Molar Mass

Molar mass is the mass of ÿ'1ÿ ÿ]t}{ÿ• Other names for molar mass include:

. 4bm la ma

of a substance.

One rnoieq#mic

Ill

II

of any element will have a mass in grams corresponding to the value of its

For example:

1 tool Carbon = JnÿD I J g/molw •

I tool Nitrogen= /ÿ{ÿ0ÿ ÿ g/mÿl

Diatomic Elements

The following elements do not naturally occur as one atom-they are always in a pair:

,. h qdro m I

4. f Idol/he_. fÿ5. illtfOÿr..,i ÿ j(Jz.

7" ÿ]ÿ }l'}e, ,,) ,ÿ'g

*Trick to remembering the seven diatomics*

One ÿYÿ0L of any molecule/compound will have a mass in grams corresponding to the value of its molar

mass (the sum of the masses of the elements that compose it).

• Ex. HzO H: 1.008 X 2 = 2.016

O: 15.999X 1 = 15.999

181015 g/mole

1 EX, Ca(NO3)2 Ca: 40.078 x 1 = 40.078N: 14.007x 2 = 28.014O: 15.999 x 6 = 95.994

164.086 g/mole

Sample Problems #1-2: Calculate the molar mass for the following compounds:1. Potassium carbonate --> ÿ {1('ÿ)%

' ...... J ÿ1ÿ. 1%

#of Caroms: 10]'Ott x l

2._> idr

# of H atoms: 1,00 ÿ x ÿ

91,olff+

I{,OÿH

.o, oo,omÿ:/O,+ÿ x q

÷

PRACTICE: (SHOW ALL WORK & UNITS to receive full credit.)1, What is the atomic mass of sodium?

1ol92. Calculate the molar mass for AI2(SO4)3.

A i = ol6,qÿa x ÿ -

g :la,oi x 5 -0 - iD ,ClCfClX i<7, :

6J,qÿ,ÿq

D

. Calculate the molar mass for nitrogen (hint: is it diatomicÿ)!).

4

lll [] UNOTES:

B [] B [] H [] H FMolar Mass

i o convert between units, follow the highway. Notice,there is no shortcut from grams to liters or between any []

[] of the three units surrounding the mole.

(from periodic table)in grams

[] m []

22.4 LVolume

/ÿases onlv)

I This means you have to convert tobefore converting to another unitf

[] l [] ( [] ( []

6.02 X 1023

Representative Particles{atoms, ions, molecules, formula units)

PRACTICE: Moles & Mass

Draw the Mole Road Map:

1 mol (o,o xlO d-id

1 MOLE

1 tool

5

Molar mass:• called p;ram atomic mass when single element is used.• called ÿram formula unit when ionic compound is used.• called ÿram molecular unit when molecular compound or diatomic molecules used.

o Diatomic molecules are atoms that bond with themselves. There are SEVEN of these that you need toremember: Br212 N2 CI2 H2 02 F2 (Remember this by the name "BRINCIHOF')

Dimensional Analysis General Formula:

@van # unit W Unit Want }ÿ.ÿ...ÿFina| answer in Wanted unitlL Unit given

Conversion factorConversion Factors:

> 1 mole = 6.02 x 1023 particles (Avogadro's number)> i mole = molar mass (Sum of atomic masses in grams)

I mole = 22.4L of any gas at STP (Standard temperature & pressure)Any gas density at STP = molar mass / molar volume

PRACTICE: (SHOW ALL WORK & UNITS to receive full credit.)Determine the number of moles in each of the quantities below.

1. 25 sodium 1. 1.

: l.O q o<

2.

ci%oaaDetermine the number of grams in each of the quantities below.

: 5 ,'t1% or"3. 2.5 moles of sodium

, r C

4. 0.50 moles of HÿS04 ÿ a C" A, ÿ ÿ '

3, 3.

4.

/<f.oii

,

C :tÿ,oli x

fl: 1.0ol x G

Solve the following mole-mass conversion problems.5. How many moles are there in 27 g of ethanol (C2HsOH)? O.

15111q6,o l

Homework: Moles & Mass

2. 74g Potassium Chloride

3, 35 g Copper (II) Sulfate

Convert to moles (SHOW ALL WORK & UNITS to receive full credit.; _ ÿi. lOOg KMn04:

2.

eu :ÿ3:55 ÿ

Convert to grams ÿ UN]TS to receive ÿuH credit. 15ÿ ÿ4. 1.7 moles of KMn04 4.

