P4 + 6Cl2 -- 4PCl3
I have 1 mol Cl2 and 2 mol P4
How do I predict the product? Which mol ratios do I use?

Question

P4 + 6Cl2 --> 4PCl3
I have 1 mol Cl2 and 2 mol P4
How do I predict the product? Which mol ratios do I use?

anonymous · Answer

|dw:1406176218197:dw|

aaronq · Answer

You would need to find the limiting reagent first.

This can be done by dividing the moles of each reactant by their corresponding stoichiometric coefficient in the balanced equation:

$\sf \dfrac{moles~of~Cl_2}{6}=\dfrac{1}{6}mol$

$\sf \dfrac{moles~of~P_4}{1}=\dfrac{2}{4}=\dfrac{1}{2}mol$

Now by comparison we see that $Cl_2$ is the limiting reagent (less moles).

We use the those moles and the same concept, make a ratio of the $Cl_2$, $PCl_3$ and their coefficients:

$\sf \dfrac{moles~of~Cl_2}{6}=\dfrac{moles~of~PCl_3}{4}$

            $\sf \dfrac{1~mol}{6}=\dfrac{moles~of~PCl_3}{4}$

$\sf moles~of ~PCl_3=\dfrac{1*4}{6}mol=0.667 ~mol$