Question

Given: C6H6 + Cl2 --> C6H5Cl + HCl. When 36.8g of C6H6 reacts with an excess of chlorine, the actual yield of C6H5Cl is 38.8g. What is the percent yield and percent error of C6H5Cl?

Answer 1

C6H6 + Cl2 ---------------> C6H5Cl + HCl

HERE WE OBSERVE THAT 78.11 g (MOLAR MASS) OF BENZENE PRODUCES 112.56 g OF chlorobenzene

now 1 g of benzene will produce = 112.56/78.11 = 1.44104468 g chlorobenzene

36.8 g of benzene will produce = 1.44104468 * 36.8 = 53.0304442 g chlorobenzene

% yield = (actual production/ total production) * 100 =(38.8/53.08) * 100 = 72.166 %

error = theoretical - actual

now error = 53.03 - 38.8 = 14.23

% error = (error / theoretical value) * 100= (14.23 / 53.03) * 100 = 26.83%

HERE I HAVE TEKEN UPTO DECIMAL PLACES

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