Report Template

Tài liệu học tập môn Chemistry Laboratory (CH012IU) tại Trường Đại học Quốc tế, Đại học Quốc gia Thành phố Hồ Chí Minh. Tài liệu gồm 20 trang giúp bạn ôn tập hiệu quả và đạt điểm cao! Mời bạn đọc đón xem! 

48 24 lượt tải Tải xuống
Chia sẻ Báo cáo tài liệu

Môn: Chemistry Laboratory (CH012IU)

Trường: Trường Đại học Quốc tế, Đại học Quốc gia Thành phố Hồ Chí Minh

Thông tin:

18 trang 7 tháng trước

Tác giả:

Profile Như Hoa
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC1
CHEMISTRY LABORATORY
REPORT
EXPERIMENT 1: CHEMICAL REACTIONS
Group: ______________ Class: ______________ Date: ____________
Group members:
Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion
Full name
Student ID
Declaration of Contribution
Signature
1
2
3
4
5
Total score: _______/100
1
2+
Reaction
Observation
Chemical Equation
M CuSO
0.5
4
+
2M NaOH
0.5
M CuSO
4
+
2M NH
4
OH
Discussion:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC2
CHEMISTRY LABORATORY
(Discuss: i) Explanation for the above observation; ii) Possible reasons for any misconducted
results)
2. REACTIONS OF SILVER HALIDES
Reaction
Observation
Chemical Equation
0.5
M KCl
+
0.1M AgNO
3
0.5
M KCl
0.1M AgNO
+
3
+
2M NH
4
OH
0.5
M KBr
+
0.1M AgNO
3
0.5
M KBr
+
0.1M AgNO
3
+
2M NH
4
OH
Discussion:
3
. REACTIONS OF H
2
O
2
Reaction
Observation
Chemical Equation
0.1
M KMnO
4
+
2M H
2
SO
4
+
H
2
O
2
M KI
0.1
+
2M H
2
SO
4
+
H
2
O
2
H
2
O
2
+
MnO
2
Discussion:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC3
CHEMISTRY LABORATORY
Discussion:
4
. REACTIONS OF KMnO
4
Reaction
Observation
Chemical Equation
0.5
M Na
2
SO
3
2M H
+
2
SO
4
+
0.1M KMnO
4
0.5
M Na
2
SO
3
+
6N NaOH
+
0.1M KMnO
4
M Na
0.5
2
SO
3
+
H
2
O
+
0.1M KMnO
4
Discussion:
. A. REACTIONS OF Fe
5
3+
Reaction
Observation
Chemical Equation
0.5
M FeCl
3
+
2M KOH
0.5
M FeCl
3
+
2M NH
4
OH
5
. B. REACTIONS OF Fe
2+
Chemical Equation
Reaction
Observation
0.5
M FeSO
4
+
2M KOH
0.5
M FeSO
4
+
2M NH
4
OH
Discussion:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC4
CHEMISTRY LABORATORY
Part 4. Conclusions
END.
. REACTIONS OF Al
6
3+
Reaction
Observation
Chemical Equation
0.5
M Al
2
(
SO
4
)
3
+
2N NaOH
2M HCl
+
0.5
M Al
2
(
SO
4
)
3
+
2M NaOH
2M NaOH
+
Discussion:
. FLAME TEST
7
Solution
Dominant flame
color
Wavelength
(
nm
)
Frequency
(
s
1
)
Photon energy (J)
LiCl
NaCl
KCl
CaCl
2
BaCl
2
Discussion
:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC5
CHEMISTRY LABORATORY
REPORT
EXPERIMENT 2: pH AND BUFFERS
Group: ______________ Class: ______________ Date: ____________
Group members:
Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion
Full name
Student ID
Declaration of Contribution
Signature
1
2
3
4
5
Total score: _______/100
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC6
CHEMISTRY LABORATORY
3. pH OF WEAK ACID
. pH OF DEIONIZED WATER
1
Time
(
second
)
Observed pH
Discussion
1
st
(
Group___
)
2
nd
)
(
Group___
0
20
40
60
2
. pH OF STRONG ACID
Solution
Theoretical
pH
Measured pH
Discussion
1
st
(
Group___
)
2
