The reaction of 11.9 g of CHCl₃ with excess chlorine produced 10.2 g of CCl₄,carbon tetrachloride: What is the percent yield? A)100% B)33.2% C)66.3% D)86% E)44.2%

Question

Quizplus · Accepted Answer

According to the given information, the theoretical yield of CCl4 can be calculated by stoichiometry as follows:

1 mol CHCl3 produces 1 mol CCl4
Molar mass of CHCl3 = 119.38 g/mol
Molar mass of CCl4 = 153.82 g/mol

Therefore, 11.9 g CHCl3 = 11.9/119.38 = 0.0998 mol CHCl3
And, the theoretical yield of CCl4 = 0.0998 mol CCl4 x 153.82 g/mol = 15.35 g CCl4

The actual yield given in the problem is 10.2 g of CCl4. Therefore, the percent yield can be calculated as:

Percent Yield = actual yield / theoretical yield x 100%
Percent Yield = 10.2 g / 15.35 g x 100% = 66.3%

Hence, the answer is (C).

The Reaction of 11