Answer
$$K_p = 4.42 \times 10^{-5}$$
The reactants are favored at equilibrium.
Work Step by Step
- Since the reaction was inverted, the new equilibrium constant will be equal to the multiplicative inverse of the original one:
$$K_p = \frac 1{2.26 \times 10^{4}} = 4.42 \times 10^{-5}$$
- Since $K_p \lt 1$, the reactants will be favored at equilibrium.
