For a reversible reaction temperature is increased, the  incorrect statement is

$K_f=$rate constant of forward reaction

$K_b=$rate constant of backward reaction

$K_{eq}=$Equilibrium constant

As temperature increases, both $K_f$ and $K_b$ increases $K_{eq}=\frac{K_f}{K_b}$

Depending on the magnitude of increase in  $K_f$  and  $K_b$  

$K_{eq}$ may increase (or) decrease