test 4 handouts
TRANSCRIPT
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BALANCING
CHEMICALEQUATIONS
Name
Rewrite
and
balance
the
equations
below.
. N
2
+ H
2
NH,
2. KCIO, KCI + C X
3. NaCI + F
2
-* NaF +CI
2
4.
H
2
+ O
2
H
2
O
5. AgNO
3
+ MgCI
2
AgCI+ Mg(NO
3
)
2
6.
AIBr
3
+
KjSO,
KBr + A I
2
(SO
4
)
3
7. CH,
+
O
2
-* CO
2
+
H
2
O
8.
C
3
H
8
+ O
2
-*
CO
2
+
H
2
O.
9. C
8
H
18 +
0
2
10
2
+H
2
0
10. FeCL
+ NaOH
Fe(OH)
3
+
NaCI.
11.
P+
O,
12. Na +
H
2
O
NaOH +
13.
Ag
2
O
-
Ag
+
O
2
14. S
8
+0
2
- S0
3
.
O A. 0
15. C0
2
+
H
2
0
0
16. K
+ MgBr
2
17,
HCI + CaCO,
KBr + Mg
CaCI
2
+ H
2
O +CO
2
.
Chemistry IF8766
58
Instructional
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EQUATIONS
Name
theword
equations
belowaschemical equationsandbalance.
zinc
+
lead(II) nitrate yield
zinc
nitrate
+
lead
2
aluminumbromide +chlorine yield aluminum chloride +bromine
3 ,
sodiumphosphate
+
calcium chlorideyieldcalcium phosphate
+
sodium
chloride
4. potassiumchloratewhenheatedyields potassiumchloride + oxygen gas
5 . aluminum
+
hydrochloricacidyield aluminum chloride
+
hydrogen
gas
6 .
calcium hydroxide
+
phosphoricacid yieldcalciumphosphate
+
water
7 .
copper
+ sulfuricacid
yield copper (II)sulfate
+
water
+
sulfur dioxide
8 .
hydrogen +nitrogen monoxide yield water + nitrogen
i
nc
Chemistry IF8766
59 Instructional
Fa i r ,
in
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TYPES OF REACTIONS
Thereare 5main typesofreactions.
1. Direct CombinationCompositionSynthesis:
Two ormore elements orcompounds A and B)combine toforma
more complex substance. ABoneproduct)
A + B AB
Examples:
Write equationsshowing
the
direct combination
of the
elements below:
a. Sodium
and
iodine
b. calciumandoxygen
c. hydrogen and chlorine
d.
hydrogen
and
carbon monoxide
and
oxygen
to
form carbonic
acid
e. nitrogenandhydrogentoform ammonia
2. DecompositionAnalysis:
^ Reverse
of
direct combination.
A
complex compound
ABone
reactant)
isbroken down intotwo ormore simpler substances.
Aand B,elements and/or compounds)
AB *
A + B
Examples: Write equations showing
the
decomposition
of
each
of
the
following substances:
a. Water
b. silver chloride
c.
aluminum oxide
d. lithium phosphate to form
lithium,
phosphorous and oxygen
e.
sulfuric acid to form hydrogen, sulfur and oxygen
3. Single Replacement:
Onesubstance isreplaced from-itscompound byanother
substance.
Element + compound -^ element + compound
A + BC
*
B + AC
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Note: Cationic single
replacement: is
when metals replace
metals andhydrogen. +ion)
AnionicSingle replacement: is when nonmetals replace
nonmetals.
-
ion)
To see if a
reaction takes place
use
Table
J. A
more active
metal replacesaless active metalor amore active nonmetal
replaces
a
less active nonmetal.
If
this
is not the
case
a
reaction will not occur.
Examples: Decideif thefollowing reactions will occur. If
they
dotake place determinetheproductsofeach reaction.
a.
zinc and nitric
acid
b. iron andcopper IIsulfate
c. sodium and water
d. magnesium chlorideandfluorine
e. sodium chloride and bromine
4. Double Replacement:
Twocompounds combine toformtwo newcompounds.
AB + CD
*
AD + CB
Note: +
ions switch places.
These equations are also known as ionic equations. Ionic
equations have
two
possibilities:
a. Reactions go to completion stops): When ions in a solution
combine to form a productthatleaves the scene of a
reaction. There are three types of products that leave the
scene of a
reaction.
