#### Answer

The reverse reaction will occur, so the forward reaction will not occur.

#### Work Step by Step

1. Write the equilibrium constant expression:
- The exponent of each concentration is equal to its balance coefficient.
$$K_C = \frac{[Products]}{[Reactants]} = \frac{[ H_2O ][ CO ]}{[ H_2 ][ CO_2 ]}$$
2. At equilibrium, these are the concentrations of each compound:
$ [ H_2 ] = 3.0 \times 10^{-5} \space M - x$
$ [ CO_2 ] = 3.3 \times 10^{-4} \space M - x$
$ [ H_2O ] = 1.6 \times 10^{-2} \space M + x$
$ [ CO ] = 6.25 \times 10^{-3} \space M + x$
$$1.11 = \frac{(1.6 \times 10^{-2} + x)(6.25 \times 10^{-3} + x)}{(3.0 \times 10^{-5} - x)(3.3 \times 10^{-4} - x)}$$
$x_1 = -0.0043$
$x_2 = 0.21$
$x_2$ is invalid, because $[H_2] = 3.0 \times 10^{-5} - 0.21 = $ negative number. A concentration cannot be negative.
So x = -0.0043
Which means that the concentration of reactants will increase, and the same of the products will decrease, which means that the reverse reaction will occur.