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Honors Chemistry: Chapter 9 Stoichiometry Problem Set
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Directions: Solve each of the following problems. Show work using the factor label method or the irf box. Include correct
units and significant figures with each answer. Clearly indicate final answer. Be sure to start with a balanced equation
Part 1: Straight Stoichiometry Problems
Target Goal: Calculate amounts of
reactants and products in a reaction.
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1.) For the reaction
HN03(aq) + _Mg(OH)2(S) ~ _Mg(N03)2(aq)
nitrate are produced from 8.00 mol of nitric acid (HN03)?
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2.) For the reaction
KCI03(s) ~
produce 160. g of oxygen?
Ib{).,()2.
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2...
01..
3
02(g),how marE,.~~le'
2.~/(a/)..
~
'3 ~
02-
f1j(III~)2-
J, !J(M!J)1..
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KCI(s)+
+ ~ H20(I), how many grams of magnesium
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potassium chlorate are required to
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3.) For the reaction 2H2(g)+ 02(g)~ 2H20(g), how many grams of water are produces from 5.22 liters of oxygen gas?
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4.) In the reaction
Na(s) +
H20(g) ~
1.33 grams of sodium react completely?
2.
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NaOH(aq)+ _H2(g),
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6.) _C~(g)
+
02(g)~ ~ H20(g) + _C02(g)
what is the mass of water that is produced?
how many grams of hydrogen are produced if
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When 1000. grams of methane react with an excess of oxygen,
7.) In the reaction _C02(g)
+ _H20(g)
~ _H2C03(aq),
of water to produce 640. grams of carbonic acid?
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.
9.)
g- 02(g) -7~S02(g)
1:...
H2S(g)+
02(g)~ ~ S02(g) +
H20(g)
liters of oxygen gas are reacted at STP.
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Calculate the mass of dihydrogen monosulfide required when 15
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Calculate the liters (at STP) of O2 needed when 128 liters of S02 are formed.
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+
8.) _S8(s)
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how many grams .•of carbon dioxide react with an excess
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Calculate the moles of NaCI formed when 5.40 moles of Na are reacted.
11.)_TiCI4(s) +
are reacted.
2
b.: c19 -ry 10X
(J.
+ _02(g)
2i?
~
1"
13.)_P4(S)
+
5H2(g)~
_P~lO(g)
-_
bf.739J1fij
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Calculate the volume ofH2 required at STP when 0.920 moles of P4 are reacted.
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Calculate the mass of Na required when 0.347 moles of Na20 are formed.
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Calculate the mass of HCI formed when 6.097 g of IJ20
~/_~_II,.~
Na20(s)
AI~ () x
_~~f
t HCI(aq)
le~lt0
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12.).,fNa(s)
+
H20(l) ~ _Ti02(s)
Did you achieve our target goal?
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+:+ Target Goal: Calculate amounts of reactants and products in a reaction.
1
Feeling VERY confused
2
Not sure that I get this
3
I think I am catching on I
4
Doing great! Bring it on!
Part 2: Limiting Reactant and Percent Yield
.:. Target Goal: Determine the limiting reactant in a reaction .
•:. Target Goal: Calculate excess and amounts of products in a limiting reactant problem .
•:. Target Goal: Calculate percent yield of a product.
1.) One of the steps in the commercial process for converting ammonia to nitric acid involved the conversion of NH3
to",NO. In a ce,uain exper~ent 22.59 g of NH3 reacts with 28.5 grams of O2
tf-NH3(g) + .., 02(g)-7 ~NO(g) + b...H20(g)
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0
2 1.50;,1.
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II.
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a.' What is the limiting reactant?
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b.
How many liters of NO will form at STP?
c.
How many grams of the excessreagent
d.
What is the % yield of the reaction if 16.0 grams of water is recovered?
will be left at the end oftbe reaction?
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2.) 105 grams of beryllium selenate and 197 grams of gold react as in this equation:
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g
a.
What is the limiting reactant? __
b.
How many moles of gold (I) selenate are produced?
c.
How many grams of non-limiting reactant are left over?
d.
If the percent yield of the reaction is 88%, how many grams of beryllium metal are collected in this lab?
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b.
c.
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How many liters at STP of the non-limiting reactant are leftover?
d.
a.
How many moles of magnesium chloride can be expected from this reaction?
b.
How many grams of excess reagent are left over?
c.
If 1470 grams of magnesium chloride is rec~
what is the percent yield of the reaction?
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Did you achieve our target goals?
.:. Target Goal: Determine the limiting reactant
in d reaction .
•:. Target Goal: Calculate
excess and amounts of products in a limiting reactant
•:. Target Goal: Calculate
percent yield of a product.
1
Feeling very confused
2
Not sure that I get this
3
I think I am catching on
problem .
4
Doing great! Bring it on!