Ethyl chloride is prepared by the reaction of ethane with chlorine according to the reaction: 2 C₂H₆ (g) + Cl₂(g) → C₂H₅Cl(l) + HCl(g)
The percent yield of ethyl chloride in one experiment was 96.3% and the actual yield was 74.4 G) How much ethylene did the chemist use in this experiment?

Question

Quizplus · Accepted Answer

The percent yield is calculated as (actual yield / theoretical yield) x 100%. The theoretical yield is the amount of product that would be produced if the reaction went to completion. In this case, the theoretical yield can be calculated using the stoichiometry of the reaction. For every 2 moles of ethane that react, 1 mole of ethyl chloride is produced. Therefore, the theoretical yield of ethyl chloride is:theoretical yield = (74.4 g / 64.5 g/mol) x (1 mol C2H5Cl / 2 mol C2H6) = 56.8 gThe percent yield is then calculated as:percent yield = (74.4 g / 56.8 g) x 100% = 96.3%This means that the chemist used 96.3% of the theoretical yield of ethyl chloride. Therefore, the amount of ethylene that the chemist used in this experiment is:amount of ethylene used = (56.8 g / 0.963) = 59.0 g

Ethyl Chloride Is Prepared by the Reaction of Ethane with Chlorine