Phosphorus pentachloride, PCl5(g), undergo decomposition as shown:
PCl5 (g) ⇔ PCl3(g) + Cl2(g)
The equilibrium expression for the reaction is
The equilibrium expression for the reaction is:
Kc = [PCl3(g)][Cl2(g)] / [PCl5(g)]
are you sure?
My apologies for the confusion.
The correct equilibrium expression for the decomposition of phosphorus pentachloride is:
Kc = [PCl3(g)][Cl2(g)] / [PCl5(g)]
To write the equilibrium expression for the given reaction, we need to consider the concentrations of the reactants and products at equilibrium.
The equilibrium expression is written as the ratio of the concentrations of the products raised to their respective stoichiometric coefficients, divided by the ratio of the concentrations of the reactants raised to their respective stoichiometric coefficients.
For the given reaction:
PCl5 (g) ⇔ PCl3(g) + Cl2(g)
The equilibrium expression can be written as:
Kc = [PCl3] * [Cl2] / [PCl5]
Here, [PCl3], [Cl2], and [PCl5] represent the concentrations of PCl3, Cl2, and PCl5 at equilibrium, respectively.
The equilibrium constant (Kc) represents the ratio of the product concentrations to the reactant concentrations at equilibrium, with each concentration raised to its stoichiometric coefficient.
Note that since the reaction is only shown as a single direction with the double arrow, the Kc value represents the ratio of the product concentrations to the reactant concentrations when the reaction reaches equilibrium.