We have
`"log" K_(p2)-log K_(p1)=(DeltaH)/(2.303 R)xx(T_(2)-T_(1))/(T_(2)T_(1))`
As we know from the above equation that if on increasing temperature, `K_(p)` increases, `DeltaH` becomes positive, i.e., the reaction is endothermic. Thus, from the given data, we see that the reaction is endothermic.