I. TITLE

Nitrogen and Ammonia

II. DATE OF EXPERIMENT

Wednesday, November 26th 2014

III. EXPERIMENT DONE

Wednesday, November 26th 2014

IV. PURPOSE

a) Knowing how to prepare nitrogen and ammonia gas in laboratory

b) Knowing the properties of nitrogen and its compound

c) Knowing the gas of nitrogen, ammonia, the compound

V. BASIC THEORY

1. NITROGEN

Nitrogen is a non-metallic element in the periodic table is in group VA or

group 15 and has the symbol N with atomic number 7. At room temperature in the

form of gas is colorless, odorless, tasteless and form diatomic element (N2).

Nitrogen disbursed also colorless and odorless.

Image molecular formula nitrogen and liquid nitrogen

Nitrogen is very difficult to react with other elements or compounds that is

also called nitrogen. Nitrogen is the most gas in the atmosphere is about 78%. In

addition to the atmosphere, nitrogen is also found in Mars (3%).

The chemical bond between two atoms in a molecule of nitrogen is the

strongest bond between two atoms of the same element. This makes N2 gas is very

stable and inert. In the body tissues of living beings, some containing nitrogen, for

example in proteins and nucleic acids into one of the fundamental building blocks

of DNA and RNA.

There are two stable isotopes of nitrogen, namely: 14N and 15N. Isotopes most

is 14N (99.634%), which is produced in stars and the rest is 15N. In industrial

nitrogen obtained from the air liquefaction with a high enough pressure, followed

by fractional distillation or fractionation distillation. When nitrogen is heated, can

react directly with magnesium, lithium and calcium.

6Li + N2 → 2Li3N

3Mg + N2 → Mg3N2

When mixed with oxygen and subjected to electric sparks, forming nitric

oxide (NO) then becomes dioxide (NO2). When heated under pressure with

hydrogen and the presence of a suitable catalyst will form ammonia (Haber

process).

Nitrogen compounds are widely used in industry and in the laboratory such as

nitric acid and ammonia (at most in the industry). Ammonia, NH3 is toxic nitrogen

hydride and the most important base material for chemical nitrogen and is one of

the chemicals most widely produced in the world. Ammonia is used as a base

material such as urea nitrogen fertilizers and explosives.

NITROGEN COMPOUNDS

Sodium nitrate (NaNO3) and potassium nitrate (KNO3) is formed by the

decomposition of organic materials with the metal compounds. In dry conditions in

beberapat place, saltpeters (salt) is found in sufficient quantities and used as

fertilizer. Inorganic nitrogen compounds other is nitric acid (HNO3), ammonia

(NH3) and oxides (NO, NO2, N2O4, N2O), cyanide (CN-), etc. Nitrogen cycle is one

of the important processes in nature for living organisms. Although nitrogen gas

does not react, the bacteria in the soil can fix nitrogen into a useful form (as a

fertilizer) for plants. In other words, nature has provided a method for producing

nitrogen for plant growth. Animals then eat these plants where nitrogen was

contained in their system as proteins. The cycle is complete when other bacteria-

bacteria convert the waste nitrogen compounds to nitrogen gas. As a major

component of proteins, nitrogen is an essential ingredient for life.

PREPARATION NITROGEN IN LABORATORY

In the laboratory, nitrogen is prepared by heating a mixture of ammonium

chloride and sodium nitrite and a little water. If ammonium nitrite heated

decomposes produce nitrogen gas. However, this reaction is very fast and may be

explosive.

For security, campukan ammonium chloride and sodium nitrite with a mass

ratio of 4: 5, and then heated with a little water. The presence of water to prevent

ammonium chloride mensublimasi when heated. Initially, the two substances

undergo double decomposition to form sodium chloride and ammonium nitrite.

Ammonium nitrite formed then decomposes into nitrogen gas and water.

Nitrogen gas formed later flowed through the water like in the picture. In this

way, the moisture will be left behind while the nitrogen gas continues upward

because of their low solubility in water.

