Is there a way to calculate values in the Arrhenius equation without a graphing calculator?

Well, you can do it on Excel, or by hand... You may want to take a look at this 10-minute video I made, which teaches you how to use Excel for Chemistry:

DISCLAIMER: LONG ANSWER! Lots of images.

Let's try an example... consider the following reaction.

https://kinetics.nist.gov/kinetics/Detail?id=1989NES/PAY5158-5161:1

https://kinetics.nist.gov/kinetics/Detail?id=1989NES/PAY5158-5161:1

The straight-line version of the Arrhenius equation is:

`overbrace(ln k)^(y) = overbrace(-E_a/R)^(m) overbrace(1/T)^(x) + overbrace(ln A)^(b)`

METHOD 1

Since you know that the activation energy is a constant with respect to a small enough temperature range, this should be a straight line if you plot `ln k` vs. `1//T`.

Once you calculate `ln k` and `1//T` by hand... and it is an exercise you should attempt... you should get:

When doing it by hand, you could pick the first and last data points, as it is a straight line... in doing so, estimate the slope:

`=> "slope" = (Delta(lnk))/(Delta(1//T)) = (-26.7639 - (-27.361))/(0.002681 - 0.004348)`

`~~` `-"358.19 K"^(-1)`

The y-intercept will also be needed, and it is estimated by extrapolating back to `1//T = 0` using the slope:

`-"358.19 K"^(-1) = (ln A - (-27.361))/(0 - 0.004348)`

`=> "y-intercept" = ln A = -25.804`

From here we should compare to the straight-line version of the Arrhenius equation:

`ln k = -E_a/R 1/T + ln A`

The slope then allows us to find the activation energy:

`color(blue)(E_a) = -R cdot "slope"`

`= -8.314 cancel"J""/mol"cdotcancel"K" xx ("1 kJ")/(1000 cancel"J") xx -358.19 cancel("K"^(-1))`

`=` `color(blue)("2.98 kJ/mol")`

The y-intercept allows us to find the frequency factor:

`color(blue)(A) = e^("y-intercept")`

`= e^(-25.800)`

`= color(blue)(6.24 xx 10^(-12) "cm"^3"/molecule"cdot"s")`

or perhaps in units we are more familiar with... this is equal to `3.76 xx 10^9 "M"^(-1)cdot"s"^(-1)`.

METHOD 2

Or, if you aren't that visual... on Excel, simply set up data columns like this:

Then select D3 through E9 and go to Insert > Recommended Charts > All Charts > X Y (Scatter).

You should get this:

With a little bit of formatting, you could get this:

And by right-clicking on the data point, go to Add Trendline, then scroll down to find and click "Display equation on chart" and "Display R-squared value on chart".

What you should end up with is:

From this we should again compare to the straight-line version of the Arrhenius equation:

`ln k = -E_a/R 1/T + ln A`

From this, the example slope is

`-E_a/R = -"359.78 K"^(-1)`

and the example y-intercept is

`ln A = -25.798`

Therefore, the activation energy is:

`color(blue)(E_a) = -R cdot "slope"`

`= -8.314 cancel"J""/mol"cdotcancel"K" xx ("1 kJ")/(1000 cancel"J") xx -359.78 cancel("K"^(-1))`

`=` `color(blue)("2.99 kJ/mol")`

and the frequency factor is:

`color(blue)(A) = e^("y-intercept")`

`= e^(-25.798)`

`= color(blue)(6.25 xx 10^(-12) "cm"^3"/molecule"cdot"s")`

or perhaps in units we are more familiar with... this is equal to `3.77 xx 10^9 "M"^(-1)cdot"s"^(-1)`.

We more-or-less got the same thing either way, so both ways work.