report experiment 1 chemical reactions

GENERAL CHEMISTRY LABORATORYChemical reaction is a process in which one or more substances, the reactants, are converted to one or more different substances, the products.. A chemical re

EXPERIMENT 1: CHEMICAL REACTIONS

Group: 2 Section: _1 _ Date: 13 June 2020rd

Group members:

Seq

Full name Student ID contribution (%) Signature Score

1 Nguyễn Như Thiên Nhã IELSIU19223

2 Phan Quốc Khánh IELSIU19176

3 Nguyễn Khai Nguyên IELSIU19218

4 Đoàn Lưu Kim Ngân IELSIU19211

5 Phạm Bảo Trâm IELSIU19078

Total score: _/15

I Introduction

GENERAL CHEMISTRY LABORATORY

Chemical reaction is a process in which one or more substances, the reactants , are converted to one or more different substances, the products Substances are either chemical elements or compounds A chemical reaction rearranges the constituent atoms of the reactants to create different substances as products In this first experiment, there are 25 chemical reactions and 1 flame test By observing phenomenon

of each reaction, products can be identified through 5 different types of chemical reactions, these are: Synthesis (combination), Single replace-ment, Double replacereplace-ment, Decomposition and Combustion The pur- pose of this Chemistry Laboratory is to study the way to discover the identity of a product through observing the reaction and write a lab re-port about experiments of inorganic and organic substances.

II Experimental

1 Reactions of Cu 2+

0.5M CuSO 4

+ 2M NaOH

Appear greenlish blue precipate Cu(OH)2

CuSO4 + 2NaOH → Cu(OH) ↓ + 2

Na SO2 4

0.5M CuSO 4

+ 2M NH 4 OH

Appear greenlish blue precipate Cu(OH)2

CuSO4 + 2NH OH → Cu(OH) ↓ +4 2

(NH SO4)2 4

Comments:

These are double replacement reactions as there are an exchange in ions of two

different compounds

Ionic equation:

Cu 2+ + OH → Cu(OH) ↓

-2

2 Reactions of silver halides

GENERAL CHEMISTRY LABORATORY

0.5M KCl

+ 0.1M AgNO 3

White precipitate

0.5M KCl

+ 0.1M AgNO 3

+ 2M NH 4 OH

First, white precipitate appeared Then, it was dissolved in the solution

KCl + AgNO → KNO + AgCl↓3 3

AgCl + 2NH OH → Ag(NH Cl 4 3)2

+2H O2

0.5M KBr

+ 0.1M AgNO 3

Light yellow precipitate appeared KBr + AgNO → KNO + AgBr↓3 3

0.5M KBr

+ 0.1M AgNO 3

+ 2M NH OH

Yellow precipate become white precipate

KBr + AgNO → KNO + AgBr↓3 3

AgBr + 2NH OH → Ag(NH Br 4 3)2

+2H O

0.5M KI

+ 0.1M AgNO 3

Light yellow precipitate appeared KI + AgNO → KNO + AgI↓

0.5M KI

+ 0.1M AgNO3

+ 2M NH 4 OH

Light yellow precipitate appeared

KI + AgNO → KNO + AgI↓3 3

AgI + NH OH → No reaction4

Comments:

These are double replacement reactions as there are an exchange in ions of two different compounds

Ionic equation:

Ag+ + Cl- → AgCl↓

Ag+ + Br- → AgBr↓

Ag+ + l- → Agl↓

GENERAL CHEMISTRY LABORATORY

3 Reactions of H 2 O 2

0.1M KMnO 4

+ 2M H 2 SO 4

+ H 2 O 2

The purple solution KMnO4 lost the color, effervescence appeared

2KMnO4 + 3H2SO4 + 5H O2 2 → 5O + 2 2MnSO4 + K2SO4 + 8H O2

0.1M KI

+ 2M H 2 SO 4

+ H 2 O 2

First produce light yellow fluid Then H2O2 make black precipitate appeared

2KI + H2SO4 + H2O2 →

K SO2 4 + I2↓+ 2H O2

H O 2 2

+ MnO 2

Effervescence and black precipitate appeared

MnO2 + 2H2O2 → MnO↓

+ O + 2H O2 2 2H O2 2 → O + 2H O2 2

Comments:

2KMnO 4 + 3H 2 SO 4 + 5H 2 O 2 → 5O + 2MnSO + K 2 4 2 SO 4 + 8H O 2

2KI + H 2 SO 4 + H 2 O 2 → K 2 SO 4 + I ↓+ 2H O 2 2

MnO 2 + 2H 2 O 2 → MnO↓ + O + 2H 2 2 O

→ These three reactions are called Redox Reaction ( also known as Reduction/

Oxidation reaction)

Ionic equation:

2MnO 4 - + 6H + 5H + → 2Mn + 8H O + 5O

2I - + 2H + H + → I + 2H O

2 O 2 2 2

GENERAL CHEMISTRY LABORATORY

4 Reactions of Nitrate

1M NaNO 3

+ FeSO 4

+ concentrated

H SO 2 4

NaNO3 + FeSO 4

produce yellow Then add H2SO4,

turned brownish-red, effervescence appeared

2NaNO3 + 6FeSO + 4 4H SO2 4 → 3Fe2(SO4)3 + Na2SO4 + 4H O + 2 2NO

1M NaNO 2

+ FeSO 4

+ concentrated

H SO 2 4

The greenish solution turned brownish-red, effervescence appeared

2NaNO2 + 2FeSO + 4 2H SO2 4 → Fe2(SO4)3 + 2NO + Na2SO4 + 2H O2

1M NaNO 3

+ FeSO 4

+ concentrated

CH COOH 3

The light yellow green turned white-yellow, effervescence appeared

NaNO3 + 2FeSO + 4

+ 2(CH3COO)3Fe + 2SO3 + 3H O2

Comments:

