Need an answer to this chemistry problem. Thank you!

Question

A chemist ran a particular reaction at different temperatures to determine the activation energy of the reaction. The plot of his data displayed the following linear regression. Determine the activation energy of the studied reaction.

y = ax + b

a = -1449

b = 13.788

Answer 1

You neglected to mention what the plot was, or what the x and y axes were. I'll assume it was an Arrhenius plot of ln k vs 1/T according to the linear equation ln k = -Ea/R(1/T) + ln A in the form of y = ax + b.

a = slope = -Ea/R = -1449 where R = 8.314 J/mol-K

-Ea = (8.314)(-1449)

Ea = 12,047 but since you gave no units for the slope or the experiment in general, I can't assign units to this except that it is generally given in joules/mole