Which of the following is the correct form of the equilibrium constant expression for the following reaction?A(aq) + B(aq) ⇄ D(aq) + E(aq)
([D] * [E]) / ([A] * [B])
Will it always be products divided by reactants?
yes
To determine the correct form of the equilibrium constant expression for a reaction, we need to know the stoichiometric coefficients of the reactants and products in the balanced equation.
In this case, the balanced equation for the reaction is:
A(aq) + B(aq) ⇄ D(aq) + E(aq)
The general form of the equilibrium constant expression is:
Kc = ([products])/([reactants])
To write the equilibrium constant expression, we need to consider the concentration of each species involved. Let's assign variables to represent the concentrations:
[A] = concentration of A(aq)
[B] = concentration of B(aq)
[D] = concentration of D(aq)
[E] = concentration of E(aq)
Now we can write the equilibrium constant expression:
Kc = ([D][E])/([A][B])
Therefore, the correct form of the equilibrium constant expression for the given reaction is:
Kc = ([D][E])/([A][B])