PHYSICAL AND CHEMICAL PROPERTIES OF NITROGEN

Having an atomic mass = 14.0067 amu

Has the atomic number = 7

Boiling point = -1960C

Freezing point = -2100C

Have atomic radius = 0.920 A

Having a Configuration [He] 2s2 2P3

In compounds have an oxidation number -3, +5, +4, and +2.

Has the atomic volume = 17.30 mol / cm3

Has a hexagonal structure

Has a density = 1.2151 g /cm3

Has a heat capacity = 1.042 J /gK

Ionization energies have to-1 = 1402.3 kJ / mol

Have ionization energies 2nd = 2856 kJ / mol

Have ionization energies 3rd = 45 781 kJ / mol

Have electronegativity value = 3.04

Heat conductivity = 0.02598 W / Mok

Having a price enthalpy = 0.36 kJ / mol

Prices have bentalpi evaporation = 2,7928kJ / mol

Relative Density = 0.967

Molecular Weight = 28.013

Critical temperature = -147.1°C

Gas Specific Gravity (@ 101.3 kPa and 15°C) = 1,170 kg /m3

Solubility in water (@ 101.3 kPa and 20°C) = 0.016 cm3 /cm3

In the form of gas is colorless, tasteless, odorless, and non-toxic.

Volatile

Not reactive

Is diamagnetic

Electronegative highest in the group.

SOURCES OF NITROGEN

Nitrogen gas (N2) is contained as much as 78.1% in the air. For comparison,

the atmosphere of Mars contains only 2.6% nitrogen. Of the earth's atmosphere,

nitrogen gas can be produced through the process of liquefaction (liquefaction) and

fractional distillation. Nitrogen is found in living organisms as part of biological

compounds.

NITROGEN ABUNDANCE

Nitrogen is present in nature as a free element in the form of diatomic

molecules (N2) approximately 78.09% by volume of the atmosphere. Found in

essential minerals such as (KNO3), and Chile saltpeter (NaNO3). In plants and

animals, nitrogen in the form of the protein that forms the average composition of

51% C; 25% O; 16% N; 7% H; 0.4% P; and 0.4% S.

2. AMMONIA

Ammonia is a chemical compound with the formula NH3. These compounds

are usually found in the form of a gas with a pungent odor characteristic (called

ammonia smell). Although ammonia has a significant contribution to the presence

of nutrients in the earth, ammonia itself is a caustic compound and can be harmful

to health. Occupational Safety and Health Administration of the United

PekerjaanAmerika give a 15 minute limit for contact with ammonia gas

concentration of 35 ppm in volume, or 8 hours to 25 ppm volume. Contact with

high concentration of ammonia gas can cause lung damage and even death.

Although ammonia in the US is set as non-flammable gas, ammonia is classified as

a toxic substance by inhalation, and transport of ammonia amounted to greater than

3,500 gallons (13,248 L) must be accompanied by a license.

Ammonia is used commercially called anhydrous ammonia. This term

indicates the absence of water in the material. Because ammonia boils at a

temperature of -33 ° C, liquid ammonia must be stored in high pressure

atautemperatur very low. However, very high evaporation heat so it can be handled

with the usual reaction tubes in the smoke hood. "Ammonia home" or ammonium

hydroxide is a solution of NH3 in water. The concentration of the solution is

measured in units of Baume. Concentrated solution of ammonia commercial

products usually have a higher concentration of 26 degrees Baume (about 30

percent by weight ammonia at 15.5°C). Ammonia which is in the house usually has

a concentration of 5 to 10 percent by weight ammonia. Ammonia is generally

alkaline (pKb = 4.75), but can also act as a very weak acid (pKa = 9.25).

THE PROPERTIES OF AMMONIA

The properties of ammonia are as follows:

a. Ammonia is a colorless gas and smells very stimulating so that the gas is

easily recognized by smell.

b. Very soluble in water, which is the default state, 1 liter of water dissolved in

1180 liters of ammonia.

c. Gas is easy to melt, liquid ammonia freezes at -78oC and boils at -33oC.

