK and obtained the equation y=7,756x-16.8 for her trendline. Using Maeve's equation, what is the activation energy, Eₐ, in kJ/mol for this reaction?

R=8.314 J mol⁻¹ K⁻¹

Answer 1

To find the activation energy, Eₐ, in kJ/mol, we need to determine the value of the slope in the given equation.

Step-by-step explanation:

To determine the activation energy, Eₐ, we need to find the value of the slope, which represents the activation energy in the Arrhenius equation.

From Maeve's equation, y = 7,756x - 16.8, we can see that the slope is 7,756. However, the activation energy needs to be in kJ/mol, so we need to convert it from J/mol to kJ/mol.

Given that R = 8.314 J mol⁻¹ K⁻¹, we use the conversion factor 1 kJ = 1000 J to convert the activation energy to kJ/mol. Therefore, the activation energy, Eₐ, is 7,756 J/mol * (1 kJ/1000 J) = 7.756 kJ/mol.

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