1. What is the mass of 7.50 moles of sulfur 17. What is the percentage c0II!.~~~"dioxide (S02)? TlfW dinitrogen tetroxide (N20J?(8 = 32.1 g/mol; 0 = 16.0 g/mol) ~ (N = 14.0 g/mol; 0 = 16.0g/mol) 70""/00

2. What is the mass of 0.438 mole of ammo- . What is the percentage composition of a 43 010 Gnium chloride (NILCI)? ~ carbon-oxygen compound, given that a 95.2-g 0

(N = 14.0 g/mol; H = 1.Qg/mol~5 g/mol) sample of the compound contains 40.8 g of carbon ~7 /1 0r3) How many moles are there in 250.0 g of and 54.4 g of oxygen?

sodi~ phosphate (Na;?04)? . 19. What is the percentage composition of "(Na = 23.0 g/mol; P = 311~Ql; \ . suIfur-chlorine compound, given that a 30.~ Jl ~/4 ..5

.0.::;: 16;O.g/mol) .. ,·U5j>-tfV\i)\e sampleofthec~~poundisf~undtocontain9.93 ,.q.<lj. 1/".", ..' -'~'. 4. How many 'rnoies are th~re in 993. g of . of sulfur and -21.;5 g of chlorine? ' '. - lY. ~ l

: .c-:,:.: -potassiurrt.sulfate (KiS04)? 5./0 I me Ie: . 20.' Asample ora compoundthat has-a mass :_ : .(K = 39.1 glmol; S = 32:1 g/mo; = 16.0 g/mol) 'of 0.432 g is analyzed. The sample is found to be' 70 ~ F==-s. How many atoms . 3.00 moles made up of oxygen and fluorine only. Given that b

of sodium (Na)? 1.1.1 'f.. m;!~oll>vy)~ the samplecontainsO.128 g of oxygen, calculate 30%06 H· th· 1 638 x the percen e com osition of the com ound.

e ow rnanyoms are ere ill .10-9 mole of lithium (Li)? 1-q.<6101 'f-.. 1014 a\-vm ') \ 2 Find the empirical formula of a com-

L _ pound, given that the compound is found to be )-----.17. 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). l? ,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 com-ere m. mo es 0 rntrogen 2J. ."'1 'f-.jl) i1jpNll; IVa.l d· th t 48 5 I fth d~. - .poun ,gIven a a . -g samp e 0 e compoun' f39. How many atoms are there m 0.663 molt: is found to contain L75 g of carbon (C) and 46.75 g t t'-f

of water (H20)? ·1 \. 2.Cl 1- (010\- iHo)'y\..S J 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)? I ;/",'57 me I] 23 What is the empirical formula of a com-

11. How many moles are there in .32 x -1l. d, given that a 212.1-g sample of the com-rc;tn} i .-,.._.......,1;.;.0_12~lecules of carbon tetrachloride (CCI4) ~.?b'~'fVJ\tpound contains 42.4 g .of hydrogen (II) and 169.7 g~

;>" . W What is the volume occupi~ of carbon (C)? What 15 the molecular formula of420 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)

gen dioxide gas (N02) occupy at STP? .3Z.Qclm·3 .' mo, . mo14 H . I there i 45 0 dm3 f . 24. A compound is known to have a gram

. ow many mo es are ere m. 0 I ul f 391 5 I L Find th . . almethane as (C~) measured at STP?~ mo ec ar mass 0 . g mo e empmc ~

g . . ~3 . and the molecular formulas of the compound, BI15. 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~gongas (Ar) at STP? lIso 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)

. o (oTn.po:::,H;0 () - 1To t:hd -errtPif-t 'ccu tor-mu.la.,N\(1)~k&"'1=;- To\-J ,P&r~ W1~) = % Cr;fYI,p. t~{cltmtJlt1 t. t;e;i- Moles .... I ~ut

L~\v rdt. Ail ~1'1(}\e:) plJ j'ma./lt5t- /)10 eA!:'.~:: 3. tC: YCju,~b abovt C\1)<*- whole VltttYIhtf5, y()Jfi p~ h'j .. ,. J.. 3 ecl- 10 mili -then; ~vh()r

I t..{il't ~ -k flJ \lY\o\e'eu.J4 v .{OrtVtu.l&..,", I/, .OA-Nutj~~~5 5 . \70 tiliOJe.. :5>~51 AtJD up ~mAs'S of CfI'Lpr n CA./-- ..8-8 CHEMISTRY:The Study of Matter COPYRIGHTby Prentice Hall. Inc. ~'i ~ <t" rom fik-Y"l 1+ q.o 1M\ewav h7.tL '>5.

r.ax;,'cl~ . Reproduction of this master is restricted to duplication 'for classroom use only. ,/~()'/'l.>

