Percentage Yield

Multiple Choice Red mercury (II) oxide decomposes to form mercury metal and oxygen gas according to the following equation: 2HgO (s) 2Hg (l) + O2 (g). If 3.55 moles of HgO decompose to form 1.54 moles of O2 and 618 g of Hg, what is the percent yield of this reaction? a-13.2% b-42.5% c-56.6% d-86.5%

Multiple Choice In the manufacturing process of sulfuric acid, sulfur dioxide is reacted with oxygen to produce sulfur trioxide. Using the equation, 2SO2 (g) + O2 2SO3 (g), if 192 g of sulfur dioxide is given the opportunity to react with an excess of oxygen to produce 225 g of sulfur trioxide, what is the percent yield of this reaction? a-46.8% b-70.2% c-93.7% d-99.9%

Multiple Choice In the manufacturing process of sulfuric acid, sulfur dioxide is reacted with oxygen to produce sulfur trioxide. Using the equation, 2SO2 (g) + O2 2SO3 (g), if 64.06g of sulfur dioxide is given an opportunity to react with an excess of oxygen to produce 75.00 g of sulfur trioxide, what is the percent yield of this reaction?  a. 46.83%  b. 60.25%  c. 75.55%  d. 93.68% 

True or False The percent yield for a chemical reaction can not be calculated until the reaction is completed. a. True b. False

True or False The actual yield can be less than the predicted (theoretical) yield. a. True b. False

True or False The actual yield is usually less than the predicted (theoretical) yield. a. True b. False