THE PREPARATION OF AMMONIA

a. In medieval times, the manufacture of ammonia by heating the horns and

hooves of cattle.

b. Until the time of World War I, the manufacture of ammonia by the United

States through the cyanamide process, as follows:

At first stone quicklime (CaO) and coal (C) is heated in an electric furnace

to obtain calcium carbide (CaC2).

CaO (s) + 3 C (s) CaC2 (s) + CO (g)

Then, calcium carbide flowed nitrogen gas (N2) to form calcium

cyanamide (CaCN2).

CaC2 (s) + N2 (g) CaCN2 (s) + C (s)

Finally, calcium cyanamide flowing water vapor to produce ammonia.

CaCN2 (s) + 3H2O (g) CaCO3 (s) + 2NH3 (g)

c. Since World War I to the present.

Ø The Haber-Bosch process

Between 1908 until 1913, Fritz Haber (1868-1934) of Germany succeeded

in synthesizing ammonia directly from the elements, namely of nitrogen gas and

hydrogen gas. Then the process of ammonia formation is enhanced by his

compatriot, Karl Bosch (1874-1940) with a high-pressure method so that the

manufacture of ammonia is known as the Haber-Bosch process. This process is

urgent because the cyanamide process Haber-Bosch process is the manufacture

of ammonia cheaper. In the Haber-Bosch process, the raw material in the form

of N2 and H2.

N2 obtained from the fractional distillation of liquid air

H2 is obtained from natural gas (methane) which flowed along the water

vapor with nickel catalyst at high temperature and high pressure.

CH4 (g) + H2O (g) CO (g) + 3H2 (g)

CO (g) + H2O (g) CO2 (g) + H2 (g)

Manufacture of ammonia by the Haber-Bosch process is an exothermic

equilibrium reaction which takes place at a temperature of about 400-600oC and

a pressure of about 200-600 atm.

N2 (g) + 3H2 (g) 2NH3 (g) ΔH = -92 KJ

Ø In the laboratory

In the laboratory, NH3 can be derived from:

Nitride plus water

Mg3N2 (s) + 6 H2O (l) 3Mg (OH) 2 (aq) + 2 NH3 (g)

Ammonium chloride + strong base

NH4Cl (s) + NaOH (aq) NaCl (aq) + H2O (l) + NH3 (g)

2NH4Cl (s) + Ca (OH) 2 (aq) CaCl2(aq) + 2H2O(l) + 2NH3(g)

VI. TOOLS AND MATERIALS

Tools

No Tools Amount1234567891011121314

Erlenmeyer flask 100mLFlute flaskMeasuring glass 100mLSeparation funnelTripod and kassaStatif and clampBunsen burnerTest tubeDrop pipetteMeasuring glass 250mLVesselStirrerBalanceRubber

121111131011112

Materials

No Materials Amount1234567891011121314151617

A piece of woodNaNO3 crystalNH4Cl crystalConcentrated HCl solutionCa(OH)2

Amylum solutionKI solutionConcentrated ammonia solutionH2S gas(from HCl and pirit)Concentrated H2SO4 solutionH2SO4 solution FeSO4 solution Concentrated HNO3 solutionHCl solution PP indicatorNH4OH Sulfur flower

1M, 0.1M0.2M

0.1M

2M, 0.1M

VII. PROCEDURE

- Entered into porcelain cup

-Flush with disttilled water-Observed

-Checked with litmus paper

Red litmus paper turns blue

A few pieces of calcium

White powder

White solution

-Entered into porcelain cup containing aquadest

-Heated over a flame

-Checked by PP-Observed

Small spoon of magnesium powder

Pink solution

The powder does not dissolve

Slightly soluble water

-Entered into test tubes containing wet and dry cotton -Entered dry cotton-Closed the test tube with a rubber cap-Heated

-Tested flameFormed gas bubbles

0,02 gram of zinc powder

Gray powder

Arise burst

Some zinc metal

-Entered in tube side piped-Hose conected to a container measuring cup placed upside down in the water-Added 4M solution of hydrochloric acid sufficiently

-Closed with a rubber cover -Tested flame

Hydrogen Experiment

1.

