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How do I balance the following chemical reaction: ClO3- + Cl- = Cl2 + ClO2?
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Md. Nure Alam
How do I balance the following chemical reaction: ClO3- + Cl- = Cl2 + ClO2?
How do I balance the following chemical reaction: ClO3- + Cl- = Cl2 + ClO2?
This is not one reaction, but two.
We have reactants with chlorine in the +5 and -1 oxidation states. They can react with each other to form elemental chlorine (oxidation state = 0) or chlorine dioxide (oxidation state + 4). There is no forcing mechanism that requires any particular ratio of Cl2 to ClO2. That ratio can be anything you want … because the reactions are independent.
So write this as two separate redox reactions:
ClO3- + Cl- = Cl2
ClO3- + Cl- = ClO2
and balance each one independently using the usual approach (whatever works).
ClO3- + 5 Cl- + 3 H2O = 3 Cl2 + 6 OH-
5 ClO3- + Cl- + 3 H2O = 6 ClO2 + 6 OH-
You can then, if you wish, combine them in any proportions you choose (1 × Reaction 1 + 1 × Reaction 2, or 3 × Reaction 1 + 2 × Reaction 2, etc.), and the combined reaction will appear balanced.
But this will still be a case of two independent reactions, so any combination is not really a valid chemical equation.
How do I balance the following chemical reaction: ClO3- + Cl- = Cl2 + ClO2?
This is not one reaction, but two.
We have reactants with chlorine in the +5 and -1 oxidation states. They can react with each other to form elemental chlorine (oxidation state = 0) or chlorine dioxide (oxidation state + 4). There is no forcing mechanism that requires any particular ratio of Cl2 to ClO2. That ratio can be anything you want … because the reactions are independent.
So write this as two separate redox reactions:
ClO3- + Cl- = Cl2
ClO3- + Cl- = ClO2
and balance each one independently using the usual approach (whatever works).
ClO3- + 5 Cl- + 3 H2O = 3 Cl2 + 6 OH-
5 ClO3- + Cl- + 3 H2O = 6 ClO2 + 6 OH-
You can then, if you wish, combine them in any proportions you choose (1 × Reaction 1 + 1 × Reaction 2, or 3 × Reaction 1 + 2 × Reaction 2, etc.), and the combined reaction will appear balanced.
But this will still be a case of two independent reactions, so any combination is not really a valid chemical equation.
How do I balance the following chemical reaction: ClO3- + Cl- = Cl2 + ClO2?
This is not one reaction, but two.
We have reactants with chlorine in the +5 and -1 oxidation states. They can react with each other to form elemental chlorine (oxidation state = 0) or chlorine dioxide (oxidation state + 4). There is no forcing mechanism that requires any particular ratio of Cl2 to ClO2. That ratio can be anything you want … because the reactions are independent.
So write this as two separate redox reactions:
and balance each one independently using the usual approach (whatever works).
You can then, if you wish, combine them in any proportions you choose (1 × Reaction 1 + 1 × Reaction 2, or 3 × Reaction 1 + 2 × Reaction 2, etc.), and the combined reaction will appear balanced.
But this will still be a case of two independent reactions, so any combination is not really a valid chemical equation.
How do I balance the following chemical reaction: ClO3- + Cl- = Cl2 + ClO2?
This is not one reaction, but two.
We have reactants with chlorine in the +5 and -1 oxidation states. They can react with each other to form elemental chlorine (oxidation state = 0) or chlorine dioxide (oxidation state + 4). There is no forcing mechanism that requires any particular ratio of Cl2 to ClO2. That ratio can be anything you want … because the reactions are independent.
So write this as two separate redox reactions:
and balance each one independently using the usual approach (whatever works).
You can then, if you wish, combine them in any proportions you choose (1 × Reaction 1 + 1 × Reaction 2, or 3 × Reaction 1 + 2 × Reaction 2, etc.), and the combined reaction will appear balanced.
But this will still be a case of two independent reactions, so any combination is not really a valid chemical equation.
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