A gaseous system containing \(\text{N}_2\text{O}_4\text{(g)}\) and \(\text{NO}_2\text{(g)}\) at \(350 \text{ K}\) is represented in the diagram below. The reversible reaction is represented by the following equation:

\[ \text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\,\text{NO}_2\text{(g)} \quad K_c = 2.0 \text{ at } 350 \text{ K} \]

The reaction vessel has a rigid volume of \(1.0 \text{ L}\), and each particle in the diagram represents \(1.0 \text{ mol}\) of the designated gas. Which of the following correctly compares the forward and reverse reaction rates at the instant shown and provides the valid justification?