The rate constant for a reaction is measured as a function of time. A plot is created by graphing ln(k) on the y-axis and 1/T on the x-axis, and a best fit line with a slope of -98,535 K is obtained.

Question

Based on this data what is the activation energy of this reaction (in kJ/mol)?

R= 8.314 J/(K mol)



Enter your value with three significant figures.

Answer 1

let the slope be equal to -E_a/R

slope = -Ea_/R

rearrange the equation to solve for E_a

-E_a = slope/R

-E_a = -98,533K/8.314J/K*mol

-E_a = -8.19*10⁵J/mol multiply the whole equation by -1 to get rid of the (-) on E_a

E_a = 8.19*10⁵J/mol divide by 1000 to covert J to kJ

E_a = 819kj/mol