6. 3.2 moles of Copper (II) Sulfate

Solve the following(t HÿW ALL WORK & UNITSÿ..ÿceive full credit.;7. How manykÿ4 4ÿs of NaCI are in 16.0 grÿ:ÿs of NaCI? 7. I

8. How man l grams of glucos CÿHÿ206, are there in les of glucose?

O,.,-. lÿ,OiX (o: 7ÿ,06

0 iÿ,fiqlx(ÿ: ÿtS,1qÿ

5,5. 0.25 mol :s of Potassium Chloride

O, ÿ %4 I1 ÿ -.

O aTffmÿ Uo6t

NOTES : REPRESENTATIVE PARTICLES ÷÷ MOLES

Representative ParticlesA representative particle is the

Types of Particles (atoms / molecules / formula units)pO

Avogadro's number, which is

mole of any substance. For the monatomic elements, the "chemical unit" is an

any chemical : ÿ, OÿX Ibÿ particles.

, represents the number of "chemical units" in one"lÿo nÿ 1 too, oÿ

Examples (1

• 1 real

• 1 real

• 1 real

• 1 real

• 1 real

• 1 real

mol = 6. 02 x 10ÿ atoms / molecules / formula units)

Caÿ'= (o,OÿXlO°ÿ q,)ÿ,ÿ

cl (aq)= (O,OC)X@ÿ ,ÿIÿcute-J

c,ÿ= (ÿ, ÿXÿOÿ:ÿ rnotÿutÿoÿ

Particles ÷ Moles OR Moles ÷ ParticlesSample Pr°blemS ÿe xÿÿ

1. How many s are in ,4.50 ÿ atoms of manganese?

2. How manyÿoms are found in 3.ÿ'nol of magnesium?

3. Chalk is composed primarily of calcium carbonate. How many parÿcÿes are in 3.4 moles of calcium

carbonate?

Moaes of Crayon Lab

Purpose: To determine how many moles of crayon and how many formula units of crayon are used to write a

name. Materials: crayon paper balance

Part A:

1. Obtain a piece of crayon, find its mass, and record in your data table.2. Color the picture of your mole completly with your crayon.

3. Find the mass of your crayon again and record.

Crayon data

Mass (g)

Mass of crayon before coloring

Mass of crayon after coloring

Show work and include units when answering the following questions:

1. How many grams of crayon did you use?

2. The chemical formula for a crayon is C31H64 calculate the molar mass of a crayon.

3. How many moles of crayon did you use?

4. How many formula units of crayon did you use all together?

Particles --) Moles OR Moles --) Particles Homework

Now You Try! Remember to show all work and report your answers with the correct number of significant figuresand the correct units!

1. How many s are found in 9.26 26molecules of CO2?

2. How are found in 12 tool ofÿarium.

Im tScc3. How many foÿlÿtÿla units are found in 3.55 mo@ll of NaCl?

4/goc-I

id rn CO

are in 4..27 x

5. How many mÿare present in 2 45 x lÿmolec• les of CF4ÿ

, Iodine is an element required by humans in order to produce thyroid hormones. /Tÿhelp prevent iodinedeficiencies in the US, our table salt is enriched with iodine. If you need O.O211ÿper year, how manymoles ÿVodine are required per year? (Remember iodine is a diatomiÿ4.)

7. How many pÿcles would that beÿ a*

tÿ . :) , &Q: Why was the mole of oxygen molecules so excited after b.e !eft the paÿ';7ÿ?A: He got Avogadro's number!!!

10

NOTES: VOLUME 4-÷ MOLES

TI°51In Chemistry, we use the initials,

standard temperature= 0 ÿ

, to represent standard temperature and standard pressure.

standard pressure = ! Cÿ

The molar volume of any gas at STP is

at STP is equal to ÿ'Cÿ0 H L.L. In other words, one mole of any gas

Dimensiona! Ana|ysis General Formula:

Given#unitILLÿ'un!twantunitgiven )ÿ.,... Fina| answer in wanted uÿit

Conversion factor.onvufslorl raÿ1;ors;

I mole = 6.02 x 1023 particles (Avogadro's number)1 mole = molar mass (Sum of atomic masses in grams)

1 mole = L of any at STP (Standard temperature & pressure)Any gas density at STP = molar mass / molar volume

Moles ÷ Liters and Liters ÷ Moles

Sample Problems(SHOWALL WORK & UNITS to receive full credit.)

