The equation $$k = (6.5 \times 10^{12} s^{-1})e^{-26000 K/T}$$ is followed for the decomposition of compound A. The activation energy for the reaction is ______ KJ mol$$^{-1}$$. [nearest integer]
(Given: R = 8.314 J K$$^{-1}$$ mol$$^{-1}$$)

We are given the Arrhenius equation: $$k = (6.5 \times 10^{12} \text{ s}^{-1})e^{-26000\text{ K}/T}$$. The Arrhenius equation is: $$k = Ae^{-E_a/(RT)}$$, so comparing the exponents gives $$\frac{E_a}{RT} = \frac{26000}{T}$$.

From this, $$\frac{E_a}{R} = 26000 \text{ K}$$ and $$E_a = 26000 \times R = 26000 \times 8.314 \text{ J mol}^{-1}$$.

Therefore, $$E_a = 26000 \times 8.314 = 216164 \text{ J mol}^{-1}$$ and $$E_a = 216.164 \text{ kJ mol}^{-1}$$. Rounding to the nearest integer: $$E_a = 216$$ kJ mol$$^{-1}$$.