2.

3.

A few drops of solution H2O2 4,5%

-Entered into test tube-Added 1mL KI

-Added a little starch solution-Observed

The solution changed purple

Yellow solution

Potassium Chlorate

-Inserted into the test tube as high as ±0,5 cm from the bottom of the tube

-Added a little powder manganese

-Heated

-Collected gas by moving into water-Tested with sticks glow

Fire the greater

White powder

White powder and black

Black powder melts, gases arising

4.

5.

6.

- Entered into porcelain cup

-Flush with disttilled water-Observed

-Checked with litmus paper

Red litmus paper turns blue

A few pieces of calcium

White powder

White solution

VIII. DATA OF EXPERIMENT

No. PROCEDURE RESULT REACTION CONCLUSION

1

Hydrogen Experiment Before :

Calcium: white

powder

Litmus paper: red

After :

Added aquadest: the

powder doesn’t

dissolve

Red litmus paper

become blue

Arise H2 gas

Ca(s) + 2H2O(l)

Ca(OH)2(aq) + H2(g)

Calcium metal added water

produces hydrogen gas and it’s

basic solution

Small spoon of magnesium powder

Pink solution

The powder does not dissolve

Slightly soluble water

-Entered into test tubes containing wet and dry cotton -Entered dry cotton-Closed the test tube with a rubber cap-Heated

-Tested flameFormed gas bubbles

0,02 gram of zinc powder

Gray powder

Arise burst

2

Before :

Magnesium powder:

grey

PP indicator: colorless

After :

Added aquadest:

magnesium doesn;t

dissolve

Heated: arise H2 gas

Added PP indicator:

solution become pink

Mg(s) + 2H2O(l)

Mg(OH)2(aq) + H2(g)

Magnesium metal added water

produces hydrogen gas and it’s

basic solution

3

Before :

Zinc powder: grey

Cotton: white

After :

After heated: grey and

arise H2 gas

Tested the flame:

arise burst and the

volumeof gas is 67

mL

Zn(s) + 2H2O(g)

Zn(OH)2(aq) + H2(g)

Heating Zn powder that are on

the wet cotton produces

hydrogen

Arise burst

The solution was gray, arise bubble

A few drops of solution H2O2 4,5%

-Entered into test tube-Added 1mL KI

-Added a little starch solution-Observed

The solution changed purple

Yellow solution

4

Before :

Zn powder: grey

HCl 4M: colorless

After :

Added HCl: doesn’t

dissolve, grey

solution and arise H2

gas

Tested flame: arise

burst and the volume

of gas is 10 mL

Zn(s) + 2HCl(aq) ZnCl2(aq)

+ H2(g)

The reaction between metallic

Zn with HCl produces hydrogen

gas with a volume is 10 mL

5

Before:

H2O2 solution:

colorless

Ki: yellow solution

Starch/amylum:

colorless

After:

H2O2+KI: colorless

Added amylum:

purple solution

2KI(aq) + H2O2(aq)

2KOH(aq) + I2(aq) + H2(g)

The reaction between Ki with

H2O2 produces hydrogen gas and

occur oxidation where I- I2

Potassium Chlorate

-Inserted into the test tube as high as ±0,5 cm from the bottom of the tube

-Added a little powder manganese

-Heated

-Collected gas by moving into water-Tested with sticks glow

Fire the greater

White powder

White powder and black

Black powder melts, gases arising

6

Before:

Potassium chorate:

colorless

Magnesium powder:

black

After:

Heated: gas arise with

volume >100 mL

Tested with sticks

glow: fire the greater

2KClO3(s) + 2MnO2(s)

KCl(aq) + 4O2(g) +

2KClO4(aq)

The reaction between KClO3

with MnO2 produces oxygen gas

with a volume >100mL.