nd
(
Group____
)
10
mL of 0.1M HCl
Add 90 mL of distilled
water
Add 10 mL of
0.1
M NaOH
Add 90 mL of
0.01
M NaOH
Calculation:
Solution
Measured pH
K
a
Discussion
1
st
(
Group___
)
2
nd
(
Group____
)
0.1
M acetic acid
0.01
M acetic acid
0.001
M acetic acid
Calculation:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC7
CHEMISTRY LABORATORY
Discussion:
Part I: Addition of 10 drops 0.1 M HCl
Part II: Addition of 10 drops 0.1 M NaOH
. pH OF SALTS
4
Solution
Predicted
pH
Measured pH
Discussion
1
st
(
Group____
)
2
nd
(
Group____
)
0.1
M NaCl
0.1
M CH
3
COONa
0.1
M NH
4
Cl
Calculation:
. pH OF BUFFERS
5
Buffer
Volume
(
mL) 0.1M
CH
3
COOH
Volume (mL)
0.1
M
CH
3
COONa
Acid
Base
Calculated
pH
Measured pH
1
st
(
Group__
)
2
nd
(
Group__
)
A
10.0
40.0
B
40.0
10.0
Calculation
pH:
Buffer
pH from
the start,
pH
o
pH after
adding 10
drops HCl
Total volume HCl (drops)
to change pH by one unit
(
pH
o
-1)
Discussion
A
B
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC8
CHEMISTRY LABORATORY
END.
REPORT
EXPERIMENT 3: REDOX TITRATION
Group: ______________ Class: ______________ Date: ____________
Group members:
Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Buffer
pH from
the start,
pH
o
pH after
adding 10
drops NaOH
Total volume NaOH
(
drops) to change pH by
one unit (pH
o
+1)
Discussion
A
B
Part 4. Conclusions
Full name
Student ID
Declaration of Contribution
Signature
1
2
3
4
5
Total score: _______/100
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC9
CHEMISTRY LABORATORY
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion
1. STANDARDIZATION OF PREPARED KMnO
4
SOLUTION
Calculation:
Normality of the standard H
2
C
2
O
4
solution, N(H
2
C
2
O
4
) = ___________________
Volume of the standard H
2
C
2
O
4
solution used, V(H
2
C
2
O
4
) = ___________________
Average Normality of KMnO
4
= ____________
Discussion:
2. DETERMINATION OF UNKNOWN CONCENTRATION H
2
C
2
O
4
SOLUTION
Calculation:
Normality of the standard KMnO
4
solution, N(KMnO
4
) = ___________________
Volume of the unknown H
2
C
2
O
4
solution used, V(H
2
C
2
O
4
) = ___________________
Trial #
Burette reading (mL)
Volume of KMnO
4
(mL)
Normality of KMnO
4
(N)
1
-
2
-
Trial #
Burette reading (mL)
Volume of KMnO
4
(mL)
Normality of H
2
C
2
O
4
(N)
1
-
2
-
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC10
CHEMISTRY LABORATORY
Average Normality of H
2
C
2
O
4
= ____________
Discussion:
3. DETERMINATION OF UNKNOWN CONCENTRATION FeSO
4
SOLUTION
Calculation:
Normality of the standard KMnO
4
solution, N(KMnO
4
) = ___________________
Volume of the unknown FeSO
4
solution used, V(FeSO
4
) = ___________________
Discussion:
Part 4. Conclusions
END.
REPORT
EXPERIMENT 4: CHEMICAL EQUILIBRIUM
Group: ______________ Class: ______________ Date: ____________
Group members:
Trial #
Burette reading (mL)
Volume of KMnO
4
(mL)
Normality of FeSO
4
(N)
1
-
2
-
Average Normality of FeSO
4
=
____________
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC11
CHEMISTRY LABORATORY
Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion
Full name
Student ID
Declaration of Contribution
Signature
1
2
3
4
5
Total score: _______/100
. ACID/BASE EQUILIBRIA
1
Equilibrium System:
2
CrO
4
2
+ 2H
+
(
aq)
Cr
2
O
7
2
+ H
2
O(l)
Description of
conditions
Predicted
outcome
Observation
Discussion
Initial solution
+
Conc. HCl
+
6 N NaOH
Note:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC12
CHEMISTRY LABORATORY
Note:
3. EQUILIBRIA OF PRECIPITATION REACTIONS
2
. EQUILIBRIA OF ACID/BASE INDICATORS
Equilibrium System:
H(MV)(aq) + H
2
O(l)
H
3
O
+
(
aq) + MV
aq
)
(
Addition
Predicted
outcome
Observation
Discussion
None (control)
6
M HCl
6
M NaOH
6
M HCl
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC13
CHEMISTRY LABORATORY
Equilibrium System: Ca (aq) + C O
2+
2
4
2
(
aq)
CaC
2
O
4
(
s
)
Addition
Predicted
outcome
Observation
Discussion
Test tube 1:
0.1
M Na
2
C
2
O
4
Test tube 2:
+
0.1 M
H
2
C
2
O
4
Test tube 2:
+
6 M HCl
Test tube 2:
+
6 M NH
4
OH
Note:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC14
CHEMISTRY LABORATORY
4. TEMPERATURE EFFECTS ON EQUILIBRIA
Part 4. Conclusions
END.
REPORT
EXPERIMENT 5: FACTORS AFFECTING
REACTION RATE
Group: ______________ Class: ______________ Date: ____________
Group members:
Equilibrium System:
Co(H
2
O)
6
2+
(
aq) + 4Cl
(
aq)
CoCl
4
2
aq) + 6H
(
2
O(l)
Description of
conditions
Predicted
outcome
Observation
Discussion
Nothing changed
(
control
)
Hot water bath
Ice-water bath
Note:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC15
CHEMISTRY LABORATORY
Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion
1. EFFECT OF CONCENTRATION ON REACTION TIME
Reaction 1: __________________________________________________
Reaction 2: __________________________________________________
Calculate the initial concentrations of I
-
and S
2
O
8
2-
ions:
Mixture # 5:
[I
-
] =
[S2O82-] =
Full name
Student ID
Declaration of Contribution
Signature
1
2
3
4
5
Total score: _______/100
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC16
CHEMISTRY LABORATORY
Plotting the concentration of iodide ion versus time: [Note: X – axis: time; Y – axis: concentrations].
* Mixtures # 1-6:
- Graph
- The order of reaction with respect to iodide ion?
- Discussion:
* Mixtures # 1, 7, 8, 9, 10, and 11:
- Graph
- The order of reaction with respect to iodide ion?
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC17
CHEMISTRY LABORATORY
- Discussion:
2. EFFECT OF TEMPERATURE ON THE REACTION RATE
3. EFFECT OF A CATALYST ON THE REACTION RATE
Note:
Reaction System:
Description of
conditions
Predicted
outcome
Observation
Reaction
time
Discussion
Room
temperature
50
0
C
90
0
C
Note:
Reaction System:
Trial
Description of
conditions
Predicted
outcome
Observation
(
Reaction rate
)
Discussion
1
+
MnCl
2
2
+
MnO
2
3
+
NaCl
4
+
CaCl
2
5
+
Zn
6
+
KNO
3
7
+
Fe(NO
3
)
3
The order of catalyst activity:
lOMoARcPSD|364906 32
International University, Vietnam National University - HCMC18
CHEMISTRY LABORATORY
Part 4. Conclusions
END.
| 1/18
| | Tải xuống

