Direction

[Jarrett Peyrefitte 2K]

How does the value of the reaction quotient allow the direction of non-equilibrium reaction to be predicted?

[Connie Chen 1E]

If Q<K, then we know that the reaction will favor the forward reaction because there is not enough product for the reaction to be at equilibrium.
If Q>K, then we know the reaction will favor the reverse reaction because there is not enough reactant for the reaction to be at equilibrium.

[Kate Osborne 1H]

if Q is less than K then the reaction will proceed in the forward direction, while if Q is greater than K the reaction will proceed in the reverse direction.

[nicole-2B]

If Q<K, then we know that the reaction will favor the forward reaction because there is not enough product for the reaction to be at equilibrium.
If Q>K, then we know the reaction will favor the reverse reaction because there is not enough reactant for the reaction to be at equilibrium.

Thanks for clarifying!!

[Emily Lo 1J]

If the Q value is less than K, then there is more reactant than there is product in the reaction, and the direction which the reaction favors it forward.
If the Q value is greater than K, then there is more product than there is reactant in the reaction, and the direction which the reaction favors is reverse.