NAME~
~
PERIOD:
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HOMEWORK 9,2
a. Review your notes.
b. Answer the following:
1. Citric acid, H3C6Hs07, is a product of the fermentation of sucrose, C12H22011in air:
C12H2201J(aq)
+ 302 (g)
-+
2H3C6Hs07 (aq)
+ 3H20 (1)
Determine the mass (g) of citric acid produced when 2.50 moles of sucrose is used.
3
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Cc. 1-1
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s:
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SO ""~
1-2
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o?w·~ I~3 (;-::."...:..-1-I=.5
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L{_.3~/-J....,,3•••.C_&_!-I_S_()7
/ h1 ~ 1-13 C, I-/s 07
[c/{".l1
%0.7 =
z:
0"
2. A solution of potassium chromate reacts with a solution of lead (II) nitrate to produce a yellow precipitate oflead
(II) chromate and a solution of potassium nitrate:
K2Cr04 (aq) + Pb(N03)2 (aq) ~ PbCr04 (s) + 2KN03 (aq)
Determine the mass (g) ofPbCr04
produced when 0.250 moles K2Cr04 reacts.
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j
PbCrO~ ::
I(,-C~ ~J_.IVM~~b
I
....
{ Irv\l~ I()
co. I J~ 3. ~OfJ PhC,.O<-!
C~O-;JII1I~~b co,
- [80.? J J
3. One in a series of reactions that inflate air bags in automobiles is the decomposition of sodium azide, NaN3:
2NaN3 (8) .....•2Na (s) + 3Nz (g)
Determine the mass (g) of N, produced if 100.Omoles of Nal-l, decomposes.
z:
4. In the formation of acid rain, sulfur dioxide reacts with oxygen and water in the air to form sulfuric acid:
2S02 (g) + 02 (g) + H20 (1)
-+
2H2S04 (aq)
Determine the mass (g) of sulfuric acid formed when 2.50 moles of sulfur dioxide react.
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HJ so;
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9~, 0 ~ !j l-t saC(
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