ft tW S = Fe (.eWAltA+i S'/ +Vrt v6fli 4)oVewK s = COi C oitC'/la com ov t)

f 0vvvwl(\ i S K ftCl Cl nic cov it oc d )

THE MOLE AND Name AVOGADRO S NU BE > "Particle$,, can be atoms, molecules, or formula units.

How many pcur- icks are in the quantities below?

1. 2.0 moles of WiOy {p.Q2 lnnoltu/|tS,

Imoie 2

l.lxiomoltcultS

2. 1.5 moles of y (0 .oz x in z3 A

1 molt Acj

.o /o25

a+om

3. 0,75 mole of d®2. y ( n7 XIOz:J r oltci;lt

1 olt CO2.

14.5 XlO23molecu lt CO 2.

4. 15 moles of CClt x (p.ozxiO2 3 olecul | ole CCl'i

•0 X/02l1

5. 0.35 mole of at| v (n.ftz iO23 Fc m /tA t/ i+ I ovt NaC\

21 X10 25Fomx/lA uni-

h/aCI

How many moles are in the number of po -b c- below?

1, 6,02 X 1023 ohms f Cu~ % | rYlu Ctr( .02 10 5 ( DYYi Cw

j.00 ol Clj

2, 1.204 X 1024 ov uia- Mifs A-N63 I noojfi, MaN Os _ 2-00 mol N/aNOj(j>-OZ >C025 Po r viA.

nft , ft Qs

3. 1.5xlO20 vv\o(ec uies L api . H.H,s = 2-5 XlO*t, ol m 5

(p.0ZXU>25fv,ol CulC MH3 q( ooooZ5

4, 3.4 x 1026 . i« °f% I molt Hg

Y o f sc»e< ri ooW-h 0'0

0> OIXIOZ30 mol Ho|

5, 7,5 x 1019 -fw YwultfL. \it s of SnO ! molt Zno |. 2X10* ™ol Zv O( .OZ 10Z3 Poim oia / m-7

vn ZnO 2£ 0 00012no in

Scient henot«+,®'r

D0 ot eoo«l! 05T exact ma !

© AM FORMULA M SS = tw f ss Nam©

Determine the gra formula mass (the mass of one mole) of each compound below.

1. KMnC>4

2. KCI

3. Na2S04

4. Ca(N03)2

5. AI2(S04)3

6. (NH4)3P04

7. CuS04

8. Mg3(P04)2

9. Zn(C2H302)2

10.. Zn3(P04)2

n. h2co3

12. Hg2Cr207

13. Ba(CI03)2

14. Fe2(S03)3

15. NH4C2H302

< H.Q52 r oL

7 .551 / ol

m.c g l

l( W.Q8(g g/mol

5 12.1 glmol

i .0H1 j/ ol

g I ol

22 . 5 /mol

gl oi.

ex: fl.CP z

: 3 x 2 .305p : 2 x 30. 7 /O

to+ulOf cumrojoct

o * iG .99c)

/)PD -to at+

(a2.024 g/moj

/p/7. IG>5 / ol

Q .22 g/mol

51. 7 g/mol

3

MOLES ND M SS Name

Determine the number of moles in each of the quantities below.

1. 25 g of Nad ,A I nolfr MxCI

58. 55 N Cl 0.45pnol NaCl

2, 125 g of H2S04 toaoio HiSOh8.078g H2S0h ' I • Z7 ol HzSOq

3. 100. g of KMn04 1 molo k MnOwl58.05Zg KMnOc, 0. 33 mpj J HnOq

4. 74 g of KCI x Imolb KCI-7 .1 KCI 0. mol CI

5, 35 g of CuS04 limolo Cu Otf _154. 03 Cw Oi,

0.22 mol Cu60q

Determine the number of grams in each of the quantities below.

l. 2.5 moles of NaCl x 0, Natl .

1 Nac | 160g NaCl

2. 0.50 moles of H2S04 x 4 .018 flI mote HzSO M jq HzSOh

3. T.70 moles of KMn04 158.032 8 KMnO«

I ol KMnOij 26.10 KMnOm

4. 0,25 moles of KCI 7H.55lci KC]1 moft CI 150 KCI

5. 3.2 moles of CuSOa | 5<:). (0O8 3 C Oh

1 r ol Co60ij 5iO

4

THE IVIOiS AMD OLU EFor gases at SIR (273 K and 1 atm pressure), one mole occupies a volume of 22.4 L. Whatvolume will the following quantities of gases occupy at SIR?

