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)
You don't give any choices but K = (D)(E)/(A)(B)
The correct form of the equilibrium constant expression for the given reaction A(aq) + B(aq) ⇄ D(aq) + E(aq) can be written as:
Kc = ([D][E])/([A][B])
Kc represents the equilibrium constant and square brackets indicate the molar concentrations of the respective species.
To find the correct form of the equilibrium constant expression for the given reaction, we need to determine the concentrations of the products and reactants.
In this reaction, A(aq) and B(aq) are the reactants, while D(aq) and E(aq) are the products.
The equilibrium constant expression, also known as Kc, is defined as the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficient in the balanced chemical equation.
Therefore, the correct form of the equilibrium constant expression for the given reaction is:
Kc = [D(aq)]/[A(aq)] * [E(aq)]/[B(aq)]
Here, the square brackets represent the concentration of each species.
Note: The equilibrium constant expression can also be written using partial pressures instead of concentrations, depending on the state of the reactants and products (i.e., if they are gases). In that case, the expression would use the partial pressure values instead of concentrations.