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If 5 moles of P4 reacted with 22 moles Cl2 according to the above reaction, determine:

AHow many moles PCl3 are produced ________________
BHow many moles of P4 are left in excess after the reaction (if any) ________________
CHow many moles of Cl2 are left in excess after the reaction (if any) ________________

Verified Answer :

Solution:

\(P_4+6Cl_2\rightarrow 4PCl_3\)

a) By stoichoimetry If 6 moles of \(Cl_2\) gives 4 mole of \(PCl_3\) , then 22 moles of \(Cl_2\) will give: \(\frac{4}{6}\times 22=\frac{44}{3}=14.66\) moles of \(PCl_3\)

b) If 6 moles of \(Cl_2\) reacts with one mole of \(P_4\) , then 22 moles of \(Cl_2\) will react : \(\frac{1}{6}\times 22=\frac{11}{3}=3.66\) moles of \(P_4\)

Moles of \(P_4\)  left after the reaction = \(5-3.66=\frac{4}{3}=1.34\) moles.

c) 0 Moles of \(Cl_2\) , since it is present in less amount it will get completely consumed in the reaction. Hence, it is limiting reagent.



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