Chapter 5, Problem 5.93P

The reaction of methane ${\text{(CH}}_{\text{4}}\text{)}$ with Cl₂forms chloroform (CHCl₃) and HCl. Although CHCl₃ is a general anesthetic, it is no longer used for this purpose because it is also carcinogenic. The molar masses for all substances are given under the balanced equation.

   ${\text{CH}}_{\text{4}}\text{(g) }+3{\text{Cl}}_{\text{2}}(g)\to C{\text{HCl}}_{\text{3}}\text{(l), + 3HCl(g)}$

   $\text{16}\text{.04 g/mol 70}\text{.90 g/mol 119}\text{.4 g/mol 36}\text{.46 g/mol}$

1. What is the theoretical yield of ${\text{CHCl}}_{\text{3}}$ in grams from 32.0 g of ${\text{CH}}_{\text{4}}\text{?}$

What is the percent yield if 15.0 g of ${\text{CHCl}}_{\text{3}}$are actually formed in this reaction?