±0,5 gram of permanganate

-Entered in test tube an connected to the piped side container

-Added drops by drop 4,5% hydrogen peroxide (with caution)-The tube was closed with a rubber cover

-Left about 10 minutes for the gas to accumulate -Tested with sticks glow-Compare with the experimental gas volume 1

Greater flame

purple- black powcer

purple solution, gas arising

7

Before:

Permanganate:

purple-black powder

H2O2: colorless

After:

Permanganate +

H2O2: purplish black

solution, O2 gas arise

and the volume is 10

mL

Tested flame: greater

flame

KMnO4(s) + 2H2O2(aq) K+

(aq) + Mn2-(aq) + 3O2(aq) +

3H2O(l)

The reaction between

permanganate with hydrogen

peroxide produces oxygen gas

with a little volume.

IX. ANALYSISExperiment I

The experiment is covertly designed to make nitrogen gas in the laboratory .As

many as 0.3 grams NaNO2 dissolved in 10 mls of aquades .In a separating funnel put 0.3

grams NH4Cl aquades in 10 mls . Next instrument composed such a picture .

Flasks heated above the burner spiritus, after nearly boiling tap on separating

funnel is opened so that a solution of NH4Cl out and mixed with NaNO2 form nitrogen gas

and a solution of NaCl and H2O according equation:

NaNO2(aq) + NH4Cl(aq) NaCl(aq) + N2(g) + H2O(l)

The establishment of proven by the emergence of gas bubbles then sent through a

tube into a measuring glass filled to the water full of reverse , as time passes gas that

forms flowing through a tube and entering into reverse a measuring glass filled to the

brim water .The more gas that forms will be pressing the water in glass measurement for

out so that a measuring glass filled by gas that forms .The volume of gas that forms is

mls of 146 .Next gas that forms in a test with a burning wood , and fire

extinguished .This shows that gas that forms are gaseous nitrogen having the character of

extinguish the fire .

Experimen II

The second experiment aims to create NO gas in the laboratory. A total of 2.5 g

NaNO2 dissolved in 2.5 mls of water. Then NaNO2 solution was divided into two and put

into a test tube. In the first tube was added 1 M H2SO4 and the resulting solution was

colorless and white steam.

2NaNO2(aq) + H2SO4(aq) Na2SO4(aq) + HNO2(aq)

While the tube 2 solution was diluted 4 times to further reduce the concentration of

NaNO2 solution of KI and starch plus colorless solution after solution of H2SO4 plus

purple. H2SO4 fun ctions as an oxidant that will oxidize NaNO2 be NO. While the function

of the addition of KI and starch is an indicator that NaNO2 been oxidized to NO, because

H2SO4 will also oxidize KI be I2. At the time of I2 formed the NO gas has also been

established. Starch is an indicator I2 if I2 is formed then the purple solution.

2NaNO2(aq) + 2KI(aq) + 2H2SO4(aq) Na2SO4(aq) + K2SO4(aq) + 2H2O(l) + 2NO(g) +I2(aq)

Experiment III

In this experiment aims to create a complex compound of the element nitrogen.

The first solution of dilute HNO3 plus concentrated H2SO4 as much through the tube wall

then raised steam and hot, which indicates an exothermic reaction while the vapor formed

is NO gas. Furthermore, the added 0.2 mls of 0.2 M FeSO4 solution became yellow and

formed a ring rolled. Function H2SO4 is oxidator that oxidize HNO3 be NO and oxidizing

Fe2+ being Fe3+. Rolled rings are complex [Fe(NO)]2+ is the reaction between Fe2+ with NO.

2NO3- + H2SO4(aq) + Fe2+(aq) 2NO(g) + 4SO4

2- + 6Fe3+(aq) + 4H2O(l)Fe2+(aq) + NO(g) [Fe(NO)]2+(aq)

Experiment IV

This experiment was to prove that the ammonia can react with sulfur. As many as 1

mL NH4OH then irrigated with gas H2S solution remains colorless.

NH4OH(aq) + H2S(g) (NH4)2S(aq) + H2O(l)Furthermore, the solution coupled with sulfur flowers and filtered, a yellow

precipitate formed, the function of the addition of sulfur flowers is to add namesake that

S2- ions thus lowering the solubility of (NH4)2S.

(NH4)2S(aq) + S(s) (NH4)2S(s)

After that, coupled with dilute HCl, the precipitate dissolved. The function of HCl

is to increase the solubility.

(NH4)2S(s) + HCl(l) 2NH4Cl(aq) + H2S(g)

Experiment V

In this experiment aims to create and test the presence of ammonia gas. Solution

NH4OH 4M coupled with the tip of a small spoon of Ca(OH)2 and then heated. When

heated in ammonia gas formation was tested with red litmus paper wetted tube that is

placed in the mouth, red litmus turned blue which indicates is basic ammonia gas.

Function moistened litmus paper is as litmus paper can not react ith gas if dry, H 2O will

react with NH3 gas that can change color to blue litmus paper red. After the spatula that

has been dipped in concentrated HCl and the resulting insert the tube into the white mist

which is NH4Cl.

NH4Cl(aq) + Ca(OH)2(s) NH3(g) + 2H2O(l) + CaCl2(aq)NH3(g) + HCl(aq) NH4Cl(aq)

Experiment VI

In this experiment aims to create and test the presence of ammonia gas. Put of 5

mls of concentrated ammonium hydroxide into Erlenmeyer flask 100 mls and then in the

lid and connected by a hose. Furthermore heated, when heated hose connected with an

empty test tube and then tested with a spatula dipped in concentrated HCl, white mist

arises, this indicates that the gas formed is correct NH3 gas.

Then the hose is connected to the tube containing water which has the added PP,

water previously turned into a pink color that indicates the solution is base.

NH4OH(aq) NH3(g) + H2O(l)

NH3(g) + HCl(aq) NH4Cl(aq)

NH3(g) + H2O (l) NH4OH(aq)

X. CONCLUSIONFrom the experimental results we can conclude that

1. Nitrogen gas laboratory can be prepared by reacting a solution of NaNO2 with

NH4Cl solution through a process of heating and ammonia gas in the laboratory

can be made by heating the concentrated NH4OH.

2. The nature of the nitrogen gas is a colorless gas, odorless, flammable and non-toxic

absolute.

3. Nitrogen gas can be identified with the extinguished embers, ammonium gas can

be identified by the smell of urine that sting and the addition pp which produces a

pink solution, and moistened spatula HCl will produce white white mist, and can

change the color of litmus red to blue .

REFERENCES

Habsyi, Nunna. 2012. Senyawa Amonia.

http://nunaahabsyi.blogspot.com/2012/12/senyawa-amonia-nh3_9.html. Accessed

on 28 November 2014.

Rizky, Muhammad. 2012. Unsur dan Senyawa Nitrogen.

http://muhammadrizky17.wordpress.com/2012/03/23/unsur-dan-senyawaan-

nitroge/. Accessed on 28 November 2014.

Seran, Emel. 2012. Nitrogen, Asam Nitrat, dan preparasi Nitrogen dalam Laboratorium.

http://wanibesak.wordpress.com/2012/01/07/nitrogen-asam-nitrat-dan-preparasi-

nitrogen-dalam-laboratorium/. Accessed on 28 November 2014.

Tim Penyusun. 2014. Penuntun Praktikum Kimia Anorganik II Unsur-Unsur Golongan

Utama. Surabaya: Jurusan Kimia UNESA.

Usman, Zaini. 2012. Amonia. http://zainiusman6.blogspot.com/. Accessed on 28

November 2014.

Vogel. 1985. Buku Teks Analisis Anorganik Kualitatif Makro dan Semimakro, Jakarta :

PT. Kalman Media Pusaka.

