<span>73.0%
First, lookup the atomic weights of the elements involved
Atomic weight carbon = 12.0107
Atomic weight chlorine = 35.453
Atomic weight hydrogen = 1.00794
Calculate the molar masses.
Molar mass CHCl3 = 12.0107 + 1.00794 + 3 * 35.453 = 119.37764
Molar mass CCl4 = 12.0107 + 4 * 35.453 = 153.8227
Calculate the number of moles we have
Moles CHCl3 = 11.9 g / 119.37764 g/mol = 0.099683659 mol
Moles CCl4 = 11.2 g / 153.8227 g/mol = 0.0728111 mol
Since with 100% yield, each molecule of CHCl3 should produce one molecule of CCl4, divide the actual moles produced by the number of moles expected for 100% yield. So
0.0728111 / 0.099683659 = 0.730421623 = 73.0421623 %
Rounding to 3 significant figures gives 73.0%</span>
First, we need to calculate the theoretical yield as follows: The balanced chemical reaction is: <span>2CHCl3 +2Cl2 ----> 2CCl4 +2HCl </span>molar mass of CHCl3 = <span>119.378 grams molar mass of CCl4 = </span>153.823 grams<span> number of moles = mass / molar mass = 11.9 / 119.378 = 0.0997 moles From the balanced equation, 2 moles of CHCl3 produce 2 moles of CCl4. Therefore, 0.0997 moles of CHCl4 will produce 0.0997 moles of CCl4. number of moles = mass / molar mass mass (theoretical) = molar mass * number of moles mass (theoretical) = </span><span>153.823 * 0.0997 = 15.336 grams
Now, we will calculate the percent yield as follows: % yield = (actual mass / theoretical mass) * 100 % yield = (11.2 / 15.336) * 100 = 73.03%</span>
