What needs to be added in the following reaction to balance electrons? I2 + 12OH− ⟶ 2O3− + 6H2O Select an answerA12 e– on reactant sideB12e– on product sideC10 e– on reactant sideD10 e– on product side
Question
What needs to be added in the following reaction to balance electrons? I2 + 12OH− ⟶ 2O3− + 6H2O Select an answerA12 e– on reactant sideB12e– on product sideC10 e– on reactant sideD10 e– on product side
Solution
To balance the electrons in the given reaction, we need to first determine the number of electrons involved in the oxidation and reduction processes.
The reaction is: I2 + 12OH− ⟶ 2O3− + 6H2O
In this reaction, I2 is reduced to I- (iodide ion) and OH- is oxidized to O3- (ozone ion).
The iodine molecule (I2) is reduced to 2 iodide ions (2I-), which involves a gain of 2 electrons.
The hydroxide ion (OH-) is oxidized to ozone ion (O3-), which involves a loss of 3 electrons.
However, since there are 12 hydroxide ions (12OH-) in the reaction, a total of 12*3 = 36 electrons are lost.
To balance the electrons, we need to add these lost electrons to the reactant side.
So, the correct answer is:
A. 36 e– on reactant side.
However, this option is not given in the choices. The closest option would be A. 12 e– on reactant side, but this would not fully balance the reaction.
Please check the reaction and the options again.
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