ANSWER QUESTIONS

1. Describe the manufacture of nitrogen and ammonia in the lab!

Nitrogen gas is made by heating the azide compounds, such as sodium azide (NaN3) and

barium azide (Ba(N3)2). Heating produces nitrogen gas and sodium metal:

2NaN3 2Na + 3N2

Moreover, it can also be obtained from the slowly heating a solution of ammonium nitrite

(NH4NO2)

NH4NO2 2H2O + N2

Ammonium nitrite is used, prepared by reacting sodium nitrite and ammonium chloride:

NaNO2 + NaCl + NH4ClNH4NO2

Ammonia is made by reacting ammonium chloride with a strong base (alkaline oxide).

NH4Cl + NaOH NH3 + NaCl + H2O

2NH4Cl + CaO + H2O2 NH3 + CaCl

The gas produced can be determined by testing using litmus paper. Alkaline ammonium gas

that will change the color of litmus paper from red to blue.

2. Explain the chemical properties of nitrogen!

In the form of gas is colorless, tasteless, odorless, tasteless, and nontoxic.

Volatile, non-reactive. Is diamagnetic, electronegative highest in the class.

Most common diatomic nonmetal.

Has five electrons in its outer shell, so that the trivalent in most compounds.

3. Write the equation for all the experiments above!

The first experiment

NaNO2 (aq) + NH4Cl (aq) NaCl (aq) + N2 (g) + 2 H2O (aq)

The second experiment

The first tube:

NaNO2 (aq) + H2SO4 (aq) → Na2SO4 (aq) + 2 HNO2 → H2 (g) + 2NO2 (g) brown

The second tube:

2NO2- (aq) + 4H + (aq) + 2I- H2O (aq) + I2 (aq) + NO ↑ (g)

2NaNO2 (aq) + 2KI + (aq) + H2SO4 (aq) → Na2SO4 (aq) + I2 (aq) + NO ↑ (g)

The third experiment

HNO3 (aq) + H2SO4 (aq) + FeSO4 (aq) 2NO (g) + 3Fe2(SO4)3 (aq) + 4H2O (aq)

FeSO4 (aq) + NO ↑ (g) [Fe (NO)]SO4 (aq)

The fourth experiment

FeS (s) + 2HCl (aq) → FeCl2 (aq) + H 2 (g)

NH4OH (aq) + H2 (g) → (NH4)2S (aq) + H2O (l)

(NH4)2S (aq) + H2O (l) + S (s) → (NH4)2S (aq) + H2O (l) + S (s)

(NH4)2S (aq) + HCl (aq) NH3 (g) + H2 (g) + H2O (aq)

The fifth experiment

2NH4Cl (aq) + Ca(OH)2 (s) 2NH3 (g) + 2H2O (aq) + CaCl2 (S) (white precipitate)

NH3 (g) + HCl (aq) NH4Cl

The sixth experiment

NH4OH (aq) NH3 (g) + H2O (aq)

NH3 (g) + PP + aquadest pink solution

NH3 (g) + HCl (aq) NH4Cl

4. Mention ammonium usability!

Ammonium have some benefit in human life, among others:

Salts (usually in the form of NH4NO3 or NH4SO4) is widely used in industry as raw

material of nitrogen fertilizer.

Ammonium chloride (NH4Cl) used in dry battery (cell Leclanche).

Diammonium phosphate ((NH4)2HPO4) and ammonium dihydrogen phosphate

(NH4H2PO4) is used in fertilizers, fire-resistant coating on wood, paper and garments.

NH4ClO4 used as an oxidizing agent in the solid fuel rocket. 

ATTACHMENT

First experiment

Second experiment

Preparation nitrogen gas

NaNO2 + aquadest Test tube 1: added H2SO4

Test tube 2: added aquadest

Test tube 2: Added KI & amylum

Test tube 2: Added H2SO4

Third experiment

Fourth experiment

Fifth experiment

Dilute HNO3 + conc. H2SO4

Added FeSO4

NH4Cl + Ca(OH)2 + heated

Put spatula that dipped in conc. HCl

Added HCl

Sixth experiment

Preparation amonia gas

Gas + aquadest + PP indicator