Question

Carlos is making phosphorus trichloride using the equation below. He uses 15.5 g of phosphorus and collects 50.9 g of phosphorus chloride. 2P +3Cl2 → 2PCl3 How much chlorine reacted with the phosphorus? 15.5 g 17.7 g 35.4 g 66.4 g

Answer 1

Answer: 35.4 g

Explanation:

The balanced reaction is :

$2P+3Cl_2\rightarrow 2PCl_3$

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$    

$\text{Moles of phosphorous}=\frac{15.5g}{31g/mol}=0.50moles$

$\text{Moles of phosphorous chloride}=\frac{50.9g}{137g/mol}=0.372moles$

$2P+3Cl_2\rightarrow 2PCl_3$

According to stoichiometry :

2 moles of phosphorous chloride are produced by = 3 moles of $Cl_2$

Thus 0.37 moles of phosphorous chloride are produced by=$\frac{3}{2}\times 0.372=0.558moles$ of $Cl_2$

Mass of $Cl_2=moles\times {\text {Molar mass}}=0.558moles\times 71g/mol=35.4g$

Thus 35.4 g of chlorine reacted with the phosphorus

Answer 2

Answer:

c

Explanation: