What is the percent yield if 185 grams of SiO₂ are made from 328 g of Cr₂O₃ by the following equation?
3 Si(s) + 2 Cr₂O₃(s) → 3 SiO₂(s) + 4 Cr(l)

Question

What is the percent yield if 185 grams of SiO₂ are made from 328 g of Cr₂O₃ by the following equation? 3 Si(s)+ 2 Cr₂O₃(s)→ 3 SiO₂(s)+ 4 Cr(l) A)142% B)70% C)56% D)105% E)95%

Quizplus · Accepted Answer

To find the percent yield, first calculate the theoretical yield of SiO2. The molar mass of Cr2O3 is approximately 152 g/mol, and the molar mass of SiO2 is approximately 60 g/mol. From the balanced equation, 2 moles of Cr2O3 produce 3 moles of SiO2. Therefore, 328 g of Cr2O3 is approximately 2.16 moles, which should produce 3.24 moles of SiO2, or about 194.4 g. The percent yield is (actual yield/theoretical yield) x 100 = (185/194.4) x 100 ≈ 95%.

What Is the Percent Yield If 185 Grams of SiO2

What Is the Percent Yield If 185 Grams of SiO₂