Na ==> Na+
Cl2 ==> Cl^-
You balance
Separate this redox reaction into its component half-reactions.
Cl2 + 2Na --> 2NaCl
4 answers
is it
e- + Cl2 = 2Cl^-
e- + Cl2 = 2Cl^-
close
2e + Cl2 ==> 2Cl^-
In a redox equation it must balance three ways.
1. by atoms
2. by charge
3. by electron change.
Na ==> Na^+ + e
Cl2 + 2e ==> 2Cl^-
Multiply #1 by 2 and #2 by 1 to make the electron change the same.
2Na ==> 2Na+ + 2e
2e + Cl2 ==> 2Cl^- and add
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2Na + 2e + Cl2 ==> 2Na^+ + 2e + 2Cl^-
The 2e cancel (that's why you make them equal; they are on opposite sides and will cancel). You are left with
2Na + Cl2 ==> 2NaCl
2e + Cl2 ==> 2Cl^-
In a redox equation it must balance three ways.
1. by atoms
2. by charge
3. by electron change.
Na ==> Na^+ + e
Cl2 + 2e ==> 2Cl^-
Multiply #1 by 2 and #2 by 1 to make the electron change the same.
2Na ==> 2Na+ + 2e
2e + Cl2 ==> 2Cl^- and add
------------------
2Na + 2e + Cl2 ==> 2Na^+ + 2e + 2Cl^-
The 2e cancel (that's why you make them equal; they are on opposite sides and will cancel). You are left with
2Na + Cl2 ==> 2NaCl
Redox reaction
What is being oxidised and reduced
What is being oxidised and reduced
4 answers