Có thể bạn quan tâm:

Preview text:

lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC1 CHEMISTRY LABORATORY REPORT
EXPERIMENT 1: CHEMICAL REACTIONS
Group: ______________ Class: ______________ Date: ____________ Group members: Full name Student ID Declaration of Contribution Signature 1 2 3 4 5 Total score: _______/100 Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion
1 . REACTIONS OF Cu 2+ Reaction Observation Chemical Equation 0. M
5 CuSO 4 + 2M NaOH
0.5 M CuSO 4
+ 2M NH 4 OH Discussion: lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC2 CHEMISTRY LABORATORY
(Discuss: i) Explanation for the above observation; ii) Possible reasons for any misconducted results)
2. REACTIONS OF SILVER HALIDES Reaction Observation Chemical Equation 0.5 M KCl
+ 0.1M AgNO 3 0.5 M KCl + 0.1M AgNO 3
+ 2M NH 4 OH 0.5 M KBr
+ 0.1M AgNO 3 0.5 M KBr
+ 0.1M AgNO 3
+ 2M NH 4 OH Discussion:
3 . REACTIONS OF H 2 O 2 Reaction Observation Chemical Equation
0.1 M KMnO 4
+ 2M H 2 SO 4
+ H 2 O 2 0. M 1 KI
+ 2M H 2 SO 4
+ H 2 O 2
H 2 O 2 + MnO 2 Discussion: lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC3 CHEMISTRY LABORATORY
4 . REACTIONS OF KMnO 4 Reaction Observation Chemical Equation
0.5 M Na 2 SO 3
+ 2M H 2 SO 4
+ 0.1M KMnO 4
0.5 M Na 2 SO 3 + 6N NaOH
+ 0.1M KMnO 4 0. M
5 Na 2 SO 3
+ H 2 O
+ 0.1M KMnO 4 Discussion: .
5 A. REACTIONS OF Fe 3+ Reaction Observation Chemical Equation
0.5 M FeCl 3 + 2M KOH
0.5 M FeCl 3
+ 2M NH 4 OH Discussion:
5 . B. REACTIONS OF Fe 2+ Reaction Observation Chemical Equation
0.5 M FeSO 4 + 2M KOH
0.5 M FeSO 4
+ 2M NH 4 OH Discussion: lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC4 CHEMISTRY LABORATORY .
6 REACTIONS OF Al 3+ Reaction Observation Chemical Equation
0.5 M Al 2 ( SO 4 ) 3 + 2N NaOH + 2M HCl
0.5 M Al 2 ( SO 4 ) 3 + 2M NaOH + 2M NaOH Discussion: . 7 FLAME TEST Solution Dominant flame Wavelength Frequency Photon energy (J) color ( nm )
( s 1 ) LiCl NaCl KCl CaCl 2 BaCl 2 Discussion : Part 4. Conclusions END. lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC5 CHEMISTRY LABORATORY REPORT
EXPERIMENT 2: pH AND BUFFERS
Group: ______________ Class: ______________ Date: ____________ Group members: Full name Student ID Declaration of Contribution Signature 1 2 3 4 5 Total score: _______/100 Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC6 CHEMISTRY LABORATORY .
1 pH OF DEIONIZED WATER Observed pH Time 1 st 2 nd Discussion
( second ) ( Group___ ) ( Group__ ) _ 0 20 40 60
2 . pH OF STRONG ACID Measured pH Theoretical Solution Discussion 1 st 2 nd pH ( Group___ ) ( Group____ )
10 mL of 0.1M HCl Add 90 mL of distilled water Add 10 mL of 0.1 M NaOH Add 90 mL of 0.01 M NaOH Calculation: 3. pH OF WEAK ACID Solution Measured pH K a Discussion 1 st 2 nd ( Group___ ) ( Group____ )
0.1 M acetic acid
0.01 M acetic acid
0.001 M acetic acid Calculation: lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC7 CHEMISTRY LABORATORY . 4 pH OF SALTS Measured pH Predicted Solution 1 st 2 nd Discussion pH ( Group____ ) ( Group____ ) 0.1 M NaCl
0.1 M CH 3 COONa
0.1 M NH 4 Cl Calculation: .
5 pH OF BUFFERS Volume Volume (mL) Measured pH Calculated
Buffer ( mL) 0.1M 0.1 M Acid Base 1 st 2 nd pH
CH 3 COOH
CH 3 COONa ( Group__ ) ( Group__ ) A 10.0 40.0 B 40.0 10.0
Calculation pH: Discussion:
 Part I: Addition of 10 drops 0.1 M HCl Buffer pH from pH after
Total volume HCl (drops) Discussion the start, adding 10
to change pH by one unit pH o drops HCl
( pH o -1) A B
 Part II: Addition of 10 drops 0.1 M NaOH lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC8 CHEMISTRY LABORATORY pH from pH after Total volume NaOH Buffer the start, adding 10
( drops) to change pH by Discussion pH o drops NaOH
one unit (pH o +1) A B Part 4. Conclusions END. REPORT
EXPERIMENT 3: REDOX TITRATION
Group: ______________ Class: ______________ Date: ____________ Group members: Full name Student ID Declaration of Contribution Signature 1 2 3 4 5 Total score: _______/100 Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment) lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC9 CHEMISTRY LABORATORY
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion
1. STANDARDIZATION OF PREPARED KMnO4 SOLUTION Calculation:
Normality of the standard H2C2O4 solution, N(H2C2O4) = ___________________
Volume of the standard H2C2O4 solution used, V(H2C2O4) = ___________________
Trial # Burette reading (mL) Volume of KMnO 4 (mL) Normality of KMnO 4 (N) 1 - 2 -
Average Normality of KMnO4 = ____________ Discussion:
