,
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Date
Class
_
Text Reference: Section 8-10
CHAPTER 8
Practice Problems
1. What is the mass of 7.50 moles of sulfur
dioxide (S02)?
(8 = 32.1 g/mol; 0 = 16.0 g/mol) ~
17. What is the percentage c0II!.~~~"
dinitrogen tetroxide (N20J?
(N = 14.0 g/mol; 0 = 16.0g/mol)
70""/00
TlfW
.
What is the percentage composition of a 43 010 G
carbon-oxygen compound, given that a 95.2-g
sample of the compound contains 40.8 g of carbon ~7 /1 0
and 54.4 g of oxygen?
19. What is the percentage composition of "
. suIfur-chlorine compound, given that a 30.~ Jl ~/4 ..5
sampleofthec~~poundisf~undtocontain9.93
,.q.<lj. 1/"
. of sulfur and -21.;5 g of chlorine? '
'. lY.
~ l
20.' A sample ora compoundthat has-a mass :_ :
'of 0.432 g is analyzed. The sample is found to be'
made up of oxygen and fluorine only. Given that
b
the samplecontainsO.128
g of oxygen, calculate 30%0
the percen
e com osition of the com ound.
2. What is the mass of 0.438 mole of ammonium chloride (NILCI)?
~
(N = 14.0 g/mol; H = 1.Qg/mol~5
g/mol)
r3) How many moles are there in 250.0 g of
sodi~ phosphate (Na;?04)?
.
(Na = 23.0 g/mol; P = 311~Ql;
\
.0.::;: 16;O.g/mol) ..
,·U5j>-tfV\i)\e
.", ..'
-'~'. 4. How many 'rnoies are th~re in 993. g of
: .c-:,:.: -potassiurrt.sulfate (KiS04)?
5./0 I me Ie: .
(K
39.1 glmol; S = 32:1 g/mo;
= 16.0 g/mol)
How many atoms
. 3.00 moles
of sodium (Na)?
1.1.1 'f.. m;!~oll>vy)~
th·
1 638 x
6 H·ow rnanyoms
are
ere ill .
10-9 mole of lithium (Li)? 1-q.<6101 'f-.. 1014 a\-vm ')\
0
70 ~ F
=
==-s.
.
e
2
Find the empirical formula of a compound, given that the compound is found to be
7. H.ow many ~olecules are there m 4.55
47.9% zinc (Zn) and 52.1% chlorine (CI) by mass. Zn tI;bJ
'" moles of rntrogen (N2).
,74 1-- ~()'4' V'(\o\q:,!!:,ks 1
(Zn = 65.4 g/mol; CI = 35.5 g/mol)
'.
~
•
~
How many atoms of rntro en (N are
22
Find th
- . al 4'
ula f
'---. th ~218
1
f (N-\?~
;L _.L.I
•
e empmc
rorm
0 a comere m.
mo es 0 rntrogen
2J.
. - ."'1 'f-.jl) i1jpNll; IVa.l
.poun d·,gIven th at a 48 .5-g samp Ie 0 fth e compoun' d~
f3
9. How many atoms are there m 0.663 molt:
is found to contain L75 g of carbon (C) and 46.75 g
t'-f
of water (H20)? ·1 \. 2.Cl 1- (010\- iHo)'y\..S
of bromine. (Br).
.
10. How many moles are there in 15.5 x
(C~- 2.0 g/mol; Br = 79.9 g/mol)
1()23molecules of carbon dioxide (C02)? ;/",'57 me I]
23
What is the empirical formula of a com11. How many moles are there in .32 x -1l.
d, given that a 212.1-g sample of the com-rc;tn} i .
12
-,.._.......,1;.;.0_
~lecules
of carbon tetrachloride (CCI4) ~.?b'~'fVJ\tpound contains 42.4 g .of hydrogen (II) and 169.7 g~
What is the volume occupi~
of carbon (C)? What 15 the molecular formula of
420 moles of oxygen gas (02) at STP? \""qrr.1 dlY\~
the compound, given that it has a gram molecular
L.
mass of 30.0 g/mol?
