Name
lB Chqmistry1
JCiwt TstrV
m'
Practice
TestUnit2
Fkgil\b GasStoichiometry
F-{Btit
2011-2012I Massey
(answer
keyonline!)
(atm):
1.) Convertthe followingto unitsof atmospheres
o,6?2.
a. 488 mm Hgy
2. ) A ri g idco n tai nerhol dsa gas at a pr e s s u r eo f 0 . 5 5 a t m a t a t e m p e r a t u r eo f - 1 00 .0 "C .
Whatwill the pressurebe whenthe temperatureis,increased.to
200.0 'C?
=M
3.) What is the volumeof a sampleof 02 that has a massof 50.0 g and is undera pressure
of 1.2Oatm at 27.0"C? Fszrt^ f) ,\. !4d, elr-^/
n -
of1zo^t-^Ltk$ gaoAozy
ffi=
,) nAT
T-r-
-0,r
/.9(mo/O7_
=
/, eot&7
4.) A pieceof aluminumwith a massof 4.25 g is usedto generatehydrogengas by the
followingreaction:2 Al(s) + 6 HCI(aq)--->
lf the hydrogenis collectedat a temperatureof 15.0 "C and a pressureof 94.4 kPa,what
volumeof hydrogenwill be produced?
ry.AcAE/yffixffi=a'A37no47
.V=; n/Lr
--;5-=
-r
g&0,
(o,1,3?m,)(filzffi
(?q.ry/(R)
Tl
/
^\
< ) ..-
,r l' ///
f )/
\/(
7,
n
tgrt
i
to produce
5.) Duringan experiment,potassiumchloratewas completelvdecomposed
water with
potassiumchlorideand oxygengas. The oxygengas was collectedby displacing
a gas collectiontube. The followingdata was collected:
= 0.2 5 6 g
Mas sof K C IOg
V = V ol umeof 02! = 76 ' 9 m l
= 20.8"c
= e?3'8K
"-Temperatur€
"' r - "
+=Room
t/
Barometricpressure= 731.3 mm Hg
Vaporpressureof water = 18.7 rnm Hg
a. Write a balancedequationfor this reaction:
?uTlos\+ a,re/Qr so.h)
the numberof molesof oxygengas produced.
b. Calculate
.r2, a r>/'
t//t/
/4
/'eo /
. - $ no/
o.erftrfc/osxm"ffi
02
a-A
003/3
v
Plgd_tPtrrol)
c. Determinethe pressurefor the oxygengas. (Hint:Pbar=
P= 7E /,3 -/tr.7=7H.6-,
t/
.
d. Usethe CombinedGasLaw to calculatewhat the volumeof the oxygengas wouldbe if it
- nurE
L-
/2fi
= /ZoaL
e. Fromthe abovedata,calculatethe molarvolumeof the oxygengas at STP(expressyour
answerin L/mol).
dZ om L
V7
t;
-
t ro/
-r
b,m6/3nq/
= a4ryeA 7/.??,,"-l
f . Usethe knownmolarvolumefor a gas at STPto calculatethe percenterror for this
investigation.
fffvvJL fvq
2
li
6 .) A cyl i n d e i n a n aut
The
insideto e
nal measuredpressurewa
T
measureda
alculatethe frnalvolumeof the cylinder.
measured
R4T
vz=%-u.rr;lnlw!
&,T __-
7.)A tw h a d Cffi re}rui | | 0.505mol ofc a r b o n d io x id e , a t a p r e s s u r e o f 4 . 2 5
atm, occupy-avolumeof 3500 mL?
'7/=ttr rr,,<= S/o/<\
r/'-fi6jPt1-- U,Ara/m' |rrl
'/
,fficJlat/n.rof;/W
,o/)
36o-erc=tw/ (tr2"c
8.) A gas is foundto havea volumeof 22.5 L at a pressureof 180 mm Hg. At what
pressurewill the volumebe 2.50 L?
pr f u,.= QPrntzl\(-z'r/ l.
/ ze
V.
,_s i /'
measuredat 1800. mm Hq and 28"C.
diox-ide,
the massof 275 mL-of;nitrogen
9.) Calculate
= O. O 4/Vno//1/02
o.oe6vmo/ilot_y#=l t@
at 25'C.Thevolume
measured
Z.Zlft$of carbondioxide,
contains
10.)A frreextinguisher
pressure
of the tank (in atm).
internal
is 3.2 L. Calculatel6e
of the extinguisher
I tlF)
t-4./.eo-?= f/, / mr/c0zX,*rnCozx #x
7?.o/A
.#)(a?14
(g.t .DP'ofa,H
/c- /2/T a.
V
/
--v
' ^-
(J ,^L)
to form solidpotassium
1 1.) Whenheated,solidpotassiumchlorate(KC|O3)decomposes
potassiumchlorate
gas. lf 2.0.8g of potassium
how mar
many litersof
chloratedecomposes,
decomposes,
oxygengas/RO.8
chlorideandoxygen
chloride
oxygengaswillform
^#y\Hint:
t^anstet
/^rqa /
#5)
reactionis in question
Samechemical
3nt/
O z -,-
Z 7, 7l
Ao , 7 6lff/ar rfuxffir r
-
=e7D/
-
O2
12.) Solidpotassiummetalwill reactwith CIZgas to form potassiumchloride.How many
litersof cl2 gas are neededto completelyreactwith 0.204 gramsof potassiumif its
pressureis measuredto be 680 mm Hg aqd its temperatureis 55"C?
afTT-c/t+ Atrc/
13.) In th e syn t hes i sof ammoni afrom it s e le m e n t s ,
N2 (o) + 3 Hz (g)--->z NH3(o) ,
a.) what volumeof nitrogengas is requiredto produce5.3 L of ammonia?
s3LN//a.*r%=@
b.) what volumeof ammoniais producedwhen0.75 L of hydrogenreact in excess
nitrogen?
z L/V4r o . 7 rL4x SLtz
.
c.) lf 5.00 L of nitrogenreactscompletelyby this reactionat 3.00 atm and 298 K,
how many gramsof ammoniaqrg produced?