1. Slightlyionizedwater
2.
Gases escape Cf)
3. Precipitates settle
to the
bottom 4*)
Precipitates are solid substances formed by a physical
orchemical change in a liquid medium. It separates
from the liquid by settling to thebottom.Precipitates
are insoluble compounds see table F.
b. If a reaction does not go to completion they are said to be
Reversible. 5). Areversible reactionis one inwhichthe
products can themselves react to form the reactants.
Examples: For each reaction write themolecular,ionic and
Netionic equations:
a. silver nitrateandzinc chloride
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b.
copper
IIhydroxideandacetic acid
c.
iron II
sulfate
andammonium sulfide
5. Complete Combustion:
When
a
hydrocarbon compound composed
of
onlycarbon
and
hydrogen) or acarbohydrate compound composed ofcarbon,
hydrogen andoxygen) react with oxygentoform carbon dioxide
andwater.
Example: Write anequationfor thecomplete combustion ofeach
ofthe
following
organic substances:
a.
b. CH
4
c
C
2
H
2
d.
C
6
Hi
2
0
6
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Name
Date
Class
CHAPTERS REVIEW
ACTIVITY
TtxtReferenct:Section-13
Chemical Changes
Choose word*fromtrwlistto fill In the blanks in the paragraphs.
WordUat
analysis
arrow
chemical equation
chemicalreaction
coefficient
delta
doublereplacement
electrolysis
endothermic
exothermic
ionic equation
precipitate
product
reactant
single
replacement
spectator
synthesis
Another name for a chemical change is
a(n)
LD Such a change can
be
represented
by means of a written statement called a(n)
(
2
)
. The
symbol
for the
word yields
in
such
a
statement
is
a(n) GD
Any
substancewrittento the leftof thissymboliscalled
a(n)
.
W
_ .Any
substancewritten to the right ofthis
symbolis
called
a(n)
GJ) A
number written
just
to the
left
of a formula is called a(n)
()
A
chemjMf
changeinwhich energy is absorbed is called a(n) (?)
reaction.
One in which energy is released iscalled a(n) (8) reaction.
Some chemical
changes
involve charged particles. Anequation that
showsthe
reaction
or
production
of
such
paniclesis
called
a(n)
C O
.
Any
charged
particle
that
is
present
but that
does
not change or react
during areaction isusually omitted from theequation; it iscalled
a(n)
(IP)
A
chemical change
in
which
two or
more substances combine
to form
a more complex substance is called a(n) (H) reaction. A change in
which
asubstanceisbroken down into
simpler
substancesiscalleda(n)
(12) reaction.Any such change that is caused by the flow of anelectric
current is called a(n) (13) . If the change iscausedby heat supplied to
the reaction, the Greek symbol
(H) isoften
written above the yields
symbol
in the
equation.
A chemical change
in
which
a
free
element replaces and releases
another
element
in acompoundiscalleda(n) (15) reaction. Achemical
change inwhich there isanexchangeofions betweentw ocompoundsis
called
a(n)
(*6) reaction. Asolid substance producedbysucha reac-
tion
inaliquid
medium
is
called a(n)
(
17
) .
1.
2.
3.
4.
5.
.
7.
g.
9.
10.
11.
12.
13.
14.
IS.
16.
17.
9 4 CHEMIST1Y:
Th
StudyofMattar
COPYRIGHTbyPrtotic*Hall,Inc
Reproductionofthil matter u
rvttrkltd
toduplicationfixd*uroomUM only.
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Name
Date
Class
CHAPTERS
REVIEW ACTIVITY
Text Reference:Section9-12
Categories of Chemical Reactions
State whether each of thefollowingequations represents a synthesis
i),analysis a),single replacement sr),
or
doublereplacement dr)
reaction.
1.
CO
2
-*
C +
O,
1.
2.
NaCl
+ AgNOa
-
NaNO,+
AgCl
2.
8. S + CU
-+
SCU 3.
4.
BaClt
+
2NaOH
-*
2NaCl
+
BaTOH),
4.
5.
Zn
+
CuSO
4
-*ZnSO
4
+ Cu 5.
6.
CH*
-*
C +
2H
2
6.
7.
