electrolysis simulation

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THE ELECTROLYSIS CELL An electrolytic cell is a cell consisting of two electrodes (anode and cathode) immersed in an electrolyte for carrying out electrolysis, a direct electric current is passed through the electrolyte from an external source. Molten salts and aqueous solution of ionic compounds are electrolyte commonly need in electrolysis. Anode is the electrode that connected to the positive terminal of the battery. At this electrode, anions was release their electron. Cathode is the electrode that connected to the negative terminal of the battery. At this electrode, cation was received an electrons. Factor affecting the selective discharge of ions 1

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Page 1: Electrolysis Simulation

THE ELECTROLYSIS CELL

An electrolytic cell is a cell consisting of two electrodes (anode and cathode) immersed in an

electrolyte for carrying out electrolysis, a direct electric current is passed through the electrolyte

from an external source.

Molten salts and aqueous solution of ionic compounds are electrolyte commonly need in

electrolysis.

Anode is the electrode that connected to the positive terminal of the battery. At this electrode,

anions was release their electron.

Cathode is the electrode that connected to the negative terminal of the battery. At this electrode,

cation was received an electrons.

Factor affecting the selective discharge of ions

When more than one type of cation or anions is present in a solution, only one cation and anion

is preferentially selected for discharged. The selective discharge of ions depends on three factors.

a) The concentration of the ion in the electrolyte.

b) The standard electrode potential of the ion (the position of the metal in the

electrochemical series)

c) The type of electrode (active or inert) used.

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Page 2: Electrolysis Simulation

Electrolysis is used for effluent treatment. Heavy metal ions from manufacturing process that are

found in effluent can be removed by electrolysis.

Spontaneous reaction is known as, if a reaction of its own accord when the reactants are mixed

at room temperature and pressure.

Non-spontaneous reaction is known as, if the reaction does not occur of its own accord at room

conditions.

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Page 3: Electrolysis Simulation

ENGAGE

You are given the picture as shown below: Electric current was supply to the water.

1. What do you observe?

2. What happen on the wire?

3. How this happen?

4. How this could apply in daily life?

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Page 4: Electrolysis Simulation

EMPOWER

Steps

1. Electrolysis is a method of using an electric current to drive an otherwise non-spontaneous chemical reaction. Electrolysis is commercially highly important as a stage in the separation of elements from naturally-occurring sources such as ores using an electrolytic cell.

2. Electrolysis Cell is cell that use electric power through itself to produce chemistry reaction.

3. Oxidation: A process in which a substance loses one or more electrons

4. Reduction: A process in which a substance gains one or more electrons

5. Anode is the electrode that connected to the positive terminal of battery

6. Cathodeis the electrode that connected to the negative terminal of battery

7. Log on the web site to observe the animation to answer the question. http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/simDownload/index4.html#electrochem

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Page 5: Electrolysis Simulation

Results:

Electrolysis of Ni (NO3)2

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Page 6: Electrolysis Simulation

Electrolysis of Fe(NO3)

Electrolysis of Cu (NO3)2

Electrolysis of Ag (NO3)2

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Page 7: Electrolysis Simulation

Question

1. What the reaction at the anode and cathode in the process electrolysis of Nikel(II) Nitrate?

2. Why the mass off anode is reduce in the anode?

3. Why the mass off cathode is increase in cathode?

Answer:

Cathode: Ni2+ (aq) + 2e- Ni(s)

Anode: Ni(s) Ni2+ (aq) + 2e-

2. Because the cation (Ni2+) was remove from the anode make the mass of electrode is reduce.

3. Because the cathode electrode was accepted the cation (Ni 2+).That make the mass off cathode

is increase.

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Page 8: Electrolysis Simulation

ENHANCE

Figure 1

Activity 2 http://www.chem.iastate.edu/ChemEdGroup/GREENBOWE/sections/projectfolder/

flashfiles/electroChem/electrolysis10.html

According to figure 1

a) Will nickel metal spontaneously react with aqueous nickel (II) nitrate?

b) Predict what will happen when the power is turned on?

c) Identify the metal used for each electrode?

d) Indicate the direction of the flow of electrons in the wire?

e) Indicate what will happen at each electrode?

f) Identify the anode and the cathode?

g) Write the half-reactions and full-reaction that will occur?

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Page 9: Electrolysis Simulation

Figure 2

According to figure 2

a) Will nickel metal spontaneously react with aqueous iron (II) nitrate?

b) Indicate the direction of the flow of electrons in the wire?

c) Indicate what will happen at each electrode?

d) Identify the metal used for each electrode?

e) Identify the anode and the cathode?

f) Write the half-reactions and full reaction with the balanced chemical equation?

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