NAME:~
PERIOD:
UNIT 9 REVIEW PROBLEMS
1. Calculate the number of Os atoms in 0.5 15 moles of Os .
. 31
.s ht~ Os
J
2. Calculate the number of Se atoms in 1.17 moles of Se.
3. Calculate the number of moles in 6.70 x 1018 atoms of Cd.
4. Calculate the number of moles in 3.91 x 1028 atoms ofKr.
5. Calculate the mass (g) of .030 I moles of S.
'lo. 9~1
I
6. Calculate the mass (g) of2.93 moles ofTe.
I
7. Calculate the number of moles of Si in 71.5g of Si.
7/, 5J S",._· 4==/ h1._~_S_~;
__
I
;; f? 0 ~
S.,:
8. Calculate the number of moles ofCe in 9.35g ofCe.
I
It/O,/~
Ce
OVER
- [0. O~O
ht..lJ
9. Calculate the mass (g) of7.64 x 1025atoms of AI.
.J All{:::
7, c
~s
« '1-10 ~v
Al
JiVI,..! A ~
.;}fH.
~. 0 rJ. '/.10 .;)~14
I
9 gJ AI
III I WI,..! AI
s
I
la.
- _
l/rl
X(o! a.
10. Calculate the mass (g) of2.95 x 1019 atoms ofSi.
O),QS
SA.'
'f-IO''7jenv
s.
''''')
}
11. Calculate the number of atoms in 2.56g of Ho.
I
12. Calculate the number of atoms in O.361g of Ca.
Ct
,.3&(
=
I
Ilvtr/ ~
'10'O~
&.O~XIO
(l
/1Vlt!
~3
/J
Jp)~~
a.
13. Calculate the mass (g) of one atom of Gd.
3 «b« Gd
~/~~~~~C~d~J~~~~~~d~
__~_rl_S_71~~~~~Gq=
It.
z
d~ XIO&1~rw
~t!
14. Calculate the mass (g) of one atom of Y.
j~
"( =
15. Calculate the volume, in liters, occupied by 0.00320 mol of C02 at STP .
. 00.3 010
L
COO- ::
"",,.Q
CO d-.
I
16. Calculate the volume, in liters, occupied by 3.70 mol of N, at STP.
1~/,j
G~
j
-
17. Calculate the number of moles of 02 that will occupy a volume of8.40L at STP.
Irw..J OIA
18. Calculate the number of moles ofNH3 gas that will occupy a volume of 13.OL at STP.
I
19. Calculate the volume, in liters, occupied by 106.35g of Cl- at STP.
20. Calculate the volume, in liters, occupied by 4.54g of Ct) at STP.
21. Calculate the molar mass of (NH4hC204 to two decimal places.
rJ z
I-l z:
~ K. 0 )..
(L") 'l{ .0\:::
en
C=-C2-'\
() z:
r. 0 t
'iF, 0 ;
s:
d.<--(.o"J.
/(}..,O\::
;: rot/dO
1!.t.aO
(L()
22. Calculate the molar mass of Valium, C1sH!3ClN20
C .dlS) 1«,0 I: I~(), 1.5
14 = (1'31\ .f)\ ~ (3.13
C-l s: (\) s s. <.(.$: .3 S. 4 J
",-I s: (2..'\
0:. (I)
s:
to two decimal places.
l
d 7 d. 75
-1'..-e
J
g-. 0 L..
Ill. 0 \
~
~
I~,OO
s:
1f"O()
23. Calculate the percent composition OfCUS04 to two decimal places.
Cu.
::(I~ to
s=
o
r:
Cl)
3.
ss :
c 3,5S
s:
~3. s.s
(100):
I stj,f.. (
3d.O~
3~<(}iJ.:
(4) I (" 00
Iu ~
z:
"V·
I S9,
0 1>_
ro (
OVER
lo 0
& f{,
s:
(
O{)
s». & {
~
(100):
C(O. 1011
24. Calculate the percent composition of aspirin, C9Hg04 to two decimal places.
C=(4)t;).O(
~ fOf.o1
1-1 = (8) 1,01:
g, oj
0.- (l.( ')
I~, 00 .- ~ (I t
iso.
C.-
10
Iv
0
()
log,a,
Ie-O, 17
f-/:
(100)
lJ-; c)(5
/7
(
.:.
S9. C;9~
l/, ((
(Ioa).-
s%
0·/7
'ct, ()0
IfO./7
25. Calculate the percent Ba(OH)2 in Ba(OHk
i3ct
I 31 ~ 3 3
.: (I)
O~
I~.(QO
(2-)
I~"' (2.)
1-+tO ~
~
,.
o
I 3 -,.
33
(7/, 3 S
10 f3A.(OIl)J,.:
32.01)
s:
I
8H20 to two decimal places.
z:
,;). 0 ~
17/,3..5
/1.., 'f,
(8) ,8, 02...:-
(lfJo)
3(5.$1
l s~.