1. The average lung capacity of a male is 6.0 L. The average lunch capacity of a female is 4.7 L. Assume thefollowing:If your TEACHER's lungs are completely filled with oxygen, determine the number of moles of oxygen gas

in the lungs of your chemistry teacher at STP.

2. At STP, how many are found in 54 neon gasP

------ AIc

How many hlÿ-ÿ are found in 3 ol of helium at STP?,

Llc1 I m l-I%I;ÿ.IL H,-¢

11

Homework: Mixed Mole ProblemsNow You Try] Remember to show all work and report your answers with the correct number of significant figures

and the correct units! USE YOUR MOLE MAP.I!m: 0

aÿ

1ÿ__

0aÿ

D0>

f 1. How many grams are in 14.05 tool _ _=____ÿt-ÿ--ÿ

3. At S.TP,oneon is a gas. How many moÿes are found in 0,31Jÿ

4, How many liters are in 44.3 moles of keliumÿgas-al-S-]-4ÿ?-. ÿ

fÿtf_., btÿ

0 :ls'l?lxaÿbi'ÿl%:

Mixed MoleSolve the following problems. SHOW ALL WORK! Report your answer with the correct units and the correct

number of significant-figures. ÿJJ ,ÿ=1. Assuming STP, how many mÿlÿs are in 5.42 x 101! L Ne?

2. Convert 1.3 mol of neon into pÿrlÿticles. 1, I- - ÿ'ÿ , --ÿÿ

- li,,l;o, oC o oo "

3. Determine the numbe in 3. t1ÿ61 f Ir..3uÿu'ÿ.ÿ .,ÿ U^ (]'ÿ 'dÿ, - laO,a3

MULTI-STEP CONVERSIONSRemember how to use your Mole Road Map! ( You must a/ways go through the

I ÿMoles!aÿrti c lesÿÿ

I atoms . )formula units J

Mass (grams)

Sample Problems: ÿ ÿ1. How many ÿrams are in 45"L of neon

iÿtÿttL ÿe

as at STP?

Irnÿ

2. How many forml la units are in 36.4 g of NaCl?

. ÿ0 ÿ,ooJÿlJocI

3. What is the mass of 550 L of hÿlium gas at STP?

/

4. How man liters are in 5.6 x 10z4 atoms of helium as STP?

13

MULTZ-STEP CONVERSIONS Homework

Now You Try! Remember to show all work and report your answers with the correct number of significant _.

figures and the correct units! 0 ÿ'ÿ0ÿ ÿ ÿ ÿ ; ÿ ,(-ÿ

1. How many liters are in 56 g of helium gas at STP? __.ÿ_ÿ__ÿ-ÿ .1 ÿ :l,0()ÿ'ÿ'l(ÿ} tl0ÿ()<ÿ

2. A 12 oz can of Coke® contains 0.0345 g of caffein etermine the number of moCTecules

3. Laughing gas is dinitrogen monoxide. How many grams of dinitrogen monoxide gas are in 45.0 L of

4. Bromine comes from the Greek word meaning "stench." It has a strong, irritating odor. How many atoms ofbromine are found in 92.1 g of bromine? o

5. How many, atoms are in 65.6 L of Feÿ

6. What. is the volÿme of 5.6 g of sulfuric acid? _ Lÿ ,' ÿ1ÿ, ÿÿ}|--ÿ€ÿ'ÿ

7. If you burned 6.10x10zÿ molecules of ethane (C2H6), what mass of ethane did ÿou b, urn?

8. How many formula units are in 5.1 g of titanium (IV) oxide? ÿ ,.ÿ ,

14

PERCENT COMPOSITION

• The percent composition 0f a substance or mixture is the ÿ'ÿ(ÿ'ÿ pAÿi[T.ÿ.ÿ";ÿ

.J L'ÿqÿtÿ or component.

° To find % of an element in a compound, use ÿ01ÿ ÿ)ÿ'ÿ

of each

as the whole amount.

Example:Percent Composition of Water (HÿO):

oxygenhydrogen

When asked to find theelement in the substance or mixture.

., you are calculating the percentage of just

PRACTICE:1) Find % sodium in NazO.

