A plot of LNK versus inverse temperature has a slope of -8313. What is the activation energy for this reaction? So remember when they give us a plot, it's always of Y versus X, and the fact that we're dealing with LMK versus inverse temperature means that we're going to deal with the linear form of the Arrhenius equation.
So here we're going to say that lnK=-EA/R∙1T+lnA. And remember this is equal to the formula for straight line, which is Y=MX+B. M represents our slope and it's also equal to negative activation energy divided by R, our gas constant. So them telling us our slope here is them really giving us M? We're going to set them equal to each other here.
This is -8313 Kelvin equals -EA/R. R is our gas constant 8.314 Joules over moles times K. We're going to multiply both sides by 8.314 joules over moles times K. Kelvin's can't slap and we'll have our answer in joules per mole. Now here, initially we're going to have is -69114.282 joules per mole equals -EA.
Just divide both sides by -1 and we'll get EA equals here. This has four sig figs in it. Or answer should have four sig figs as well, so we're going to say 69110 joules per mole as our final answer.