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Problem: The reaction of 11.9 g of CHCl3 with excess chlorine produced 11.2 g of CCl4, carbon tetrachloride:What is the percent yield?A. 94%B. 36.4%C. 100%D. 48.5%E. 72.8%

🤓 Based on our data, we think this question is relevant for Professor St Hill's class at UH.

FREE Expert Solution

Establish the balanced equation of the reaction of CHCl3 and CCl4 and use stoichiometry to determine the actual yield and eventually the percent yield

The balanced equation of CHClwith Cl2 will appear as:

CHCl+ Cl→ CCl4 + HCl

Recall that percent yield is given by:

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Problem Details

The reaction of 11.9 g of CHCl3 with excess chlorine produced 11.2 g of CCl4, carbon tetrachloride:

What is the percent yield?

A. 94%

B. 36.4%

C. 100%

D. 48.5%

E. 72.8%

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Based on our data, we think this problem is relevant for Professor St Hill's class at UH.