This is probably a super easy problem but the studying overload has made me mix everything up 
So when solving for K, you know how we do the concentration of products of concentration of reactants??
If its a diatomic molecule like Cl2, don't we do [Cl-]^2 ? I got a question and it seems to solve by [Cl2] ?!
The question is:
When 14.250 moles of PCl(5) gas is placed in a 3.0 liter container and comes to equilibrium at a constant temperature, 40.0% of the PCl(5) decomposes according to the equation:
PCl(5)(g) ----> PCl(3)(g) + Cl(2)(g)
<---
What is the value of K(c) for this reaction?
The answer is (1.896)^2/2.854
I understand where the numbers come from, but if there is the (1/896)^2 it means that this question was solved by doing x^2 for [PCl3] and [Cl2] but i thought Cl2 would be [Cl-]^2 aka x^3.....If someone could clarify thak you!!!!
So when solving for K, you know how we do the concentration of products of concentration of reactants??
If its a diatomic molecule like Cl2, don't we do [Cl-]^2 ? I got a question and it seems to solve by [Cl2] ?!
The question is:
When 14.250 moles of PCl(5) gas is placed in a 3.0 liter container and comes to equilibrium at a constant temperature, 40.0% of the PCl(5) decomposes according to the equation:
PCl(5)(g) ----> PCl(3)(g) + Cl(2)(g)
<---
What is the value of K(c) for this reaction?
The answer is (1.896)^2/2.854
I understand where the numbers come from, but if there is the (1/896)^2 it means that this question was solved by doing x^2 for [PCl3] and [Cl2] but i thought Cl2 would be [Cl-]^2 aka x^3.....If someone could clarify thak you!!!!