Q5P - Chemistry: Molecular Nature Of Matter And Change

Question

White phosphorous, ${\mathbf{p}}_{\mathbf{4}}$, is produced by the reduction of phosphate rock, ${\mathbf{Ca}}_{\mathbf{3}}{\left({\mathrm{PO}}_4\right)}_{\mathbf{2}}$.If exposed to oxygen, the waxy, white solid smokes, bursts into flames, and releases a large quantity of heat. Does the reaction ${\mathbf{P}}_{\mathbf{4}}\left(g\right)\mathbf{+}\mathbf{5}{\mathbf{O}}_{\mathbf{2}}\left(g\right)\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{P}}_{\mathbf{4}}{\mathbf{O}}_{\mathbf{10}}\left(S\right)$ have a large or small equilibrium constant? Explain. 

Step-by-Step Solution

Answer

The answer is,

Yes, a small equilibrium constant  

Step 1: Equilibrium

The equilibrium state of a reaction is represented using the double-headed arrows and the equilibrium constant is used to denote the scene mathematically. It is the ratio of the concentration of products to the ratio of the concentration of the reactants.

Step 2: Explanation

The equilibrium constant K of a reaction is written as the ratio of the concentration of the products to the concentration of the reactants of the aqueous or gaseous substances. The solid and liquid substances are omitted from the equilibrium constant equation.

Hence the equilibrium constant of the given equation can be written as shown below.

                                                             $\mathrm{K}=\frac{1}{\left[{\mathrm{P}}_4\right]{\left[{\mathrm{O}}_2\right]}^5}$

Therefore the value of K will be very small.