🤓 Based on our data, we think this question is relevant for Professor Tucci & Matchacheep's class at HARVARD.

C_{2}H_{6} + Cl_{2} → C_{2}H_{5}Cl + HCl

**$\mathbf{106}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{6}}}\mathbf{}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{6}}}}{\mathbf{30}\mathbf{.}\mathbf{068}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{6}}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{5}}\mathbf{Cl}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{6}}}}\mathbf{\times}\frac{\mathbf{64}\mathbf{.}\mathbf{51}\mathbf{}\mathbf{g}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{5}}\mathbf{Cl}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{5}}\mathbf{Cl}}}$ =227.42 g C _{2}H_{5}Cl**

When ethane (C_{2}H_{6}) reacts with chlorine (Cl_{2}), the main product is C_{2}H_{5}Cl; but other products containing Cl, such as C_{2}H_{4}Cl_{2}, are also obtained in small quantities. The formation of these other products reduces the yield of C_{2}H_{5}Cl.

A) Calculate the theoretical yield of C_{2}H_{5}Cl when 106 g of C_{2}H_{6 }reacts with 247 g of Cl_{2}, assuming that C_{2}H_{6 }and Cl_{2 }react only to form C_{2}H_{5}Cl and HCl.

B) Calculate the percent yield of C_{2} H_{5} Cl if the reaction produces 181 g of C_{2} H_{5} Cl.

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