Chemistrhyreduksi Dan Oxidasi
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Transcript of Chemistrhyreduksi Dan Oxidasi
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8/14/2019 Chemistrhyreduksi Dan Oxidasi
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CHEMISTRY PRACTICAL
Activity XIV
REDUCTION AND OXIDATION
REACTION
Members:
IL RAHMA PRADIRA GESARI X5/13
INAYAH NUR UTAMI X5/14KHAIRINA IZZATI AMALIA X5/15
SMA NEGERI 3 YOGYAKARTA
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I. AIM
Student can differ the reaction between elements which reacted redoxly
and not redoxly.
II. BASIC THEORY
Redox (shorthand forreduction-oxidation reaction) describes allchemical reactions in which atoms have their oxidation number (oxidation state)
changed. This can be either a simple redox process such as the oxidation of carbon
to yield carbon dioxide or the reduction of carbon by hydrogen to yield methane(CH4), or it can be a complex process such as the oxidation of sugar in the human
body through a series of very complex electron transfer processes.
The term redox comes from the two concepts ofreduction and oxidation.
It can be explained in simple terms:
Oxidation describes the loss of electrons / hydrogen orgain of oxygen / increase
in oxidation state by a molecule, atom or ion
Reduction describes thegain of electrons / hydrogen or a loss of oxygen /decrease in oxidation state by a molecule, atom or ion
Classical
Oxidation
React between some substances with oxygen.
Reduction React between some substances with hydrogen.
Modern Oxidation - Oxidation increase.number
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- Electrons exhaust.
Reduction- Oxidation number decrease.- Electrons arrest.
Oxidator
- Mengalami Reduksi- Oxidation number decrease
- mengoksidasi- Gain of Electron
Reductor
- Mengalami oksidasi- Oxidation increase.number
- mereduksi- Loss of electron
Auto Redox- Redox react where some substance mengalami
reduction sekaligus oxidation
III. APPARATUS
Reaction tube
Thermometer
Sandpaper
Iron
Zinc
Magnesium ribbon
Copper(cu)
Solution: CuSo4, ZnSo4 , H2So4, HCl
IV. PROCEDURE
1. Prepare 5 reaction tubes.
Tube 1 and 2 are filled by 2 mL of CuSo4 solution.Tube 3 is filled by 2 mL of ZnSo4 solution.
Tube 4 is filled by 2 mL of H2So4 solution.
Tube 5 is filled by 2 mL of HCl solution.
2. Rub each metal with sandpaper, then put on:Tube 1: Zn.
Tube 2: Fe.Tube 3: Cu.Tube 4: Mg.
Tube 5: Mg.
3. Measure the temperature and watch the changing that happens.
V. RESULT
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Tube
no.
Solution
(2mL)Metal
Temperature, colour, precipitate.
Before After
1 CuSO4 Zn
The solution is blue,the zinc is silver, and
the temperature is
normal (cold).
The zinc is become cooper and red,appear some little bubble, the
temperature was not change.
2 CuSO4 Fe
The solution is blue,
the iron is silver, and
the temperature isnormal (cold).
Appear some little bubble, change
become red cooper, the temperaturewas not change.
3 ZnSO4 Cu
The solution is clear(white), the copper is
silver, and the
temperature isnormal (cold).
Not reacted
4 H2SO4 Mg
The solution is clear
(white), themagnesium is gray,
and the temperature
is normal (cold).
Appear some little bubble, causingsome smoke, change to be hotter, the
magnesium was melting
5 HCl Mg
The solution is clear
(white), themagnesium is gray,
and the temperature
is normal (cold).
Appear some little bubble, causingsome smoke, change to be hotter, the
magnesium was melting
VI. EXERCISES1. Write the conclusion based on the result data above!
Tube number 1, 2, 4, and 5 are redox because they are reacted. Tube number 3 is not redox because its not reacted.
2. Write each balanced equation!
CuSO4 + Zn ZnSO4 + Cu CuSO4 + Fe FeSO4 + Cu
ZnSO4 + Cu not reacted
H2SO4 + Mg Mg SO4 + H2 HCl + Mg MgCl + H2
3. Is there any element that doesnt react? Yes, ZnSO4 + Cu
4. At the element that reacted redoxly, determine the oxidator, reductor, the
result element from oxidation, and result element from reduction!
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Asessor: The experimenters :
IL Rahma Pradira Gesari / X-5/ 13Inayah Nur Utami / X-5/ 14
Khairina Izzati Amalia / X-5/ 15