Here’s how you could do that.

The Arrhenius equation does not include a ##T_2##, it only includes a ##T##, the absolute temperature at which the reaction is taking place.

However, you can use the Arrhenius equation to determine a ##T_2##, provided that you know a ##T_1## and the rate constants that correspond to these temperatures.

The Arrhenius equation looks like this

##color(blue)(|bar(ul(color(white)(a/a)k = A * “exp”(-E_a/(RT))color(white)(a/a)|)))” “##, where

##k## – the rate constant for a given reaction

##A## – the pre-exponential factor, specific to a given reaction

##E_a## – the activation energy of the reaction

##R## – the universal gas constant, useful here as ##8.314″J mol”^(-1)”K”^(-1)##

##T## – the absolute temperature at which the reaction takes place

So, let’s say that you know the activation energy of a chemical reaction you’re studying.

You perform the reaction at an initial temperature ##T_1## and measure a rate constant ##k_1##. Now let’s say that you’re interested in determining the temperature at which the rate constant changes to ##k_2##.

You can use Arrhenius equation to write

##k_1 = A * “exp”(-E_a/(R * T_1))##

and

##k_2 = A * “exp”(-E_a/(R * T_2))##

To find ##T_2##, divide these two equations

##k_1/k_2 = color(red)(cancel(color(black)(A)))/color(red)(cancel(color(black)(A))) * (“exp”(-E_a/(R * T_1)))/(“exp”(-E_a/(R * T_2)))##

Use the property of exponents

##color(purple)(|bar(ul(color(white)(a/a)color(black)(x^a/x^b = x^((a-b)), AA x !=0)color(white)(a/a)|)))##

to rewrite the resulting equation as

##k_1/k_2 = “exp”[E_a/R * (1/T_2 – 1/T_1)]##

Next, take the natural log of both sides of the equation

##ln(k_1/k_2) = ln(“exp”[E_a/R * (1/T_2 – 1/T_1)])##

This will be equivalent to

##ln(k_1/k_2) = E_a/R * (1/T_2 – 1/T_1)##

Finally, do some algebraic manipulation to isolate ##T_2## on one side of the equation

##ln(k_1/k_2) = E_a/R * 1/T_2 – E_a/R * 1/T_1##

##1/T_2 = ln(k_1/k_2) + E_a/R * 1/T_1##

Therefore,

##color(green)(|bar(ul(color(white)(a/a)color(black)(T_2 = (R * T_1)/(R * T_1 * ln(k_1/k_2) + E_a))color(white)(a/a)|)))##