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.

a. Calculate the theoretical yield of C2H5Cl when 111 g of C2H6 reacts with 207 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl.

b. Calculate the percent yield of C2H5Cl if the reaction produces 161 g of C2H5Cl.

Answer 1

The chemical reaction is Ca Hota C H5 el the In the reaction 1119 of C₂H6 and 207g of el, s taken . 111 g of C₂H6 = 1118 = 3.7 mole 304 тот" 207 g of cl₂ = 2078 = 2.91 mole 70.99 moſt From the balance equation 0 I mole el, required = 1 mole of C₂H6 2.91 mole el required = 2.91 mole of C₂H6 Howeven will have 3.7 mole of CzH6. That means we have C₂H6 in excess amount. So the product formation of the reaction depends on the amoucht af elz - C2H6 + 4 , Cets el t Hel Thus 1 mole of el, produey= 1 mole of C₂H5 el (2.91 mole of de produces = 2.91 mole of Chsel 1. 2. 207g of ele produces = 64gmatix 2.91 more = 186-24. g. So, the theoretical yield of Ca Hjel is 186.249

Actual yield uage (%) Yield = Theoretical yield X 100%, In experimently 161 g of C₂H5 el is produced from the reaction. so, pencetage (%) yield = Actual Yield looy. pencetage (%) yield - Theoretical field X 1619x1col. = 186•24 g = 86.41