2. DETERMINATION OF UNKNOWN CONCENTRATION H2C2O4 SOLUTION Calculation:
Normality of the standard KMnO4 solution, N(KMnO4) = ___________________
Volume of the unknown H2C2O4 solution used, V(H2C2O4) = ___________________
Trial # Burette reading (mL) Volume of KMnO 4 (mL) Normality of H 2 C 2 O 4 (N) 1 - 2 - lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC10 CHEMISTRY LABORATORY
Average Normality of H2C2O4 = ____________ Discussion:
3. DETERMINATION OF UNKNOWN CONCENTRATION FeSO4 SOLUTION Calculation:
Normality of the standard KMnO4 solution, N(KMnO4) = ___________________
Volume of the unknown FeSO4 solution used, V(FeSO4) = ___________________
Trial # Burette reading (mL) Volume of KMnO 4 (mL) Normality of FeSO 4 (N) 1 - 2 -
Average Normality of FeSO 4 = ____________ Discussion: Part 4. Conclusions END. REPORT
EXPERIMENT 4: CHEMICAL EQUILIBRIUM
Group: ______________ Class: ______________ Date: ____________ Group members: lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC11 CHEMISTRY LABORATORY Full name Student ID Declaration of Contribution Signature 1 2 3 4 5 Total score: _______/100 Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion .
1 ACID/BASE EQUILIBRIA
Equilibrium System: 2 CrO 4 2 + 2H + ( aq) Cr 2 O 7 2 + H 2 O(l) Description of Predicted Observation Discussion conditions outcome Initial solution + Conc. HCl + 6 N NaOH Note: lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC12 CHEMISTRY LABORATORY
2 . EQUILIBRIA OF ACID/BASE INDICATORS
Equilibrium System: H(MV)(aq) + H 2 O(l) H 3 O + ( aq) + MV (aq ) Addition Predicted Observation Discussion outcome None (control) 6 M HCl 6 M NaOH 6 M HCl Note:
3. EQUILIBRIA OF PRECIPITATION REACTIONS lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC13 CHEMISTRY LABORATORY 2+
2 4 2 ( aq)
CaC 2 O 4 ( s ) Predicted Addition Observation Discussion outcome Test tube 1: 0.1 M Na 2 C 2 O 4 Test tube 2: + 0.1 M H 2 C 2 O 4 Test tube 2: + 6 M HCl Test tube 2: + 6 M NH 4 OH Note:
Equilibrium System: Ca (aq) + C O lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC14 CHEMISTRY LABORATORY
4. TEMPERATURE EFFECTS ON EQUILIBRIA Equilibrium System: 2+ 2
Co(H 2 O) 6 ( aq) + 4Cl ( aq) CoCl 4 (aq
) + 6H 2 O(l) Description of Predicted Observation Discussion conditions outcome Nothing changed ( control ) Hot water bath Ice-water bath Note: Part 4. Conclusions END. REPORT
EXPERIMENT 5: FACTORS AFFECTING REACTION RATE
Group: ______________ Class: ______________ Date: ____________ Group members: lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC15 CHEMISTRY LABORATORY Full name Student ID Declaration of Contribution Signature 1 2 3 4 5 Total score: _______/100 Part 1. Introduction
(Introduce the general background and summarize the aims/objectives of the experiment)
Part 2. Materials and Methods
(Summarize the experimental design/structure of your experiment)
Part 3. Results and Discussion
1. EFFECT OF CONCENTRATION ON REACTION TIME
Reaction 1: __________________________________________________
Reaction 2: __________________________________________________
Calculate the initial concentrations of I- and S 2- 2O8 ions: Mixture # 5: [I-] = [S2O82-] = lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC16 CHEMISTRY LABORATORY
Plotting the concentration of iodide ion versus time: [Note: X – axis: time; Y – axis: concentrations]. * Mixtures # 1-6: - Graph
- The order of reaction with respect to iodide ion? - Discussion:
* Mixtures # 1, 7, 8, 9, 10, and 11: - Graph
- The order of reaction with respect to iodide ion? lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC17 CHEMISTRY LABORATORY - Discussion:
2. EFFECT OF TEMPERATURE ON THE REACTION RATE Reaction System: Description of Predicted Reaction Observation Discussion conditions outcome time Room temperature 50 0 C 90 0 C Note:
3. EFFECT OF A CATALYST ON THE REACTION RATE Reaction System: Description of Predicted Observation Trial Discussion conditions outcome
( Reaction rate ) 1 + MnCl 2 2 + MnO 2 3 + NaCl 4 + CaCl 2 5 + Zn 6 + KNO 3 7 + Fe(NO 3 ) 3
The order of catalyst activity: Note: lOMoARcPSD|364 906 32
International University, Vietnam National University - HCMC18 CHEMISTRY LABORATORY Part 4. Conclusions END.
Document Outline

  • REPORT
    • EXPERIMENT 1: CHEMICAL REACTIONS
  • REPORT (1)
    • EXPERIMENT 2: pH AND BUFFERS
  • REPORT (2)
    • EXPERIMENT 3: REDOX TITRATION
  • REPORT (3)
    • EXPERIMENT 4: CHEMICAL EQUILIBRIUM
  • REPORT (4)