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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