~
3I
._
10
1
I ,
31 5. S I
26. Calculate the percent Na2B407 in Na2B407
~(a..= (2..) J~.qq
t3
0=
= (t() 10, 61
s:
t.f 5. ~ t/
u..oo
»
l/d.OO
(1)
<90/,
1~t.O~((O)lf.OL=
a
C{
/0 NCt J
~ol,
0
O~ 7':
II
J;)
(,()C) \
3 fl. q ;J
s:
IS;;),
7c
~
J
J
of a compound containing arsenic and oxygen given the following
0=34.80%
4.{
& S . .1 0
0, ~
3Cf, G-O
-/~.
If
_
As = 65.20%
0',
fI)
do
27. Determine the empiricalformula
data:
.
7 t..(.
lOH20 to two decimal places.
Ifo.2..0
set.
As"
.
: tfS.qS
00
= ,g70
-
- ,;;.I ~
0
As
As:
-
I
::
.:
(~ )
s:
:J. I 6
~iO
A ~d 0
S'
:
]
~.S (J.) ~ S
28. Determine the empirical formula for monosodium glutamate (MSG), which has a composition of:
C=35.51%
3$. S
C:
J
Y,17
i:o
-I~.
0
6.
2...'9
/ J.
{g 0
o?O>,
'1 t?
::
s
. Sq'
Na
=
13.60%
:- y
A./
=1
tJ~
, sc, (
z
S
~. 37
::
N()..
N. 0'
".let ~
, S1'
No...
• S9 &..
::
z:
.c,
0
::
(.f. 7~
,\..I t\.
d.. 3 7
::
-
0:
I-J
,
3 7,8.5
0:
a. qlo
Net ~ • St) I
4.7;)
::-
N = 8.29%
0=37.85%
e.
,J,'1(,
:=
1~,O\
It :
H=4.77%
=- I
N,lA..
29. A compound is analyzed and found to have the following composition: 71.65% Cl,
27.27% C and 4.07% H. Its molar mass is 98.96 aJmo!.
C. ;(1)\';)..0\'::Determine its empirical formula.
C~~C)
Determine its molecular formula.
c, W,-/ CJ
J
C~
II. <0.5
CQ:
-::
.3 s. l{.£
on,
;L 7
C" 1;).,01
-:
;),0 ;)
rJ,C).7
::
-
::-
~. OJ-
/.0'
(I) S~.
q t ::
::-I
.;t. 0 ~
l/, 0 d
H
I.{, 0 I
I~.'
CJ:-
)
~.o-;).
l.o\:-
::-I
cl
c
Cl
a. ;l. 1
H =-(i>
I~.O)
Cl
z:
.;). a
~
0- -
CI-lz.CJ
f. FORn1
30. Caffeine has the following composition: 49.5% C, 5.1 % H, 28.9% Nand 16.5% O. Its molar mass is
195.0 g/mol.
s: (1.1)1:2,0\:.41f.o,!
c
C. 4 q..') ,J 2.... 0
Determine its empirical formula
Determine its molecular formUla~C ~
f
C,
<I
c.
q. S
::<..(.I~
'~.Ol
.$, I
H:
:
,.0\
DJi'.
c;
~:
/4. () I
0'
1(P,S
I~, 00
I
5.0.5
-~
-
;t,0(,
/.03
4.
0
:;
H
AI
z
0
S.dS
I.
0l
I ;)
=t.f
1.03
':
D
I~10 rJ <.t
H -:; (5)
D :,
::
S
0' =;)
-/.03
R>fl..rl{ :
c; 1-1s NLO
tJ~
(2.) Iq.OI=
0=
(,)1(,,00:0
S, O.s
~f.Od
)(P,OO
97.1/
I
qS
•...
X -: 97. II
'
~
.:J.
0
=I
()
OVER
E.
\
I. 0 I::.
11'1 ,R)(LWl
'
C! I~,o "'4 OJ-
31. Ibuprofen is a common headache remedy. Its percent composition is 75.7% C, 8.80% Hand 15.5% O.
Its molar mass is 206.0 glmo\.
L s: (13/ Id.O\ t: ISl>,t3
Determine its empirical formula. C\3 ~I 8 () ;)..
Ii z: (, if ') /. 0 I z: I~,
/8
Determine its molecular formula. C.13
c:
,s, I
-=
l:l, 0 I
H;
-
S,.s-
=,
o
. CI(,q
z:
V
1,01
f
~,.i~
H
:: ~,7 (
0: ,,,,00
c
I~IK 0 J. 1
ao ~. 3 I
'X
'is. 7/
:
C 3 H, 6 0 d.
Determine its molecular formula
Ii:
I;).VI
;:J.,7
/.01
-
--
;).07
I-{;, 3
Ci:
:;
3S.qS
E.
C.e-
~ tf,o~
RJR..t1{ ,
i.s;
C3
C:- (3)
I~=-
H
Cf
C-P
C~
::
C/. 0 1
/.36
::
I,
--
(a.)
