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

the answer is definitely c.

it takes on an electronical energy