PbCNO,)s
+
Mg-*Pb
+
MgCNOsk
7.
8.
Mg
+
2HC1- MgCU
+
Hi
8.
9. HjSO
4
-*
H
2
+S +20
2
9.
10.
2Oj+
N
s
-*N
A 10.
11.
3CaBr
2
+ 2Na
s
P-
Ca
s
ft +
6NaBr
11.
12. 2KI
-l - Br
2
-2KBr
+
I
2
12.
18.
CflHtfO,,
- 6C +
6HzO
13.
14.
2NaF
- 2N a+ R 14.
15.
Si +
O
2
-
SiO
2
15.
16. 2NaI -t -
Pb(NO
8
)2
-2NaNO
3
- f Pb I
2
16.
17.
N al+ Cs-*
Csl
+ Na
17.
18. H
2
+ CO
+O
2
-
H
2
CO
3
18.
19. LJaPO
4
-3Li
+
P + 2O
2
19.
20. CSz +
2FJ
-
CF
4
+ 2S 20.
J
COPYRIGHT
by Prtntic*
Hll.
Inc.
Rtproduction of
thu
mrtr
(rttridd
to duplication for
eUwoom
UM
only.
CHEMISTRY:ThStudyofMatter 9 3
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CLASSIFICATIONOF
Nome
CHEMICAL REACTIONS
Classify
thereactions belowas
synthesis,
decomposition,singlereplacement
(cationic
anionic) or
double
replacement,
2H
2
+
O
2
- 2H
2
O
2. 2H
2
O - 2H
2
+ O
2
3.
Zn +
H,SO,
ZnSO. + H
2 4
2
4. 2CO
O
2
- 2CO
2
5.
2HgO -*
2Hg
O
2
6. 2KBr + CI
2
- 2KCI +
Br
2
7.
CaO + H
2
O
-
Ca(OH)
2
8. AgNO
3
+ NaCI
AgCI
+ NaNO
3
9. 2H
2
O
2
2H
2
O +
O
2
10.
Ca(OH),
+ H
2
SO
4
~- CaSO,, 2H,O
'H .
:
, t r, '8766
50 Inotfjctionai
f f j i f . m
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Name
predict
theproductsof thereactions below. Then, writethe
balanced
equationand
c l a s s i f y
the reaction.
^
magnesium
bromide
chlorine
2 aluminum + iron (III) oxide
3 .
silvernitrate + zinc chloride
PREDICTING
PRODUCTS
CHEMICAL REACTIONS
4 hydrogen peroxide (catalyzed by manganese dioxide)
5 zinc
hydrochloricacid
6
sulfuricacid
+
sodium hydroxide
sodium
+
hydrogen
Qceticacid + copper
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PROBLEMS
INVOLVING EQUATIONS
The
coefficients used
in
balancing
a
chemical equation
represent
moles.
Instoichiometric problems involving
equations it isassumed thatthereactionis the single
reaction
with
noside reactions),thatthereaction goes
tocompletion
and the
reactants
are
completely reacted.
Every stoichiometric problem involvesthefollowing
three basic
steps.
Stepl: Find
the
moles
of the
substance
you are
given
information
about.
Moles
=
g/gfm Moles=1/22.4 Moles
= ftp/6.02 x
10
23
Step 2: Set up amole ratio.
Actual moles from step1) = Actual moles
unknown)
Theoretical moles fromcoefficients)Theoretical moles
Step 3: Find
the
grams, liters
or
particles
of
your
unknownusingone of thethree mole equations from step1.
Type 1: Mass-Mass Problems:
A
balanced equationshows
the
moleproportions
of
products
f toreactants. It ispossibletodeterminethemassof one
substance that reacts withor isproduced fromagiven mass
of
another substance.
Examples:
1.
How
many grams
of
sodium chloride
are
needed
to
react
toproduce 35.5 gramsofchlorinegas?
2. How manygramsofhydrogenareproduced by theaction
ofwateron 100.gramsofsodium?
3.
What massof
oxygen
will combinewith3. 0
grams
of
hydrogen
to
produce water?
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4.
Given
the
reaction:
N
2
+
0
2
-
2NO. What
is the
total
number
of
grams
of
oxygen needed
to
react completely
with
2. 0
moles
of
nitrogen?
Type 2: Mass-Volume
Problems:
A
mole 6.02
X 10 ) of
molecules
of any gas
occupies
a
volume
of22.4 litersat STP. This numerical valueis
called themolarvolume. It has amass equalto the
molecular mass expressed in
grams.
In abalanced equation
where
the
mole unit serves
to
relate
the
quantities
of
products andreactants,it ispossibletodetermine
quantitative
resultsindesired units, whichmay not
necessarily
be the
same
as the
original units.
Examples:
1. Howmany gramsofzinc metalareneededtoreact with
hydrochloric acidtoproduce 11.2 litersofhydrogen
gas at
STP.
2. Howmany gramsofcarbon dioxideat STP are produced
by the
complete combustion
of C
2
H
e
?
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Type 3: Volume- Volume Problems:
Since
one
mole
of any gas
occupies
the
samevolume
as one
mole of any other gas, at the same temperature and
pressure,
the
volumes
of
gases involved
in a
reaction
are
proportional to the number of moles indicated by the
numerical coefficients in a balanced equation.
Examples:
1. In the
reaction N
2
+
H
2
->
2NH
3;
calculate
the
volume
of
hydrogen
gasrequired toform100. litersofammonia?
2. What volume of carbon dioxide will beformed fromthe
complete combustion of 21.2 liters of camphene Ci
0
H
6
)?
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STOICHIOMETRY:
MOLE-MOLE
PROBLEMS
Name
4.
N
2
+ 3H
2
-* 2NH
3
Howmany moles
of
hydrogen
are
needed
to
completely react with
twomoles
of
nitrogen?
2. 2KCIO,
2 K C I +
3O,
Howmanymoles of oxygen areproducedbythe'decompositionof sixmoles
ofpotassium chlorate?
3. Zn + 2HCI -
ZnCI
2
+ H
2
Howmany molesofhydrogenareproducedfromthereactionofthree moles
ofzincwithan
excess
ofhydrochloric acid?
C
3
H
5CL
3C0
4H
2
0
. _ 2 2
Howmany
molesof
oxygen
are
necessary
to
react completely with fourmoles
of
propane(C
3
H
8
)?
5.
K
3
P0
4
+
AI(N0
3
)
3
-*
3KN0
3
+
AIPO
4
Howmanymolesofpotassium nitrateareproduced whentwomolesofpotassium
phosphate
react withtwomolesofaluminum nitrate?
Chemistry IF8766
62
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STOICHIOMETRY:
MASS-MASS PROBLEMS
Name
1 .
2KCIO,
2KCI
+ 3O
0
Howmany gramsofpotassium chlorideareproducedif 25 g ofpotassium chlorate
decompose?
2.
N
2
+
3H
2
- 2NH
3
Howmany
grams
ofhydrogenarenecessary toreact completelywith50.0g of
nitrogenintheabove reaction?
3.
How
manygrams
of
ammonia
are
produced
in the
reaction
in
Problem
2?
4. 2AgN0
3
+ BaCI
2
- 2AgCI + Ba(NO
3
)
2
How
many grams
of
silver chloride
are
produced
from5.0 g ofsilver
nitratereacting
withanexcess ofbarium chloride?
5. How much barium chlorideis necessary to reactwiththe silver nitratein Problem4?
Chemistry
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5TOICHIOMETRY:
VOLUME VOLUME PROBLEMS
Name
N, + 3 H
2
2NH,
What
volume
ofhydrogenis
necessary
toreact with fiveliters ofnitrogentoproduce
ammonia?
(Assume
constant temperatureandpressure.)
2.
What volume of ammonia is produced in the reactionin Problem1?
3. C
3
H
8
+50
2
3CO
4H
2
O
If
20
liters
o f oxygena re consumedin the above reaction,how many
liters
of carbon
dioxide are produced?
4. 2H
2
0 2H
2
+0
2
If
30ml ofhydrogenareproducedin theabove reaction,howmanymilliliters of
oxygen are
produced?
5.
2CO + O
2
-* 2CO
2
How
many liters of carbon dioxidea re produced if 75 liters of carbon monoxide
a re
burned
in
oxygen?
How
many
liters
of
oxygen
a re necessary?
