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
Trang 1EXPERIMENT 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
Trang 2GENERAL 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.
Trang 3II 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
Trang 4GENERAL 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
Trang 50.5M 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↓
Trang 6
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
Trang 7H 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
Trang 8
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
Trang 91M 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
Trang 10GENERAL 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 +
Trang 11Comments: 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
Trang 12GENERAL 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+
Trang 130.5M 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+
Trang 14GENERAL 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
Trang 15BaCl 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