For a reversible reaction ${\mathrm{K}}_{\mathrm{p}}<{\mathrm{K}}_{\mathrm{c}}$, for this reaction at equilibrium, increase of pressure favours

Given K_P <  K_C

We know K_P = K_C (RT)^Δn

given  

only when Δn_g is negative.

Δn_g = n_p (g) - n_R (g)

is negative

n_p (g) < n_R (g)

From left to right i.e. forward reaction involves  decrease  in volume.

According to Le-Chatlier's principle reactions involving decrease in volume are favoured at high pressure.