# data[].attributes.body
Al3+ + 3e- -> Al
2Cl- - 2e- -> Cl2

# data[].attributes.body
Aluminium Chloride
1) Al3+ + Cl-
2) Al3
3) Al3+(l)+3e- ~>

# data[].attributes.body
1. Aluminum to cathode
2. Chloride to anode
3. Al 3+ +3e > Al
4. 6Cl- -6e > 3Cl2

# data[].attributes.body
1)Pb2+ Br-
2)Lead is attracted to the cathode
3)Bromide is attracted to anode
4)Pb2+ + 2e- > Pb
5)2Br- - 2e- > Br2

Al3+ + 3e- > Al

# data[].attributes.body
(1) Pb 2+ and Br -
(2) Pb 2+ is attracted to the cathode
(3) Br - is attracted to the anode
(4) Pb 2+ + 2e --> Pb (Reduction)
(5) 2Br - -2e --> Br2 (Oxidation)

# data[].attributes.body
Pb2+ and Br-
The lead is attracted to the. Cathode and the bromide is attracted to the anode
2Pb+ + 2e- > Pb (reduction)
2Br- - 2e- -> Br2 (oxidation)

# data[].attributes.body
1) lead + bromine
2) Pb2+
3) br-
4) Pb2+ + 2e- -> Pb

# data[].attributes.body
1) Lead 2+, Bromine -
2) Bromine anion attracted to anode
3) Lead cation attracted to cathode
4)  2Pb - 2e- -> Pb oxidation
5) 2Br + 2e- -> Br2 reduction
ALUMINIUM CHLORIDE AlCl3
Al - 3e- -> Al
3Cl + 3e- -> Cl3

# data[].attributes.body
1. Pb2+, Br-
2. Lead to the cathode
3. Bromine to the anode
4. Pb2+  +2e-  > Pb (reduction)
5. 2Br- -2e- > 2Br (oxidation)

# data[].attributes.body
LEAD BROMIDE
1. lead (Pb²⁺) and bromine (Br⁻)
2. Pb²⁺ attracted to the cathode
3. Br⁻ attracted to the anode
4. Pb²⁺ (l) + -2e⁻ => Pb (s) (reduction at the cathode)
5. 2Br- (l) -2e- => Br₂ (s) (oxidation at the anode)

ALUMINIUM CHLORIDE
1. aluminium (Al³⁺) and chloride (Cl²⁻)
2. Al³⁺ attracted to the cathode
3. Cl²⁻ attracted to the anode
4. Al³⁺ (l) +3e⁻ => Al (s) (reduction at the cathode)
5. 6Cl⁻ (l) - 6e⁻ => Cl₂ (g) (oxidation at the anode)

# data[].attributes.body
1) lead & bromine
2)lead is attracted to cathode
3)bromide is attracted to anode
4)reduction
5)oxidation

1) Aluminium attracted to cathode
2)chloride attracted to anode
3)

# data[].attributes.body
Lead Bromide
1. Pb 2+, Br 1-
2. Pb 2+ is attracted to the cathode
3. Br 1- is attracted to the anode
4. Pb 2+ +2e= Pb (Reduction) at the cathode
5. 2Br 1- -2e=Br2 (Oxidation) at the anode

Aluminium Chloride
1. Al 3+, Cl 1-
2. Al 3+ is attracted to the cathode
3. Cl - is attracted to the anonde
4. Al3+ + 3e = Al
5. 3Cl 1- -3e = Cl

# data[].attributes.body
1) Pb 2+, Br 1-
2)Lead is attracted to the Cathode
3)Bromine is attracted to the Anode
4)Pb 2+ + 2e-----> Pb (Reduction)
5)2Br 1- - 2e-------> Br2 (Oxidation)
6)Al3+(l) + 3e-------> Al (s) (Cathode-Reduction)
7)6Cl 1-(l) - 3e------->3Cl2(g) (Anode-Oxidation)

# data[].attributes.body
1. lead and bromine
2. lead forms a positive ion that is attracted to the cathode
3. bromide forms a negative ion that is attracted to the anode
4. lead gains electrons from the anode
Pb ^2+ (l) +2e^- ----> Pb (s)
this is a reduction reaction because the lead gains electrons, making it neutral.
forming lead atoms
5. the bromide ions transfers its electrons to the anode, making it neutral.
2Br^- (l) - 2e^ ---> Br2(g)
forming bromine molecules
this is an oxidation because the bromide ion loses electrons

# data[].attributes.body
1) Lead, Bromine, Pb2+Br
2)The positive ion lead is attracted to the cathode
3) Bromine forms a negative ion which is attracted the the anode.
4) The product discharged at the cathode would be a solid state of Lead, Pb. This is reduction as the lead ion gains electrons. Pb2+2e ----> Pb
5) The product discharged at the anode would be Bromide Gas, Br. This is oxidation as the Bromide ion loses an electron. Br^1- -2e ----> Br2

# data[].attributes.body
1. Lead 2+ and Bromide
2. Lead 2+ is attracted to the cathode
3. Bromide is attracted to the anode
4. Pb 2+ + 2e⁻ -> Pb (Reduction)
5. 2Br -  2e -> Br2 (oxidation)

Aluminium Chloride
1. Aluminium 3+ and Cloride-
2. Aluminium3+ is attracted to the cathode
3. Chloride is attracted to the anode
4. Al³⁺ + 3e⁻ -> Al₂
5. 6Cl- - 6e⁻ -> 3Cl₂

# data[].attributes.body
Lead (II) and Bromide
The Lead ions will be attracted to the negative cathode Pb^2+
The bromide ions will be attracted to the positives anodes Br^-
Pb^2+ + 2e- -> Pb ( Reduction ) reaction
2Br^- - 2e- -> Br2 ( Oxidation ) reaction

Aluminium Chloride
AlCl3
Al^3 + 2e- —> Al ( Reduction ) reaction
2Cl- -2e- —> Cl2 ( Oxidation ) reaction

# data[].attributes.body
Lead Bromine
1.  molten lead bromine present
2. The  lead  cations are attracted to cathode
ㄴthe pb²⁺ ions are forced to accept 2 e- to form Pb atom
Pb²⁺ - 2e⁻ --> Pb
3. The bromine anions are attracted to the anode
ㄴthe Br-  are forced to let 1 electron to form Br atom
The br atom then join with other br atom to form Br2
2Br⁻  + 2e⁻  -> Br2
Aluminium Chloride
1. AlCl₃
2. Al³⁺ - 3e- -> Al(reduction)
3.6Cl⁻ + 6e⁻ -> 3Cl₂(oxidation)

# data[].attributes.body
1) Ions present in the electrolyte: Lead 2+, Bromine -
2) The Lead is attracted to the Cathode
3) The Bromide ions are attracted to the Anode
4) Lead is discharged at the Cathode; Reduction, Pb²⁺+ 2e⁻ --> Pb
5) Bromine Gas is discharged at the Anode; Oxidation, 2Br⁻ -2e⁻ --> Br₂

# data[].attributes.body
Lead(II) Bromide:

1. Lead(II) and Bromide

2. Lead(II) cation are attracted to the cathode

3. Bromide anions are attracted to the anode

4. Pb²⁺(l) + 2e⁻ —> Pb(s)
(Reduction)

5. 2Br⁻(l) - 2e⁻ —> Br(g)
(Oxidation)

Aluminium Chloride equations:

Cathode: Al³⁺(l) + 3e⁻ —> Al(s)

Anode: 6Cl⁻(l) - e⁻ —> 3Cl2(g)