Molar mass = Na 22.99x 2 = 45.98O 16.00xl = 16.00+

61.98 g

%Na=

2) Find the % composition of a compound that has 5.34g C, 0.42g H, & 47.08g CI.Mass (tota0= 5.34g + 0.42g + 47.08g = 52.84g

%c: 534ÿ x i00%: !Oo J l c52.849

%H: o.42LH x /ooÿ: O,lq H52.849

Q Jtÿ

52.849

3) How many grams of sodium are in 650.0 g of NazCO3?

Na: ÿl ÿ1IO X ÿ = ÿ ÿ,ÿ. (part sodium)

c: Ioÿ,011 x J : Iolÿ,Oj ÿ (part carbon)

o: I1,q11 x .5 : /ffl,clql (part oxygen)TOTAL: )Sfi,Cÿ<ÿ (Whole)

FORMULA:_part x grams(to,a0 = Answer grams Na = L# ÿ(ÿ<:ÿ

whole ÿ0ÿ,ÿX

4) Calculate the percent, compositi/on of C3H7OH (2ÿ1

H - i,oo%x 9 ,o69/ o,o%7 -

eo.o l915

Percentage of Sugar in Bubble Gum Lab

Purpose: To determine the percentage of sugar in bubble gum.

Materials: balance, bubble gum

Note: Chewed gum cannot be placed directly on the balance pan; it must be wrapped in paper and the mass of thepaper subtracted out. Also, once you are done chewing the gum, make sure you throw it away in the trash can. If Isee chewed gum anywhere else, we will no longer perform food related labs for the rest of the school year.

Safety: Do not chew gum that has touched the lab table.

Procedure:1. Place the wrapped pieces of gum of everyone in your group on the balance. Record the combined mass of all

the wrappers and all the unchewed gum.2. Unwrap your piece of gum put the gum in your mouth. Do not throw the wrapper away!3. Place everyone's empty gum wrappers on the balance. Record the combined mass of all the wrappers. Do not

throw the wrapper away!4. Chew your gum for 15 minutes. While you are waiting for 15 minutes to pass, answer questions under

the "While you are waiting...." Section.

5. After 15 minutes, put your wrapper up to your mouth and gently spit your gum into the wrapper. Try not toget too much saliva on the gum.

6. Place the wrapped, chewed gum of everyone in your group on the balance. Record the combined mass.7. Throw away the gum and wrappers.

Data:Brand of gum

Mass (g)

*Hint: The mass of the gum

Unchewed gum with wrappers

Wrappers only

Unchewed gum only

Chewed gum with wrappers

Chewed gum only

Mass of sugar

should have decreased because the sugar dissolved in your mouth.1.

While you are waiting .....

1. The chemical formula for sucrose (commonly known as table sugar) is ClzHz20ÿ. Calculate the percentageof carbon, hydrogen, and oxygen in sucrose. Show work for credit!

16

2. Nearly 99.5% of the total composition of your saliva is water. Calculate the percentage of hydrogen andoxygen in water. Show work for creditJ

o EXTENSIVE - Properties that depend on the amount of matter present. This means that the propertychanges when you alter the amount of matter present. Ex: massINTENSIVE - Properties that do notdepend on the amount of the matter present. This means that theproperty does not change when you alter the amount present. Ex: color

In the weigh boat, you have a large piece and a small piece of bubble gum. Examine the two pieces and comeip with at least 3 more properties of the bubble 9uÿ that you can classify as extensive or intensive.

Extensive Intensive• Mass (mass of small piece is less than the • Color (both pieces are pink)

large piece)

Analysis and Conclusion

1. What is the percentage of sugar in the bubble gum?

2. Convert the mass of dissolved sugar to moles.

3. How many molecules of sugar are in the dissolved sugar?

4. How would the results be affected if there was a lot of saliva on the chewed pieces of gum?

17

Homework: Percent Composition

0

i4f:>

0

, °i:4! ";ilÿ;;magdesiÿ+acid, is a solution of magnesium hydroxid-'ÿ. IWa sam-'---pie of antacid contains

2-i g of magnesiu' hydroxide, how much oxygen do s the sa-ple cOntain,ÿ ..... "ÿ 1ÿÿ' liÿ ÿ'I'Pÿ ')tÿ, 19 ff,ÿ/o ,

-- -

5. How much iron can be recovered from 25.0 g Iron (III)'Cÿxld{? -- ' :_

6. Which of the following compounds has the greatest mass percent of oxygen?-• Nickÿ__ÿate. . Li .s (o,,Cill X5

0_, -- fÿ,oi X,3-: :1go3/

aq] ,$I]

<. ,go,'7ÿ'-/

0 ÿ tS, lqclÿ(q ; ÿ1ÿ7t3li5,793L"

7. Find the percÿent composition of a compoundtÿ has 2.62 g Na and 4.04 g CI.

NOTES: Empirical

• Empirical formula:

0

0

Formulas

e.g., CH20 or CH

!lJ t lÿ be reduced. May or may not exist in this form in the real world.

o e.g.,C2H40z or C6H6

o UJi II n0%"

rÿo oÿ ,bÿ crÿn

be reduced. Formula describes a substance as it actually exists.

