Equilibrium constant and reaction Quotient
$K$ is just the specific value of $Q$ for which $\Delta_\mathrm r G = 0$.
In that case:
$$\begin{align}
\Delta_\mathrm r G &amp;= \Delta_\mathrm r G^\circ + RT \ln Q \\
0 &amp;= \Delta_\mathrm r G^\circ + RT \ln K \\
\Delta_\mathrm r G^\circ &amp;= -RT \ln K 
\end{align}$$

For any system not at the equilibrium it is possible that $Q &lt; K$ or $Q &gt; K$. What is the "forward direction" is just a convention, it depends on how you decide to write the equilibrium. There is nothing special in one direction or the other. The system will "move" toward the direction that leads to equilibrium in both cases. In the first case the reaction will consume reactants to generate products, while in the second case the opposite will happen.
You can express this idea also in terms of the ratio $\frac Q K$. If it is > 1 then the reaction will consume reactants. This is also often referred to as the "Le Chatelier principle".