Transcript lesson 17 PPT

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