How to derive if the reaction is endothermic or exothermic based on rate constants at different temperatures? [closed]








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> 
> Listed in the table are forward and reverse rate constants for the reaction $$\ce{2NO (g) <=> N\_2 (g) + O\_2 (g)}$$
>  \begin{array}{ccc}
> \text{Temperature}/\pu{K} & k\_f/\pu{M^-1s^-1} & k\_r /\pu{M^-1s^-1} \\\hline
> 1400 & 0.29 & 1.1\times10^{-6}\\
> 1500 & 1.3 & 1.4\times10^{-5}\\
> \end{array}
>  Is the reaction endothermic or exothermic?
> 
> 
> 


In my book the solution is given as



> 
> $k\_r$ increase more than $k\_f$, this means that $E\_a$ (reverse) is greater than $E\_a$ (forward). The reaction is exothermic when $E\_a$ (reverse) > $E\_a$ (forward).
> 
> 
> 


I can not understand what they mean by the given answer. 
Can anybody explain it in more detail?


