They are equal, and NONzero.
At dynamic chemical equilibrium, the rates of the forward and reverse reactions are equal to each other, i.e.
$aA + bB stackrel(k_1" ")(rightleftharpoons) cC + dD$
$" "" "" "" "^(k_(-1))$
For this, assuming the equilibrium consists of elementary reactions, the forward and reverse rate law are:
$r_1(t) = k_1[A]^a[B]^b$
$r_(-1)(t) = k_(-1)[C]^c[D]^d$
At equilibrium,
$k_1[A]^a[B]^b = k_(-1)[C]^c[D]^d$
From this, we obtain:
$K -= k_1/(k_(-1)) = ([C]^c[D]^d)/([A]^a[B]^b)$
We know that rate constants are temperature-dependent, and thus, so is
It is also important to note that the rates of the forward and reverse reactions MUST be nonzero to have a dynamic chemical equilibrium.