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I
STOICHIOMETRY:
MASS-MASS PROBLEMS
Name
\
1. 2KCIO,
2KCI + 3CX
How
many
gramsofpotassium
chloride
are
produced
if 25 g of
potassium chlorate
decompose?
2. N
2
+
3H
2
- 2NH
3
How
many
gramsof
hydrogen
arenecessaryto
react completelywith50.0
g of
nitrogen
inthe
above reaction?
3.
How
manygrams
of
ammonia
are
produced
in the
reaction
in
Problem
2?
Ba(NO
3
)
2
.
2AgNO
3
+
BaCI
2
-
2AgCI
How
many
grams
ofsilver
chloride
are
produced
from5.0 g ofsilvernitrate
reacting
with
anexcessof
barium chloride?
5.
How
much barium chloride
is
necessary
to
react with
the
silvernitrate
in
Problem
4?
Chemistry
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STOICHIOMETRY:
Name
VOLUME VOLUME PROBLEMS
1. N
2
+ 3H
2
- 2NH
3
Whatvolume
of
hydrogen
is
necessa ry
to
react withfive liters
of
nitrogen
to
produce
ammonia?
(Assume
constant temperatureandpressure.)
2.
What volume
of
ammonia
is
produced
in the
reaction
in
Problem1
?
3.
C
3
H
8
+ 5O
2
- 3CO
2
+ 4H
2
O
If20liters ofoxygenareconsumedin theabovereaction,howmanyliters ofcarbon
dioxide are produced?
4. 2H
2
0
2H
2
+0
2
If
30
mL
of
hydrogen
are
produced
in the
above reaction,
how
manymilliiiters
of
oxygen
are
produced?
5.
2CO + O
2
->
2CO
2
Howmany liters ofcarbon dioxideareproducedif 75
liters
ofcarbon monoxide
are
burned
in
oxygen?
How
many
liters
of
oxygen
arenecessary?
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llOICHIOMETRY:
MIXED PROBLEMS
Name
N
2
+ 3H
2
- 2NH
3
What
volume
of
NH
3
at
STP
is
produced
if
25.0
g of
N
2
is
reacted with
an
excess
ofH,?
2.
2KCIO
3
-* 2KCI
+
3O
2
If5.0 g ofKCIO
3
isdecomposed, what volumeof O
2
isproducedat STP?
3, Howmany gramsof
KCI
areproducedinProblem2?
4. Zn +
2HCI -
ZnCI
2
+
H
2
What
volumeofhydrogenat
STP
isproduced when2.5
g
of zincreact withan
excessofhydrochloric acid?
5.
H
2
SO
4
+ 2NaOH
-* H
2
O
+
Na
2
SO
4
How
many moleculesof water areproducedif 2.0 g ofsodiumsulfate are
produced
in the
abovereaction?
6.
2AICI
3
-
2AI +
3CI2
If
10.0
g ofaluminum chloridearedecomposed,howmany moleculesof CI
2
are
produced?
w
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STOICHIOMETRY:
LIMITING
REAGENT
Name
f onaj -fopfc)
. N
2
3 H
2
2NH,
Howmany
gramsofNH
3
can be
produced
fromthereactionof 28 g of
N
and
25g ofH
2
?
2. Howmuchof the excess
reagent
in
Problem
1 s
eft over?
3.
Mg +
2HCI
-
MgCI
2
+
H
2
What volume
of
hydrogen
at STP isproduced
from
the
reaction
of
50.0
g of M
theequivalentof 75 g of HCI?
4. How much of the excess reagent in Problem3 is leftover?
5. 3AgNO
3
+
Na
3
PO
4
-
Ag
3
P O
4
+ 3NaNO
3
Silvernitrate and sodium phosphate arereactedinequalamounts of 200. g
ea
How
manygrams
of
silver phosphate
are
produced?
6.
How
much
of the excess
reagent
in
Problem
5 is
eft?
ChemistryIF8766
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N a m e
IL
Class
Mass-Mass Problems
Solving
mass-mass
p roblems usual ly involves these steps:
1.
Convertgiven masses in gramsto moles.
2.
U se coefficients in the balanc ed equ ation to establish mo le
ratios
between
the substances involved in the problem.
3.
Calculate th e numb er of moles of the required substance.
4. Convert
that
number of moles to mass in grams.
Examples
How many moles
of
F
2
are
there
in
60.0s
o fF,?