Empirical or Molecular? (Remember that for some compounds, its empirica/ formula can a/so be its mo/ecu/arformu/a.)

• NaÿO ÿ_ÿ ÿ ÿ0ÿ • KzS04 ÿ ÿ iÿ)ÿI-

Which pair has the same empirical formula?

Calculating an Empirical Formula

1. Determine the ÿq0ÿ3ÿ of each ÿ::ÿlÿm/ÿ21 Convert the mass of each to ÿ0ÿ . ©

3. Find the iÿrÿ!ÿ to ÿqoÿ,ÿ, r(ÿoÿ of each element by dividing thenumber of moles of each element by the ÿ/]rÿlÿ[ÿ number of moles.

4. If the ratio is not a II ÿ number, multiply each ratio by a factor to

..rÿfiÿ ÿ,ern ÿiÿ| ÿ numÿ5. Write the formula using the mole ratio as the ,ÿt(/hÿÿ for the formula.

Find empirical formula of 69.5% O & 30.5% N.Step i: Divide % or grams by its atomic mass to get moles of each element.

69.5ÿO lmoleO = 4.344 moleO 30.5ÿN lmoleN = 2.177 moleN15.9999 O 14.0779 N

Step 2: Divide smallest mole numÿn each element to get ratio oÿ that element.4.344 moleO = 2.177 mole N =

i-n j !I

* This answer becomes the subscript for that element; round to nearest whole number if .8 or higher.ANSWER = ÿ

19

INDEPENDENT PRACTICE:1. Analysis of a compound shows that it contains 10188g of calcium and 19.07g of chlorine. Determine the

empirical formula of this compound.

. One of the most commonly used white pigments in paint is a compound of titanium and oxygen that contains

5.99 g titanium by mass and 4.01g oxygen by mass. Determine the empirical formula and name for t)!ÿiÿi]ÿ],ÿ:compound. : I ÿ-ÿÿ ÿ, \/ o a lo j , ?:i J

, Used in the production of nylon, a dipic acid is an organic compound composed of 49.31% C, 43.79% O, andthe rest is hydrogen. Determine the empirical formula of adipic acid.

C : ,tÿi,31 ilÿ ÿlJ - ÿt,ÿ05/ÿ ÿ37 ,,150 - Dffs.7.1ÿ:i/asÿi<:ÿi-ÿ.Tj7/ÿ.-,D7 ÿ #

i4: (o ,9/I,OOÿ : Q'IDqS/°] -la-7 ÿ,DO 650,ÿ5

Calculating Molecular Formulas

• The molecular formula will have the ÿ ÿ)

• To determine a molecular formula, we wÿ, iÿquiLipiÿ

• ]'GltJ, to by a whole number factor i'ÿ/NF).

the

as the empirical formula.

c,rÿ,md

i

20

1. Empirical Formula = P20ÿ

Molar Mass= 283.88 g/tool

What is the molecular formula of this compound?

15,111 X 5:1':/'I'5

. Nitrogen and oxygen form multiple molecular compounds together. One of these compounds is used to fuelspace shuttles and has the empirical formula NOÿ.what is the molecular formula?

If the molar mass of this compound is 92.02 g/tool,

: iq,Od7 : Iq, OO7 . ÿ (ÿ: i5,':/%,9-: dJ,!ÿ ÿ,ÿ

3. Butane is commonly used in lighters. It is composed of n. It has a molarmass of 58.17 g/tool. What is the molecular formula of butane.

. LUuF: 51},ÿ1 . a4

Homework: Empirical and Molecular Formulas

What is the empirical formula (lowest whole number ratio) of the compounds below?1) 74.9% carbon, 25.1% hydrogen ÿ ..

