A 12.39 g sample of phosphorus reacts with 40.75 g of chlorine to form only phosphorus trichloride (PCl3). If it is the only product, what mass (g) of PCl3 is formed? A possibly useful molar mass is P = 30.974 g/mol; PCl3 = 137.324 g/mol; Cl = 35.45 g/mol.

The answer is "52.18 g"

Explanation:

Phosphorus mass = 12.39  

molar mass of

Phosphorus moles =  

mass = 40.75 g

 molar mass

 moles  =  

The balanced equation is:

In the step1:

Consider reactor limiting the reaction current is less than necessary quantity as per the balanced equation is considered reactor limiting  

The equilibrium equation:

Moles of required = 0.6 moles

But only , moles are less than the amount needed Thus, is reactant restricted  

In the step2:

Find Theoretical performance the amount formed when the reactant is fully restricted

From equilibrium  

shaped mass  =

shaped mass =

Mass shaped by  =

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