Report
CHEMICAL REPORT
"Redox Reaction"
CHAPTER I
PRELIMINARY
A. Purpose:
In this activity will be studied spontaneous redox reactions and not spontaneous
B. Platform Theory:
Reduction is the acceptance of electrons or decreases in oxidation numbers, whereas oxidation is the release of electrons or an increase in the oxidation number. The redox reaction is a combination of the simultaneous reduction and oxidation reactions. There is no electron discharge event (oxidation reaction) without an electron capture event (reduction reaction). Redox reactions may be either spontaneous or spontaneous.
The spontaneity of a redox reaction can be determined using a voltaic series. The order of the metals in the volt series is:
K-Ba-Ca-Na-Mg-Al-Mn-Zn-Cr-Fe-Cd-Co-Ni-Sn-Pb- (H2) -Sb-Bi-Cu-Hg-Ag-Pt-Au
The metals next to k2H2 are active metals (strong reducing agents) while the metals on the right H2 are less active (weak reductors). The more to the left the reductor properties are getting weaker and the oxidizing properties get stronger. The metals in the voltaic series can reduce the elements of the dikanannya but not able to reduce the elements on the left. If a metal can reduce the elements to the right, the reaction is spontaneous. Conversely, if not able to reduce the elements on the right reaction is not spontaneous.
Chemical reactions that take place spontaneously, characterized by the characteristics of the resulting sediment, bubbles, changes in color, and changes in temperature.
CHAPTER II
OBSERVATION METHODS
A. Draft Practicum:
In this lab, the author designed the lab using the literature and experimental method. The literature review is conducted so that the authors obtain theories as a reference for the lab. Authors do literature review activities by surfing the internet.
To strengthen the existing theories, the authors conduct experimental model experiments to prove the author's hypothesis in accordance with theories obtained by the author.
C. Practical Variables:
A variable is something that is measured in the writing of a practicum report. The variables considered in the writing of a report of this practice is spontaneous and not spontaneous reaction.
D. Data Collection Technique:
As a reference to create practical reports, the author looks for various data related to the title of various books and internet. The literature review is used as a reference for obtaining existing data and theories. The author studied and poured existing sources into the manufacture of practical reports.
E. Work Steps
Tools and materials
Size / Unit
amount
The reaction tube / rack
Drop pipette
ZnSO4 solution
CuSO4 solution
HCl solution
Zinc metal plate / Zn
Copper metal plate / Cu
Sandpaper
-
-
1 m
1 m
1 m
0.5 x 1 cm
0.5 x 1 cm
-
4/1
3
5 mL
5 mL
10 mL
2 pieces
2 pieces
Sufficiently
B. Ways of working:
1. Fill the glass with water approximately three-quarters of a piece, add 10 drops of phenolphthalein solution
2. Squeeze with metal pliers and lift sodium metal from a storage bottle. Using paper filter any kerosene from the metal surface. Observe the metal's appearance, then irislah the metal with a dry knife, observe the surface of the slice
3. Cut the sodium metal as big as green beans. Using an iron pliers, wrap metal sodium tightly and then insert the piece of metal into a water-filled glass of phenol ftalein, immediately cover the beaker with a solder dish
4. Record all necessary observations
CHAPTER III
RESULTS OF OBSERVATIONS AND DISCUSSIONS
A. Observation Tables:
Tube 1
Tubes 2
Tube 3
Tubes 4
Solution filled
CuSO4
ZnSO4
HCl
HCl
Color of solution
Blue
Snappy
Clear
Clear
Added metal
Zinc
Copper
Zinc
Copper
Changes after metal enhancement
The metal is black and there are bubbles
No reaction
There are bubbles
The metal becomes clean
B. Analysis and Discussion:
In this experiment, the CuSO4 solution released the characteristics of spontaneous reactions as described in the theoretical basis above. Once observed, it turns out that a solution of CuSO4 is inserted in the zinc metal plate, releasing small bubbles around the zinc plate. Zinc plates are also slowly undergoing corrosion. If the experiment is carried out longer, the zinc plate will be destroyed and become a precipitate in CuSO4 solution. This negates that the reaction occurring in CuSO4 solution is a spontaneous reaction.
Meanwhile, in the ZnSO4 solution which is inserted in the copper plate, there is no change in either the slab or the ZnSO4 solution. This indicates that the reaction occurring in ZnSO4 solution is a meaningless spontaneous reaction, in which the solution requires external energy for reaction.
HCl solution secretes spontaneous reaction features. Once observed, the HCl solution in which is inserted a zinc metal plate, removing small bubbles around the zinc plates
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hi zelvy please Explain to me about the difference between spontaneous redox reaction and non-spontaneous redox? thanks
BalasHapusA redox reaction can take place spontaneously if the resulting cell potential is marked positive. The cell potential is the difference between the cathode potential and the anode. In redox reactions, cathode means reduction and anode means oxidation. Thus the redox reaction proceeds spontaneously if the potential of the stimulated species is reduced by the potential of the species with an oxidized species greater than zero.
HapusThe redox reaction is spontaneous if E red - E ox > 0
Consider the following example:
Specified:
Cu2 + (aq) + 2e <====> Cu (s) Eo = + 0.34 V
Mg2 + (aq) + 2e <====> Mg (s) Eo = -2,34 V
Check if the following reaction goes spontaneously under standard conditions
Cu (s) + Mg2 + (aq) <====> Cu2 + (aq) + Mg (s)
Answer:
In the reaction magnesium is reduced, while the copper is oxidized.
E cell = Eo red - Eo ox = -2.34 V - 0.34 V = -2.68 V
Since the cell Eo is marked negative, the reaction can not be spontaneous under standard conditions.
If a redox reaction is not spontaneous, the inverse reaction is spontaneous. Ie Mg reaski with Cu ions with potential + 2.68, can take place spontaneously
Why a redox reaction can take place spontaneously?
BalasHapusOkay, redox reactions can be estimated from the potential price of the cell.
HapusA redox reaction can take place spontaneously if the resulting cell potential is marked positive. The cell potential is the difference between the cathode potential and the anode. In redox reactions, cathode means reduction and anode means oxidation. Thus the redox reaction proceeds spontaneously if the potential of the stimulated species is reduced by the potential of the species with an oxidized species greater than zero.
The redox reaction is spontaneous if E red - E ox> 0
What characteristic of chemical reaction in this experiment ?
BalasHapusThe characteristic is There are free elements, ex: Cl₂, Cu, O₂
Hapus- There is a change of oxidation number
- There is a reducing agent à an oxidizing agent
- There is oxidizer (oxidizing) à substances that undergo reduction
Cu²⁺ (aq) + Zn (s) à Cu (s) + Zn²⁺ (aq)
+2 0 0 +2
Reduction
Oxidation
Reductor à Zn
Oxidator à Cu²⁺
Hai zelvy.
BalasHapuswhat the function of sel volta?
The Volta cell is a series of cells that can generate electrical current. In the cell there is a change from the redox reaction generates an electric current.
HapusWhy we must balancing those redox? what about autoredox?
BalasHapusWhether to make a report without literature??
BalasHapusZelvy, What if Variables are not in the report writing lab ?
BalasHapus