When ethane (C2H6) reacts with chlorine (Cl2) the main product is C2H5Cl; but other products containing Cl (chlorine), such as C2H4Cl2, are also obtained in small quantities. The formation of these other products reduces the yield of C2H5Cl. In a certain experiment 185 g of C2H6 reacts with 205 g of Cl2.
(a) Assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl, calculate the theoretical yield of C2H5Cl.
_______g
(b) Calculate the percent yield of C2H5Cl if the reaction produced 162 g of C2H5Cl.
_______%
Correct Sig Figs please!
Answers (1)
(a)
C2H6 + Cl2 → C2H5Cl + HCl
(185 g C2H6) / (30.06924 g C2H6/mol) = 6.1525 mol C2H6
(205 g Cl2) / (70.9064 g Cl2/mol) = 2.8911 mol Cl2
2.8911 moles of Cl2 would react completely with 2.8911 x (1/1) = 2.8911 moles of C2H6, but there is more C2H6 present than that, so C2H6 is in excess and Cl2 is the limiting reactant.
(2.8911 mol Cl2) x (1 mol C2H5Cl / 1 mol Cl2) x (64.5145 g C2H5Cl/mol) =
187 g C2H5Cl in theory
(b)
(162 g) / (187 g) = 0.866 = 86.6% yield