For a reaction, e.g., $$a X + b Y → c Z$$ Its reaction rate constant is $${\displaystyle r=k_f(T)[\mathrm {X} ]^{m}[\mathrm {Y} ]^{n}}$$ where the exponents m and n are called partial orders of reaction and are not generally equal to the stoichiometric coefficients a and b.
However, for the equilibrium constant, the exponents must be stoichiometric, e.g., $$K_c=\frac{[Z]^c}{[X]^a [Y]^b}$$
However, for reversible chemical reaction, $K_c=k_f/k_b$ which means that stoichiometric coefficients are required for equilibrium. Does this mean that when the exponents of the rate reaction equation are similar to that of stoichiometric coefficients, the reaction is in equilibrium?