# If the reaction quotient, Q, for a reaction is less than the value of the equilibrium constant, K, for the reaction at a given temperature what must be converted to work for the system to reach equilibrium?

Feb 27, 2017

The equilibrium must move in a forward direction..........

#### Explanation:

For the reaction,

$A + B r i g h t \le f t h a r p \infty n s C + D$,

we write ${K}_{e q} = \frac{\left[C\right] \left[D\right]}{\left[A\right] \left[B\right]}$

This describes an equilibrium condition, where the rate of forward reaction is equal to the reverse rate of reaction.

Under non-equilibrium conditions, (for instance at the start of the reaction), we write ${Q}_{\text{rxn quotient}} = \frac{\left[C\right] \left[D\right]}{\left[A\right] \left[B\right]}$.

At the start of the reaction, we can conceive that the reactant concentrations, $\left[A\right]$ and $\left[B\right]$, are LARGER than they would be at equilibrium, so ${Q}_{\text{rxn}}$ $<$ ${K}_{\text{eq}}$, and so the reaction proceeds in a forward direction, until ${Q}_{\text{rxn}}$ $=$ ${K}_{\text{eq}}$.