Question

When ethane (C2H6) reacts with chlorine (Cl2), the main product is C2H5Cl; but other products containing Cl, such as C2H4Cl2, are also obtained in small quantities. The formation of these other products reduces the yield of C2H5Cl.

1. Calculate the theoretical yield of C2H5Cl when 124 g of C2H6 reacts with 202 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl.

2.Calculate the percent yield of C2H5Cl if the reaction produces 164 g of C2H5Cl.

Answer 1

1.The chemical reaction of the given datas

C₂H₆ + Cl₂ --> C₂H₅Cl + HCl

First we have to calculate the molar weight of the two reactants and the C₂H₅Cl. This is done by finding the sum of all the atoms in each compound
Molar Weight
C₂H₆= 12x2 +1x6= 30 g/mol
Cl₂= 35.5x2= 71 g/mol
C₂H₅Cl= 12x2 + 1x5 + 35.5= 64.5 g/mol

Now the reactants must be converted into moles
30 gm contain 1 mole

then 124g contain

like wise 71 g contain 1mole of Cl₂

_{Then 202gm contain =}

This means that Cl₂ is the limiting reagent, and that the C₂H₆ will be in excess.
therefore
C₂H₆ + Cl₂C₂H₅Cl + HCl
2.84 mol 2.84mol

That means it will form 2.84 moles of C₂H₅Cl.

That means 183.18g of yield of C₂H₅Cl.

2. Percentage yield of 164g of C₂H₅Cl.is

Hence yield willbe of C₂H₅Cl if reaction produces 164g 0f C₂H₅Cl