percent yield???

Question

Titanium dioxide )TiO2) is an industrial chemical used as white pigment in paint. The conversion of volatile TiCl4 to TiO2 occurs according to the reaction. If 15.70g of TiCl4 reacts in excess oxygen to form 10.40g Cl2, what is the percent yield of the reaction?

Answer 1

TiCl4 + O2 -> TiO2 + 2Cl2
Reacting 1 mole of TiCl4 with 1 mole of O2 can form 2 mole of Cl2 gas.
(Molecular weight of TiCl4 = 189.73)

Thus, 15.70g of TiCl4 = 15.70/189.73 = 0.08275 mole

Theoretically, 0.08275 mole x 2 of Cl2 gas will form, thus it will be 0.1655 mole

molecular weight of Cl2 = 70.9
10.40g of Cl2 = 10.40/70.9 = 0.1467 mole

The yield percentage =
experimental yield/theoretical yield x 100%
0.1467/0.1655 x 100%
= 88.63 %

Answer 2

TiCl4 + O2 ---> Ti O2 +2 Cl2 the molecular weight of T1 is 48

so TiCl4 MW = 48 +4*35.5 = 190 and 2CL2 MW =2*71=142

so if the reaction had a yield of 100%

15.7 of TiCl4 would give 15.7 *142/190 =11.733

as you have only 10.4

the percent yield is 10.4*100/11.733 = 88%