Stoichiometry Chemistry Worksheets With Answers Page 7
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11has been completely consumed. This assumes perfect conditions and gives a maximum amount. The
actual yield is what actually occurs in the course of the reaction—how much product is actually
formed. Finally, the percent yield is the ratio of the actual yield to the theoretical yield, and you can
get this value using the following formula:
Going back to our last example, the 28,116 grams you calculated would be the theoretical yield.
But what would the percent yield be if you performed this reaction and you actually collected 26,450
grams of ammonia? You would calculate it using the above formula. Here it is with the numbers
plugged in:
Practice Questions
1.
How many moles of hydrogen sulfide are contained in a 35.0 g sample of this gas?
(A)
1.03 mol
(B)
2.06 mol
(C)
6.18 mol
(D)
9.45 mol
(E)
11.3 mol
2.
What is the molar mass of ethanol (C
H
OH)?
2
5
(A)
34.2
(B)
38.9
(C)
46.1
(D)
45.1
(E)
62.1
3.
Ammonia can be produced by the reaction of nitrogen and hydrogen gas. Suppose the reaction is
carried out starting with 14 g of nitrogen and 15 g of hydrogen. How many grams of ammonia can be
produced?
(A)
17.04 g
(B)
34.08 g
(C)
51.1 g
(D)
85.2 g
(E)
102 g
4.
How many atoms of hydrogen are present in 12.0 g of water?
(A)
2 3
1.1
10
(B)
2 3
2.0
10
(C)
2 3
4.0
10
(D)
2 3
8.0
10
(E)
2 4
4.8
10
5.
Which compound contains the highest percent by mass of hydrogen?
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