- #1
yellowduck
- 16
- 0
Ok, here is another one I have, this is one of a series of half-cell questions... this one is confusing.
79. Balance the following equations by the half-cell method. Show both half-cell reactions and identify them as oxidation or reduction.
b) Cl2(g) + OH- <=> Cl- + ClO3^- + H2O(l)
Oxidation Reaction:
Cl2 (g) <-> Cl-
2e- + Cl2 <-> 2Cl- --- Balanced Cl molecules and electrons
Reduction Reaction:
Cl2 (g) <-> ClO3-
Cl2 + 6H2O <-> 2ClO3- + 12H+ 10e-
Multiply the oxidation reaction by a factor of 5 to cross out the e-
5Cl2 <-> 10Cl-
Add them together:
6Cl2 + 6H2O <-> 10Cl- + 2ClO3- + 12H+
Since this is a basic solution we must swap out the H+ with OH-... in this case adding 6OH- to each side
6Cl2 + 6H2O + 12OH- <-> 10Cl- + 2ClO3- + 12HOH
This seems kinda insane but it may just be right.
Can anyone give me some input on this?
Thanks.
79. Balance the following equations by the half-cell method. Show both half-cell reactions and identify them as oxidation or reduction.
b) Cl2(g) + OH- <=> Cl- + ClO3^- + H2O(l)
Oxidation Reaction:
Cl2 (g) <-> Cl-
2e- + Cl2 <-> 2Cl- --- Balanced Cl molecules and electrons
Reduction Reaction:
Cl2 (g) <-> ClO3-
Cl2 + 6H2O <-> 2ClO3- + 12H+ 10e-
Multiply the oxidation reaction by a factor of 5 to cross out the e-
5Cl2 <-> 10Cl-
Add them together:
6Cl2 + 6H2O <-> 10Cl- + 2ClO3- + 12H+
Since this is a basic solution we must swap out the H+ with OH-... in this case adding 6OH- to each side
6Cl2 + 6H2O + 12OH- <-> 10Cl- + 2ClO3- + 12HOH
This seems kinda insane but it may just be right.
Can anyone give me some input on this?
Thanks.