Electrolysis Flashcards

1
Q

Negative electrode

A

Cathode

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2
Q

Positive electrode

A

anode

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3
Q

Substance that conducts electricity

A

electrolyte

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4
Q

Why is a mixture of aluminium oxide plus cryolite used?

A

It saves energy, as the mixture has a lower boiling point

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5
Q

Why does aluminium oxide have to be molten for electrolysis to take place?

A

Aluminium oxide has to be separated from the ore, which contains other substances.
It enables ions to move to the electrodes.

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6
Q

What forms at the cathode and what forms at the anode for the electrolysis of aluminium?

A

-Aluminium forms at cathode
-Oxygen forms at anode

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7
Q

What are the half equations for the changes at each electrode in the electrolysis of molten aluminium oxide?

A

Cathode: Al^3+ + 3e– ⟶ Al
Anode: 2O^2- – 4e– ⟶ O2

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8
Q

Why are the carbon anodes regularly replaced?

A

Because they gradually burn away as the oxygen reacts with the hot carbon anodes, forming carbon dioxide gas

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9
Q

What is electrolysis?

A

The breaking down of ionic substances using electricity

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10
Q

What is formed at the cathode and anode on the electrolysis of molten lead bromide?

A

Cathode: lead (ions gain electrons)
Anode: bromine (ions lose electrons)

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11
Q

Half equations for lead and bromine

A
  • Pb^2+ + 2e– ⟶ Pb
  • 2Br^- – 2e– ⟶ Br2
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12
Q

Rules for discharge of ions in electrolysis

A

+ions: the least reactive is discharged
-ions: group 7 is always first, then OH-
—> OH- forms O2 gas

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13
Q

When OH- forms O2 gas, what is the half equation?

A

4OH- —> 2H2O + O2 + 4e-

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