→ These reactions are called Redox Reaction ( also known as Reduction/

Oxidation reaction) which contained a substance acting as an oxidizing agent and another substance actings as a reducing agent

Ionic equation:

3 Fe + NO + 4H → 2Fe + NO + 2H O 2+ 3- + 3+

2

NO 2- + Fe + 2H → NO + H O + Fe 2+ +

2 3+

2Fe 2+ + 2SO + 6H NO → NO + 2Fe + 2SO +3 H O 4 2- + 3- 2- 3+ 3 2

GENERAL CHEMISTRY LABORATORY

0.5M Na 2 SO 3

+ 2M H 2 SO 4

+ 0.1M KMnO 4

The first, brown

precipitate

appeared Then

the precipitate

dissolved

5Na SO2 3 + 3H2SO4

+2KMnO4→ 5Na2SO4 + 2MnSO + K4 2SO4 + 3H O2

0.5M Na 2 SO 3

+ 6N NaOH+

0.1M KMnO 4

The purple

solution turned

into greenish

solution

Na SO2 3 + 2NaOH + 2KMnO4→ Na2MnO4 +

K MnO2 4 + Na2SO4 +

H2O

0.5M Na 2 SO 3

+H O 2

+ 0.1M KMnO 4

The purple

solution was in

the first stage,

then the brown

precipitate

appeared

3Na SO2 3 + H O + 2

equation

2M K 2 Cr O 2 7

+ 6M H 2 SO 4

+C H OH

The orange solution turned into green solution

2K Cr O2 2 7 + 8H2SO4 + 3C2H5OH → 2K2SO4 + 2Cr2(SO4)3 +

Comments: These reactions are called Redox Reaction (also known

as Reduction/ Oxidation reaction) which contained a substance acting

as an oxidizing agent and another substance acting as a reducing agent.

6 Reaction of Potassium Dichromate (K2Cr2O7)

Comments/Conclusions:

Ionic equation: 2Cr2O7 2- + 3C2H5OH + 16H → 3CH COOH + 11H O +

+4Cr3+

7.Reaction of and

A Reactions of

equation

GENERAL CHEMISTRY LABORATORY 0.5M FeCl 3

+ 0.5M KOH

The tawny

solution lost the

color, the

brownish-red

precipitate

appeared

FeCl3 + 3KOH → Fe(OH)3↓ + 3KCl

0.5M FeCl 3

+ 2M NH 4 OH

The tawny

solution lost the

color, the

brownish-red

precipitate

appeared

FeCl3 + 3NH OH 4

→ Fe(OH) ↓ + 3 3NH Cl4

Comments:

-The first reaction is also known as precipitation reaction Net ionic equation: Fe + 3OH3+ - Fe(OH)

-The second one is a double displacement reaction as there is an

+ 3OH-  Fe(OH)3.

B Reactions of Fe2+

0.5M FeSO 4

+ 2M KOH

The greenish

precipitate

appeared

FeSO4 + 2KOH → Fe(OH)2↓ + K2SO4

Comments: The two reactions are also known as precipitation

reaction Net ionic equation: Fe + 2OH2 -  Fe(OH)2

equation

0.5M Al 2 (SO 4 ) 3

+ 2M NaOH

The white gel

precipitate

→ 2Al(OH) ↓ + 3 3Na SO2 4

0.5M Al 2 (SO 4 ) 3

+ 2N NaOH

+ 2M HCl

The first, the white

gel precipitate

appeared, then

the white

precipitate

appeared after

adding HCl

Al (SO2 4)3 + 6NaOH

→ 2Al(OH) ↓ + 3 3Na SO2 4

Al(OH)3 + 3HCl → AlCl3 + 3H O2

0.5M Al 2 (SO 4 ) 3

+ 2M NaOH

+ 2M NaOH

The first, the white

gel precipitate

appeared, then it

was dissolved in

the solution

Al (SO2 4)3 + 6NaOH

→ 2Al(OH) ↓ + 3 3Na SO2 4

Al(OH)3 + NaOH → NaAlO2 + 2H O2

8 Reactions of Al3+

GENERAL CHEMISTRY LABORATORY

substance presents basic or acid characteristics It can react to both acid and base:

Al(OH)3 + 3H → Al + 3H O+ 3+

2 Al(OH)3 + OH- → AlO +2H O

2-2

9 Flame test.

flame

color

CaCl 2 Orange

BaCl 2 Yellow flame 5.87 5.11 3.386

Comments:

-Each alkaline meta and alkaline earth metal has different structural characteristics leads to the different structure between their salt compounds On the fire they show different color

-The relationship between the wavelength, frequency and speed of an electromagnetic wave is given by the equation: C = λ x v

-So we can calculate the frequency by the equation: v = C/ λ

-And the energy per photon is given by the equation: Ephoton = x v h