The variation of rate constant with temperature is given by the integrated from of the Arrhenius equation, `log_10k = (-Ea)/(2.303 RT)` + constant
where k = rate cosntant and Ea is the experimental activation energy. If for a certain reaction, `log_10k = (-3163.0)/T + 11.899`, calculate Ea.

Explanation

To solve the problem, we need to calculate the activation energy (Ea) from the given equation of the rate constant (k) in relation to temperature (T). The equation provided is:

\[ \log_{10} k = \frac{-3163.0}{T} + 11.899 \]

We can compare this with the integrated form of the Arrhenius equation:

...