The rate constant for the reaction, A₂B₄O→AB₄ +AO is described as, $$\log k = 14.1 - \frac{10000 \, \text{K}}{T}$$. The activation energy for this reaction (in kJ mol^-1) is closest to

Correct option is A

It is found experimentally for many reactions that a plot of ln k against 1/T gives a straight line. This behaviour is normally expressed mathematically by introducing two parameters, one representing the intercept and the other the slope of the straight line, and writing the Arrhenius equation​

​The parameter A, which corresponds to the intercept of the line at 1/T = 0, is called the pre-exponential factor or the ‘frequency factor’. The parameter E_a, which is obtained from the slope of the line

​is called the activation energy. Collectively the two quantities are called the Arrhenius parameters

​The fact that E_a is given by the slope of the plot of ln k against 1/T means that, the higher the activation energy, the stronger the temperature dependence of the rate constant (that is, the steeper the slope). A high activation energy signifies that the rate constant depends strongly on temperature. If a reaction has zero activation energy, its rate is independent of temperature. In some cases the activation energy is negative, which indicates that the rate decreases as the temperature is raised.