Use the equation C6H6 + Cl = C6H3Cl + HCL what is the theoretical yield of C6H6Cl if 22.8 if C6H6 react

Write the balanced equation-

C6H6 + Cl2 - - > C6H5Cl + HCl

1 mol C6H6 reacts with 1 mole Cl2 to yield 1 mole of C6H5Cl

Calculate the moles of each reactant-

36.8 g C6H6 / 78.1 g/mol = 0.471 mol C6H6

36.9 g Cl2 / 70.9 g/mol = 0.520 mol Cl2

0.471 mole C6H6 requires 0.471 mole Cl2. You have excess Cl2 so C6H6 is limiting.

0.471 mole C6H6 will yiels (at 100%) 0.471 mole C6H5Cl

0.471 mol x 112.5 g/mol = 53.0 g C6H5Cl

38.8 g actual / 53.0 theoretical = 0.732 (73.2% yield)