How to calculate activation energy from an equation?

To solve
\(ln(\frac{{{K}_{2}}}{{{K}_{1}}}) = \frac{{{E}_{a}}}{R}*\frac{{{T}_{2}}-{{T}_{1}}}{{{T}_{2}}{{T}_{1}}}\)
for activation energy, you would multiply both sides by RT2T1 and then divide both sides by (T2 - T1).  The result:

\(\frac{R*{{{T}_{2}}*{{T}_{1}}}*ln(\frac{{{K}_{2}}}{{{K}_{1}}})}{({{T}_{2}}-{{T}_{1}})} = {{E}_{a}}\)

I believe for this you would use 8.3144621 J K−1mol−1 as the value of R, the gas constant.

If I am not understanding the question, please let me know.  But as far as I can tell, if you have K1, K2, T1, T2, and R, you should be able to plug this into the derived equation and obtain the activation energy, Ea