Some chemical reactions may have come to an equilibrium,

**A+2B ≈ 3C+2D**

At a given temperature this reaction will eventually come to chemical equilibrium, the double half-arrows indicate that both the forward reaction and the reverse reaction are still occurring simultaneously and the rates of the forward and reverse reactions have become equal at equilibrium. Once the reaction has reached equilibrium the concentrations of the reactants and products are then constant and are related to one another by the reaction’s equilibrium constant K_{C}, which is characteristic of the reaction at that temperature. For solutions, the concentrations (e.g. c_{A}) are conventionally written as a pure number, with the molecule’s symbol in square brackets, e.g. [A], times the units of mol L^{-1}.

In the equation for K_{C} each concentration is divided by its own standard state concentration. We use as the symbol for standard state a superscript degree which is pronounced as “naught”, “zero” or “standard”. For solutes, the standard state concentration are e.g. c°_{A} = 1 mol L^{-1}. The units will cancel out to give the pure number “dimensionless concentrations” e.g. [A]. So K_{c} the equilibrium constant must also be dimensionless. In chemical equilibria each of the concentrations is raised to the same power as its stoichiometric coefficient.

Firstly, for the above equilibrium reaction calculate the value of the equilibrium constant K_{c} in a solution where all four of the concentrations are equal to 0.1 mol L^{-1}. Secondly, calculate the new concentration of [C] if we alter the concentrations to [A] = 0.2 mol^{-1}, [B] = 0.15 mol L^{-1} and [D] = 0.25 mol^{-1 }?

**Solution**

Firstly, we need to find the value for the equilibrium constant,

Secondly, we rearrange the chemical equilibrium constant equation so that [C] is the subject of the equation. This is done sequentially by: (1) multiplying both sides of the equation by [A] [B]^{2}; (2) and then cancelling out top and bottom within any single term;

(3) then dividing by [D]^{2} on both sides of the equation and cancelling top and bottom within any single term;

(4) writing [C]^{3} as the subject; (5) substituting in the physical quantities; and (6) taking the cube root of [C]^{3} gives the concentration of molecule C.

As [C] is the symbol for the pure number of the concentration, so the concentration in mol L^{-1} is

**[C] = 8.96 x 10 ^{-2} C_{c }= [C] mol L^{-1}**

Increasing the concentrations of [A], [B] and [D] has decreased the concentrations of [C] in order to maintain the chemical equilibrium constant K_{c} at a constant value.

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