I need help determining what the activation energy in kJ/mol would be. I have included the tutoring approach to the problem below for additional aid. Thank you in advance!!

Slope =247s1K The rate of the reaction N2O5(g)2NO2(g)+1/2O2(g) The rate constant for a reaction relates to activation energy and temperature by the Arrhenius equation, which can be considered to have the form of a linear equation: lnk=lnAREa(T1)y=b+mxwhere:m=slopeoftheline=REax=T1y=lnk In this case a plot of lnk vs. 1/T will give a staight line with a slope equal to Ea/R. To determine the value of the activation energy, Ea, create the plot, measure the slope using the least squares analysis, and solve for Ea : Ea=slopeRR=8.314JK1mol1