In the reaction PCl5( g) ⇌PCl3( g)+Cl2( g), the equilibrium concentrations of PCl5 and PCl3 are

step 1 In this problem we have given a reaction. PCL5 reacts reversibly to give PCL3 gas and CL2 gas. G

In the reaction PCl5( g) ⇌PCl3( g)+Cl2( g), the equilibrium...

In the reaction $\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})$, the equilibrium concentrations of $\mathrm{PCl}_5$ and $\mathrm{PCl}_3$ are 0.4 and $0.2 \mathrm{~mole} / \mathrm{litre}$ respectively. If the value of $\mathrm{K}_{\mathrm{c}}$ is 0.5 , what is the concentration of $\mathrm{Cl}_2$ in mole/ litre? (a) 2.0 (b) 1.5 (c) 1.0 (d) 0.5

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Key Concepts

Equilibrium Constant (Kc)

The equilibrium constant, designated as Kc when concentrations are used, is a numerical value that quantifies the ratio of the concentrations of products to reactants at equilibrium, with each concentration raised to the power of its stoichiometric coefficient. It provides a measure of the extent to which a reaction proceeds before reaching equilibrium.

Law of Mass Action

The law of mass action is the principle used to derive the equilibrium constant expression for a chemical reaction. It states that at equilibrium, the rate of the forward reaction is proportional to the product of the concentrations of the reactants and that the equilibrium constant is formed by the ratio of the product of the concentrations of the reaction products to the product of the concentrations of the reactants.

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions are equal, leading to constant concentrations of both reactants and products over time. This concept is fundamental in understanding how systems balance in dynamic conditions.

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