3(P
1.0
3~,03
,0;;
=3
/1.(
a. ~7
1~.OI-=
eJ:- (/) 3 sA! s:
'f
C.
J
has the composition 49.1 % C, 2.7% H, and 48.3%CI. Its
C ~ I-lL C..e
C.19 ~ C...el.. \
Determine its empirical formula.
C:
I
s:
,t),t;
32. A moth repellent, para-dichlorobenzene,
molecular mass is 147.0 glmo!.
q,
3~.oo
1~,oO=
q,c;
E . FOi2.r'\I(
t(
O~(a.)
.=~
7. 0
13.. S-O
I
v. C.R
33. Aqueous nickel (II) chloride reacts with aqueous sodium phosphate to produce solid nickel (II)
phosphate and aqueous sodium chloride.
Determine the moles of nickel (II) chloride needed to produce 0.479 moles of nickel (II) phosphate.
s.o x
3$· Cf...r
34. Chlorine can be produced in the laboratory by the reaction of hydrochloric acid with solid manganese
(IV) oxide:
4HCl(aq) + Mn02 -
Cb(g) + H20(l) + MnCh(aq)
Determine the moles of HC1 required to produce 12.5 moles of Cl-,
I;).
5 /J{j
I
CJ~ I
r
iK'! IIC/
I hit! fliT
35. Nitrogen monoxide is oxidized in air to produce brown nitrogen dioxide:
2NO(g) + 02(g) -
2N02(g)
Determine the mass (g) of O2 required to react with 2.20 moles of NO.
j
08 :
I
36. Aluminum reacts with oxygen to produce aluminum oxide:
Determine the mass (g) of aluminum oxide produced when 6.00 moles of aluminum react.
OVER
37. Lithium nitride (LhN) reacts with water to form ammonia gas (NH3) and aqueous lithium hydroxide
(LiOH):
Li-Nts) + 3H20(l)
->
NH3(g) + 3LiOH(aq)
Determine the mass(g) of water needed to react with 32.9g of Li-N.
3~J U~O
::
In".J
I
38. The complete decomposition of sucrose (C I2H220
11)
L'J
tJ
III 0 J-j f..Iz...O
Jhttr-l ilL. tJ
caused by strong heating may be represented by:
Determine the mass of water produced when 684.7g of sucrose decomposes.
3 L{ ;J. 3~
C,.J·t..0 {
39. Hydrogen reacts with ethene (C2H4) to form ethane:
C2H4(g) + H2(g)
->
C2H6(g)
If 40.0g C2~ and 3.00g H2 are used in this reaction, determine:
a. the mass of ethane produced
k/(),
~'j
C.}-I-il(
I
)WI~
e/..~tf
.;J.f.O~
C)-I"
C~ I-/t{
b. the limiting reactant
c. the reactant in excess
J.../ d.
d. the mass of excess reactant that remains after the reaction is complete
j
l-t ~ :
40 . 0
II
J
C:l If 'I
I
3.00-
';;.8f
OVER
41. Potassium superoxide (K02) is used in rebreathing gas masks to generate oxygen:
4K02(S) + 2H20(l) ~ 4KOH(s) + 302
If 17.78g ofK02
and 18.02g of H20 are used in this reaction, determine:
a. the mass of oxygen produced
/\
_ 1/"SjK.()J.
jU~ - _
j
Of).
s:
I~JKO(J.
I
71. 'OJk()~
Ii. 0 02...1
1-1.;.0
~-
I
b. the limiting reactant
c. the reactant in excess
d. the mass of excess reactant that remains after the reaction is complete
.- rJ,
d. . J..S
(l S
42. Heating an ore of antimony (Sb2S3) in the presence of iron produces the element antimony and iron (II)
sulfide:
Sb2S3(S) + 3Fe(s)
---+
2Sb(s) + 3FeS(s)
II
Determine the theoretical yield of Sb produced when l5.0g of Sb2S3 reacts.
j Sb
I S.
s:
OJ S6,} S3
-I
S~~S J
W\~
3 ~
q. lL ij
d.w,..-R. 5 ~
t
S L z, S.3
f Ivt,.f
36
1;)/,
L
S .3
Determine the percent yield if only 9.84g of Sb is actually produced.
43. Iron (II) sulfide is produced when iron is heated with sulfur:
.".....-<.
Fe(s) + S(s)
->
FeS(s)
Determine the mass (g) ofFeS produced when 25.0g of Fe reacts with 32.0g ofS.
j
Fe S -
.;?s.C
Felm.,.R.
5 s.
j~
S -
3d.. <9
J
re
~ 5J
'I~~ Ft.')
Fe
S
I~~ F-e
~7·q(1 {;J
Im~hS
67 •.9/ J reS
Determine the percent yield if only 16.5g of FeS is actually produced.
ic.
5
39, <f
'11.97.1
OVER
1h1...(
Sb
si.
7.5.