1. 1.00 mole of H2 i Hi22.HU HiI nnolc H2

2. 3.20 moles of 02 x 12ML 021 nno\t 71- 7L O2

3. 0.750 mole of N2 v 22-HL z

1 Nl 2 Hp.SL Nz

4. 1.75 moles of C02 2. L CO z5 .2 L COz.\ i violt CO2

5. 0.50 mole of NH3X 22.M 3II L /v/Hj1 nnol W H3

6. 5.0 g of H2 x I ol Hz. 22 '/\L Hi*5(0 L H -z..0l g H2 1 ole H2

7. 100. gof 02 x I ole Oz 22.' il Oz70.0 L Oi02 1 molo 02

8. 28.0 g of N2 x 1 le Nz y 22.H L Nz 22 28.0IH 3 I 2 1 mole M2

9. 60. g of C02 x I ol COx Y 22- Oz _ 5I L C02C02 \ mole O2

10. 10. g of NH3 x 1 o Ic M H 3 Y 22-H L- NH3 _ I5L M jIT.OSlj NJHs 1 mol N

5

MIXED MOLE PROBLEMSSolve the following problems.

Name

1, How many grams are there in 1.5x 1025 molecules of C02?

1 -0Z I0 o\ c l« | olt COi>00 3 002-

2. What volume would the C02 in Problem 1 occupy at STP?

> , .i , nn. I noio CO2 2C |.5XI0 COz / COiSMI L P02.

3, A sample of NH3 gas occupies 75.0 liters at STP. How many molecules is this?

n Mu irviolt KJI- b.Qim13 mQlhcu Nt

7 ' 5 21M L N j X I H: NHj 2 01XI 0 m lKulM MH,

4. W at is the mass of the sample of NH3 in Problem 3?

-7c; ni m h I rviolo NH y 17 051 g750UNHJX ' ulgH, V Imottuw,

57-0 g N1H3

5. How many atoms are there in 1.3 x 1022 molecules of N02?

( 3 XlOzlmolec i NO x 5 =1 ol c lt NOz MJLiOt daniNO

6. A 5.0 g sample of 02 is in a container at STP. What volume is the container?

molt 02 22 Qz. -

l 1& °2 L 0 5 Ogj O2Sl.ci S Oz

7, How many molecules of 02 are in the container in Problem 6? How many atomsof oxygen? 0

r z-v a |mo\ O . ffl.O2XI0 3 moltcuJC Q7 Q b\ x\dzlnno) c\j\C<> Ozg0302X -s or oz

a 02. X I ma 02 y .02 1 Ici X 3 gTorvif? 31. 5 02 | wiolt 02 i mol cule 0

1. y iO23 Q-h?m Q_

6

NamePERCENTAGE COMPOSITIONDetermine the percentage composition of each of t e co pounds below.

1, KMnO„ KM,>0H=I58.°323

y - 5M • 7( 7.

Mn = ,68,032 O = H0.5QX 7. O = x oo = o.gox

2. HCIH = <3.7 -

Cl =

3. Mg(N03)2

Mg =

n =

O = W.722.

4. (NH4)3P04N = 3 B 1 *7

h aju P = ao.78X

O =

5. AI2(S04)3Al = J6.77

S =

O = 11 X_

Solve the following problems.

6. How mony grams of oxygen can be produced from the decomposfflon of 100. g

ofKClOj? _£L2j -£> -11 VICO. 31.17/0 Hj -xicio =

7. HOW much iron can be recovered from 25.0 g of Fe ?-ii i -

8. How much silver can be produced fro 125 g of Ag2S? 10 - ft

I25a x 0.8700 = 7 2i5.7 3<i «-ioo. n/.7 25A x 0. 1

a3 1« y.

a -V lcl \- Snncrll

X oltDETERMININGEMPI ICAL FORMULAS

POfc vl

Name

8

DETERMINI G olecula FORMUL S (T UE FO ULAS)

Name

Solve the problems below.

The e pirical formula of a compound is N02. Its molecular mass is 92 g/ ol.What is its molecular formula? |s|Q2i .005 g/mol

. , __ so. o u SC P+S1

Moltcw i , M_ ql ol __

Empiric £ <1(ff.OQ5K/aOn

2. The empirical formula of a compound is CH . Its molecular mass is 70 g/mol.What is its molecular formula? Ch2 = IH. 27 g/ o|

~70g/mo|

IH.ozi g/™iC/5. IQ-

3, A compound is found to be 40.0% carbon, 6.7% hydrogen and 53.5% oxygen.Its molecular mass is 60. g/ ol. What is its molecular formula? rP/nd empiri cal

Q-Oa Cx- lt~ = 3-5 o> .n 1 CH20 = 3o-o2 g/ 7)3 12011 jC '

(j-1qH x -l - 5 z

'•ooe3 e 30.02 3

55-63 TiSy r2 5511 : :

4, A compound is 64.9% carbon, 13.5% hydrogen and 21.6% o ygen. Its molecularmass is 74 g/mol, What is its molecular formula?

CmHioO

5. A compound is 54.5% carbon, 9.1% hydrogen and 36.4% oxygen, Its molecularmass is 88 g/mol. What is its molecular formula?