2)

O:

32.4% sodium, 22.5% sulfur, 45.1% oxygen _ ÿ Pl

What is the molecular formula (whole number multiple ratio) of the compounds below?4) A compound is 64.9% carbon, 13.5% hydrogen and 21.6% oxygen. Its molecular mass is 74 g/mol,. Vÿat iÿ its

¢-cti, l/r,,e?, :- 5,ÿ0D/!:07. ;Ftÿ-/3, 51i,00s : iÿ:D<t$/#'aÿ " g.%-ÿt< 55jt, 5D - t °ÿ 15ffiÿj ÿÿ+0_O:al,/o/i$, 77-/, " -7ÿ.Ja5

wÿF:-ÿ'71--l<i - 1 G i-I,oO + ÿ1-t,ÿ5) A compound is 54.5% carbon, 9.1% hydrogen, and 36.4% oxygen. Its molecular mass is 88 g/tool. What is its

molecular formula? -- "

.-o/c>

_ lm ' 1--- d,t<f I -D, ÿ

6) The empirical formula of a compound is NO2, Its molecular mass is 92 glmol, What is its molecular formula?

o®ÿ: qa -st% /dÿOi

The compound methyl butanoate smells like apples. Its percent composition is 58% C, 9.8% H, and 31.4% O. Ifwhat is its molecular formula?

i

.:-.(: Academic Chemistry Unit-5 Test Review: Oue :ÿ/i1ÿ. Chemicaÿ Quantities & The MoUe TEST on ÿ-tÿ:ÿlÿ

4 ", Problems: For'the following problemso show all work and report your answers with thecorrect units and significant figures.

I. What is the molar mass of Bat03? <ÿBÿ- ( ÿ 13'ÿ7"ÿ Zÿ" ÿ19ÿ7• :ÿ ?

O- 3,,ÿ j'b.qeq" dÿ-Gq72. In one molecule of Pz05, how many phosphorous atoms are present7 _ÿ

, List all seven diatomics: ÿ - "ÿ

baa_ ,ÿ ©:'-! ÿa. ,, Ct,_, !

, Calculate the percent composition of Ca(OH)z.

Prr--- ÿ, oog ÿ, 9- ÿ O.

5. Calculate the percent composition of

6. How many atoms of carbon are in 3.6 moles of carbon?

i"{

, Determine the number of moles of hydrogen that are in 362.8 g of this eleme .

d. Ol( 3 14o-.8, A chemical reaction produces 13,8 tool of carbon monoxide gas. What volume will the gas occupy at STP?

, What is the moss of 5,0 X 10Zÿformula

5. o X 0

units of Fe(NOÿ)ÿ?

i0. Hÿw many liters are there in 5.25 9 dOz at STP?

,o1 f' L Doq.

zi. How many grams of Ne are there in 5.5 moles of the gas?

12. Nomenclature ReviewName the following compounds Write the formulas for the following compounds.

a. dinitrogen tetroxide_ ÿ ÿ..ÿ-

c. calcium nitrate - ÿ./

d. strontium bromide ¢ÿ._

f. pgÿBLntaphosphorus deÿcoxide

i4. Define empirical formula.

i5. Define molecular formula.

or acÿk t44ÿ o 0€Oolÿou v,A

i6. Find the empirical formula for the following substances (a. and b.) using the information given:a. 4 compound is composed of 38.67% potassium, i3.85% nitrogen, 47.48% oxygen. What is the

empirical formula?

d!/

H

gÿ..b°

formule?

qq. s J_kmgL2 1 30. qqq ÿ g

q3taÿ

0ÿ__

A compound is made up of 44.33% phosphorus and 57.18% oxygen- what is the empirical

• _ÿ ÿ ÿ_ ÿiL

17. Determine the molecular formula for each of these compounds.a. empirical formula = CHzO; the molar mass = 90 g/real ,-ÿ,

b. empirical formula = HgCl; momr,ÿss = 472.2 g/m .ÿÿ...ÿ

, ÿ- 2.00.5°< .ÿ ÿ -; ÿ%oo.e4 (/dtqF-- q'72.>0 .r.ÿ opoÿfY[ÿff ,

18. The action of bacteria on meat and fish produces a poisonous compound calledÿÿSname and origin imply, it stinks] It is 58.77% C, !3.81% H, and the remainder is Nitrogen. Its molarmass is :102.2 g/real. Find itsempirical and molecular formula. (Hint: Find the empirical formula

¢0 , ÿ o

aootl@C

t

• - :-: . .: . ".. -. , . _::: :-::!::.:"ÿ::":: " )..:::.i-: P:::-. :.-: : :< :, ÿ .............. . .