13. What volume does 0.0147 mole of rn
(H == 101 gl
l: C = 120 gl. I)
3
gen dioxide gas (N02) occupy at STP? .3Z.Qclm·
.'
mo,
.
mo
.
I
there
i
45
0
dm
3 f
.
24.
A
compound
is
known
to have a gram
14 . H ow many mo es are ere m.
0
I ul
f 391 5 I
L Find th
. . al
methane as (C~) measured at STP?~
mo ec ar mass 0
. g mo
e empmc ~
g
.
. ~3
.
and the molecular formulas of the compound,
15. How many moles are there m 0.335 dm
given the results of an analysis of a 310.8-g sample
3
==;;;;;;;o;;;;f::;;r~gon
gas (Ar) at STP?
i fO-:Z moll
that reveals that the sample contains only boron
- 16. Calculate the percentage composition of
. (B) and iodine (1). The mass of the iodine in the
lithium oxide (Li20).
L-t16 o )0 Li
sample is found to be 3022 g.
(Li = 6.94 g/mol; 0 = 16.0 g/mol)
,54: ~/D 0
(B
10.8 g/mol; I = 126.9 g/rnol)
L
)-----.1
_
l?
t
J
I
;>"
W
.
BI
lIso
=
.o
(oTn.po:::,H;0 ()
N\(1)~ k&"'1=;-
To\-J ,P&r~
A!:'.~::
W1~) =
%
Cr;fYI,p.
To
t~{cltmtJlt1
I t..{il't
/, .OA-Nutj~~~5
8-8
~
5
.
CHEMISTRY:The Study of Matter
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COPYRIGHTby Prentice Hall. Inc. ~'i ~
<t" rom fik-Y"l 1+ q.o 1M
Reproduction of this master is restricted to duplication 'for classroom use only.
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Date
. (f'vJs.)
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~131!Qa,
Class
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Converf- fo ufJlr tJft!~~~erence: Section 10-5
Practice Problems
1. Given the balanced chemical equation
10. Calculate the &plume) of chlorine gas
(Clz) that will be requiredat STP for complete
.
~r2 + 2NaI - ~N!\Br?7_L, .'reaction of 7.15 x 1()23atoms of iron (Fe) accord~1l-2J""l~
l~rr~RS'
.
how many moles of sodium bromide (.NaBrJcould
. ing to this balanced chemical equation: '2~'d
{Y!:
be produced from 0.172 mole of bromine (Br0?2Fe(s)
+ 3Clz(g) -+ 2Fe~(s) ~.
.
2. How many moles of oxygen (Oz)would be
~
needed to produce 79.60 moles of sulfur trioxide
11. Calculatethe~.Jof
mercury metal
(803) according to the follo~
balanced chem(Hg) that is required to produce 29.8 g of mercuieal equation?
"
ry(I) oxide (H~O) according to the following bal'.
anced chemical equation.
"
3,
.~":;;r15-----_~02
+
Oz-.
280
=~,~
._..
4H
(l)
+
0
(g)
2H
O()
;zi
~9c;.
H
A
.., .< GS
-=j·",\.vo.
'
g
z
-+
~ SUO
.:7. 'I;;.1/:1'-, 3. Calculate the~
occupied by 16.3
moles of nitrogen gas ~STP.
':J 1 (Hg = 200.6 g/mol; 0 = 16.0 glmol)
4. How many moles of fluorine gas
12. How ~
of water vapor (H20)
contained in a 0.269-ilm3container at STP? • .
will be produced wh~m1.18g o(hydrogen gas ~2)
. i eacts completely WIthoxygen gas (02) according
5• Assumin g.that th egasesare all at.STP.find
to th balan d ch . al
ti <)
~
f
nitro
dioxid
(NO
)
th
e
ceu cr enuc equa on.
th evo
2
at
I ume, 0 m gen OXl e gas
could be produced from 71.11dm3 of nitrogen gas
2Hig) + Oz(g) -+ 2HzO(g)? J O~~ ~ *TU
(Nz)acco~g·tothisbalancedchemicalequation.
