It is desired to produce 3.66 grams of phosphorus trichloride by the following reaction. If the percent yield of phosphorus trichloride is 83.7 %, how many grams of chlorine gas would need to be reacted?

phosphorus (P4) (s) + chlorine (g) phosphorus trichloride (l)

mass of Cl₂ = 1.46 g

Explanation:

given data

mass of phosphorus trichloride = 3.66 G

mas of chlorine gas = ?

efficiency = 83.7 %

balanced chemical equation

2P + 3Cl₂ → 2PCl₃

The mole ration of chlorine and phosphorus trichloride = 3 : 2

First we will find out number of moles of Cl₂ and PCl₃

As we know that:

number of moles = mass / molar mass

number of moles of PCl₃ = 3.66 g / 137.33 g. mol-

number of moles of PCl₃ = 0.027 mol

As the mole ratio of PCl₃ and Cl₂ = 2 : 3

so number of moles of Cl₂ = (0.027 * 3) / 2

number of moles of Cl₂ = 0.041

Now we find the mass of Cl₂

mass of Cl₂ = moles * molar mass

mass of Cl₂ = 0.041 mol * 35.5 g/mol

mass of Cl₂ = 1.46 g