F;;. I Ar
n L/V.f"
,at
r.o;L/VLx4+(.{t ,= /o.oL/Vftl
TL
'1/s
/l =# =(3,oa<Art
/a o/
= /.23m0//4
@EK)
il/s
4
14.) Forthe reaction:Z CO(g) + 2 NO(g)---> N2(O) +
Z CO2@)
a.) What is the volumeratio of carbonmonoxideto nitrogen(in liters)?
2 L(oz
b)
/LlVu
gas
vorume:'T;"n"
'"'o'$u@)hat
" liulolJ,l,33.:';acted
o Multi p leCh o i c e
andtemperature.Whichof these
15) Two samplesof equalvolumesof hydrogenandnitrogenareat the samepressure
statementsis true of the gases?
a) Both gaseshavethe samemass.
b) Particlesof both gaseshavedifferentaveragekineticenergy.
of both gasesare movingat the samespeed.
c) Particles
d) The hydrogenhasmoregasparticlesthanthe nitrogen.
6tfn" grr"r-frru" the samenumberof particles.
\J
16.) lf a gas is cooledfrom 400 K to 100 K, its volumewill
threetimes.
a) increase,three times. [,)-decrease,
c) increase,two times. 6Dt".r"rre, four times.
17.) At STP,one moleof all gases
ih" ,rt" volume.
a) havethe samemass. @ru"
c) havethe sameformula.d) havethe samemotarmass.
0 =/ < *t7
18.) An expandable
chamberhas a volumeof 2.0 |- r@fr,n".nmber
10.0 L, what will the qggrpressurebe?
a) 5 atm b) 1 atm (1p.2 arm d) 0.5 atm e) 0.1 atm
is allowedto expanduntil it has a volumeof
what
at STP. lf anothertwo molesof N2 is addedto the container,
19.) A containerholdsone moleof N2 gas molecules
is the new oressure
of the mixture?
a) 2.0 atm
b) 0.5
"rrn 6)-)o
,,r
d) 1.0 atm . e) cannotbe solved
20.) lf at STPone moleof oxygengas (O2 , 32.0 grams)hasthe volumeof 22.4L, what is the volumeof one moJqof
ozo ne
s r a mastrS r p ? ,
s as1o3. 48.0
a) 6 72
Lb)448r ffi ,
r / /U%I
tftu g
have
that gasparticles
21.) Accordingto the kinetictheory,it is assumed
a) no pressureor volume
c) pressurewith no volume
Ae r ' , 6 /e
6'(:
.verr'Ir '
I
i
V
n
a
u
i
f
r
'
a
F
"i{n',
4 &e/U
llot
fu .O
i
b) kineticenergyandpressure
size€Fattractiveforces
/d)1 no signifrcant
\/
26f
5
22.)
r&nx #lr. f,rfrrrd',
txhk r{,lt$ ct$r t}f thrs{' t*mns; irusr"r=*r,sss,.decr*-*rs*r.
FiNlfin *fu*fnf,l*lr,irttrl
*rf,gas
ir rql'flsFfirtd"
Ir-nrh t*rnr ntiltr'l:l*'us*d eru:l'r'th*ffisrrrr#.rtpsernw*Nr*srnrc*:rt
Isriprr*trre
hm*rr*
Solrrr*
inrreeger
r. decra,rcf
tntrc;tet
rtayrsth* sas:e
4. dee/&{e!
s. )neleq.feI
s. ;rr4'/e6 Ced'
inrreas*'t
ltarls the sa#*e
lni:refr5*5
FaB'1,8
6. i nefe^Ier
sttsvrth'3 $Emle
'Cerr*ese5
sta_ys
the sar*re
tnr:r€i5i35
gtey-E th*
Ite'J"tth* sarr'te
tntr€€::Et
t. deaagt€s'
s. ;a(r'e4fies'
elerr*ares
lte$E th* iarile
flFtrs;gEg
tnIfea5e!
qlerreas*s
deele4 rgI
rtays the ranre
TET
S.
"nr. deefeate{'
stes5the iaryle
t2.
-f. in<rr'e4te!
stavr5th* saffie
n. g h,tt *tfe tdvt
v
derrea*,e*
9tts?-5
the serne
d*cr*.*seg
on specifrcgas laws. Below
23.) Eachof the followingthree diagramswerecentralto your text's discussion
eachdiagram,namethe gas law beingdescribed.
n
PrPr5il14-V$hrme illarrqer
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i
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JJ
1,rttt l, u".
I
l0L:
\r:lr:{r"
tq
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iu
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34
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t r-
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fi.r'l a\*t, 5 L:
- J *- - ; t '
:
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J i,,,.,
i'l.frrr,15tl
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;:
i:r.iltin,r
r.5
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itiiil.::l'..i,i,il,,:1"Ir;i{t""'n"
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r i75 1 7i] 3r(|
r) r. 5St' ri r'{
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2r1-?4t -llir -JL\l ..5r,1 {
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c^"r^*chah/eit /.c',
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1t}, r,t!.
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r
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" t.tt,t
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.,
,s.
Gas Law:
..Jn
ji'
,:r
1..3r ,. * {i lt. I
.,{"
.,.u'{'l-rny; * ;-:r.1;;
ffi:''/nft4cf
./.at/
6