(H = 1.01 g/mol; 0 = 16.0 g/mol)
'\4
I ,
-
<,
'.
Jf..a5
&~'i:ir€.
~~l-.,
?-:2-~~li~9"T202(g)
- 2NOz(g) ,' ... 13. WhatEl'!b~f
chlorine gas (C~). ~ea~
Assuming that the gases are all at the
sured at STP, can e produced by the decemsame temperature and pressure, what Milum&'of
~sition of 73.0 ~ of hydrogen chlo~de gas ~Cl~
oxygen difluoride gas (OFz) is needed to produce /:;:;;-.8lven the following balanced chemicalequation?
1.54 dm3 of hydrogen fluoride gas (HF) accordinf- '? J
2HCl(g) - H2(g) +CI2(g)
,: -z ~ i-."'lI ~ ~
to the following balanced chemical equation? Alif..!
1 \ • :::> J f d(,.t.I..l'1
.~'1o<rL{li= 1.01 glmol; Cl = 35.5 g/mol)
, . .'
'.
z
2
OFz(g) + 2H (g)- H 0(g) + 2HF(g) .
14. Find the number or[8raIn§Jof sulfus (8)
7. How many[fonnula uni!§ of calcium oxide
that is pr<>49,cedwhen 1.87dm3 of oxygen gas (02)
(CaO) can be produced from 4.9 x 105 molecules
at STP is also produced by the decomposition of
of oxygen gas (02) that react with ca1ciurn.!Ca) . sulfur trioxide gas (S03) according to this balaccording to this balanced chemical equation?
- anced chemical equation:
'3~~
6.
.J'-'
'0
dnr.
•
0 gA
Q
2Ca(s) + 02(g) -
2CaOes)
9 5X\ct~
R<>
\,JU'"
2803(g) -
8(s)
+ 302(g)
8. Aluminum metal (AI) reacts with sulfur ~ (8 = 32.1 glmol; 0 = 16.0 glmol)
(8) ~ produce alumin~ sulfide .(AIz83]acc~~/
\"'}
15. How many~rrnula uni§ of sodium chloto this balanced chemical equation: (D
&:0Jrde (Na~l) are produc~ by ~e reaction of 40.3 g
2Al(s) + 38(s) _ AlzSs(S)~'
OrY.~lv\ pf chlonne gas (Clz) WIth sodium metal (Na) ac~
_~
..\'" ;I"cording to this balanced chemical equation?
$1.
How many ~of
pletely with 1.33 x
aluminum will re
atoms of sulfur?
corn->:
1()24
9. Given the balanced chemical equation for
the decomposition ofphosphoros oxyfluoride gas
(POF3).
LJ
.41j?~3~t
-
p.(s)
+
20z(g)
+ 6~2~~ '5
what volume, !at STP, of fluorine gas (F0 co~d be
_ produced y the decomposition of 9.22 x 1()26
molecules of PhOSPhOrys-OxynUOtid~
.
10-6
'.
2Na(s) + C~(g) -
2NaCl(s)
t,~.2)'\'0. 23
.. , li~
"',(11--<\,>"-',-
(Na = 23.0 glmo!; CI = 35.5 glmol)
.
16. Given the balanced chemical equation
2Ag + Iz_ 2AgI
how many~of
silver metal (Ag) are required
to react comletely with 531.8 g of iodine (Iz) to
produce silver iodide (AgI)?
'1 5'1")
(Ag = 107.9 g/mol; 1= 126.9 g/mol) J-t. J.. ..,
x: \~.
5;lS-X: \~
CHEMISTRY:The Study of Matter"
--t"t~I(~"",:
-+ .)
"'COPYRIGHT by Prentice Hall.lnc.
Re~rQdl.lction of this master is restricted to duplication for dassroom
U$e
.
only.
,--'
_,'
~n~
cv •.
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