(F
= 19.0
g/mole)
mole
mass
of F
2
= 2 x 19.0
g/mole
= 38.0
g/mole
60.0 g
38.0
g/mole
=
1.58 moles
In the
followingreaction,
ho w
many moles
of F
2
are
needed
to
produce 1.5
moles
of HF?
H
2
2HF
mole ratio ofF
2
to HF = 12
1:2= ?:1.5 ? = .75
How many grams of HF is .75 moles of HF? (H = 1.0 g/mole)
mole mass of HF = 1.0 g/mole + 19.0g/mole= 20g/mole
.75 moles x 20g/mole= 15 g
c
o
I Solve the
following problems. Show
your
work.
| 1.
Given
the
equat ion
N
2
(g)+
3H
2
(g)-
2N H
3
(g)
answerthe
fol-
lowing questions.
a. How many moles of N
2
are there in 200 g ofN,?
(N
= 14.0
g/mole)
la.
Date
o
b.
H ow
many moles
of
NH
3
could
be
produced
from the
above amount
of
N
2
?
c.
How many grams ofNH
3
would
this
be?
(H =
1.00 g/mole)
c.
11-3
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8/10/2019 Test 4 Handouts
21/23
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8/10/2019 Test 4 Handouts
22/23
Name
Class
Volume-Volumeand Mass-Volume Problems
Date
Volume-volume problems involve direct comparisonof the
coef-
ficients
in abalanced
equation.
The
reason
is
that equal volumes
of gases at the same temperature and pressure contain equal
numbers of moles and molecules. Also involved is thefactthat at
STP the volumeof a gas isequalto22.4L /mole.Calculationof
numbers
of
molecules involves
the use of Avogadro's
number,
6.02 x
10
23
molecules/mole.
Examples
Howmanylitersof HC1 gas can beproducedfrom 10 L ofC1
2
gas
by the reaction H
2
+C1
2
-*2HC1?
1:2=
10L:?L
? = 20 L
Howmany gramsofhydrogen gas (H
2
) areneeded toproduce
5.00
L ofwater vapor, measuredatSTP, accordingto the reac-
tion
2H
2
+O
2
-2H
2
O? (H = 1.00 g/mole; O = 16.0g/mole)
5.00
L
=.223 molesof
H
2
O
vapor
22.4
L/mole
2:2
= ?
moles
H
2
:.223
molesH
2
0
? =
.223 molesH
2
.223
moles
x
2.00g/mole
=
.446
g
H
2
Howmany H
2
molecules aretherein .223 molesof H
2
atSTP?
.223
moles
x
6.02
x
10
23
molecules/mole
= 1.34 x
io
23
molecules H
2
Solve
thefollowing problems. Show yourwork
1. Howmany
liters
of
CO
2
can beproduced
from
14.5L of C
2
H
2
by
the reaction
2C
2
H
2
(g)
+
50
2
(g)
-
4C0
2
(g) +
2H
2
0(g)
2. Howmanylitersofoxygenarereleased
from
thedecomposi-
tionof 3.6 L of hydrogen peroxide gas
(H
2
O
2
)
to produce
water vaporandoxygen? (Writethe
balanced
equation for
the
reaction
as
part
of
your work.)
2H
2
0
2
(g)-+2H
2
0(g) +0
2
(g)
2.
< ~ H F M T S T R Y
Review Activity
11 5
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8/10/2019 Test 4 Handouts
23/23
Name
Class
Volume-Volumeand
Mass-Volume
Problems Continued)
3. How many grams of zinc (Zn = 65.4g/mole) arerequired to
produce
67.2
L of
hydrogen
gas at
STP, according
to the reac-
tion
2HCl-ZnCl
2
+
H
7
3.
Date
4. a. How manyliters of
C1
2
gas
at STP can be produced by
decomposing 70.0g of HC1
gas?
(H = 1.00 g/mole;
Cl
=
35.5g/mole) (Includeabalanced equa tioninyour work.)
4a.
b. How many
C1
2
molecules would be produced?
5. How many liters of H
2
O vapor could be produced by the
reaction
of
9.03
x
10
23
m olecules
of
O
2
,according
to the re-
action
2H
2
(g)
+
0
2
(g)
-*
2H
2
0(g)