,

~me -'-- Date Class _

CHAPTER 8 Text Reference: Section 8-10

Practice Problems

-~(

I. (f'vJs.)

__ ~,....-..,-_-, Date ~131!Qa, Class _I. Get rf)olf~ .-L'

t-, Us-c CDe~'Netif rtLIlOS T3, Converf- fo ufJlr tJft!~~~erence: Section 10-5

\r:)Q

Practice Problems1. 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 '\4 {Y!:be produced from 0.172mole 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(80

3) according to the follo~ balanced chem- (Hg) that is required to produce 29.8 g of mercu-

ieal equation? " ry(I) oxide (H~O) according to the following bal-'. anced chemical equation. "

.~":;;r15-----_~02+ Oz-. 2803, =~,~ ._.. 4H (l) + 0 (g) 2H O() ;zi~9c;.HA.., .< GS I , - <, '. -=j·",\.vo. ' g z -+ ~ SUO.:7. 'I ;;.1/:1'-, 3. Calculate the~ occupied by 16.3

moles of nitrogen gas ~STP. Jf..a5 ':J 1 (Hg = 200.6 g/mol; 0 = 16.0 glmol)4. How many moles of fluorine gas &~ r€. 12. How ~ of water vapor (H20)

contained in a 0.269-ilm3container at STP? • . 'i:i will be produced wh~m1.18g o(hydrogen gas ~2)

5 Assumin that th all STP.find . ieacts completely WIthoxygen gas (02) according• g. egasesare at. to th balan d ch . al ti <)

th I ~f nitro dioxid (NO ) th e ceu cr enuc equa on.evo ume, 0 m gen OXl e gas 2 atcould be produced from 71.11dm3 of nitrogen gas 2Hig) + Oz(g)-+ 2HzO(g)? JO~~ ~ *TU(Nz)acco~g·tothisbalancedchemicalequation. (H = 1.01 g/mol; 0 = 16.0 g/mol)

~~l-.,?-:2-~~li~9"T202(g) - 2NOz(g) ,' ... - 13. WhatEl'!b~f chlorine gas (C~). ~ea~6. Assuming that the gases are all at the sured at STP, can e produced by the decem-

same temperature and pressure, what Milum&'of ~sition of 73.0 ~ of hydrogen chlo~de gas ~Cl~oxygen difluoride gas (OFz) is needed to produce /:;:;;-.8lventhe following balanced chemicalequation?1.54 dm3 of hydrogen fluoride gas (HF) accordinf- '? J 2HCl(g) - H2(g) +CI2(g) ,: -z ~ i-."'lI ~ ~ dnrto the following balanced chemical equation? Alif..! .J'-' 1 \ • :::> J f d(,.t.I..l'1 .

'0 • .~'1o<rL{li= 1.01 glmol; Cl = 35.5 g/mol) , . .' '.OFz(g) + 2Hz(g)- H20(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 ofof oxygen gas (02) that react with ca1ciurn.!Ca) . sulfur trioxide gas (S03) according to this bal-according to this balanced chemical equation? - anced chemical equation: 0 Q gA '3~~

2Ca(s) + 02(g) - 2CaOes) 9 5X\ct~ 2803(g) - 8(s) + 302(g)R<> \,JU'"

8. Aluminum metal (AI) reacts with sulfur ~ (8 = 32.1 glmol; 0 = 16.0glmol)(8) ~ produce alumin~ sulfide .(AIz83]acc~~/ \"'} 15. How many~rrnula uni§ of sodium chlo-to this balanced chemical equation: (D $1. &: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?

How many ~of aluminum will re corn->: '. .23pletely with 1.33 x 1()24 atoms of sulfur? 2Na(s) + C~(g) - 2NaCl(s) t,~.2)'\'0 .. , li~

"',(11--<\,>"-',-

9. Given the balanced chemical equation for (Na = 23.0 glmo!; CI = 35.5 glmol) . --t"t~I(~"",:-+ .)the decomposition ofphosphoros oxyfluoride gas 16. Given the balanced chemical equation(POF3). 2Ag + Iz_ 2AgI

LJ.41j?~3~t- p.(s) + 20z(g) + 6~2~~ '5 how many~of silver metal (Ag) are requiredwhat volume, !atSTP, of fluorine gas (F0 co~d be to react comletely with 531.8 g of iodine (Iz) to _,'

_ produced y the decomposition of 9.22 x 1()26 produce silver iodide (AgI)? '1 5'1") x: \~. ~n~molecules of PhOSPhOrys-OxynUOtid~ (Ag = 107.9 g/mol; 1= 126.9 g/mol) J-t. J.. .., cv •.. 5;lS-X: \~10-6 CHEMISTRY:The Study of Matter" "'COPYRIGHT by Prentice Hall.lnc. .

Re~rQdl.lction of this master is restricted to duplication for dassroom U$e only.

,--'