It is important to balance redox reactions because if a reaction is
producing 2 electrons then that same reaction must be using 2 electrons.
For example, in example 2, 2 electrons are being produced by the carbon
and only 1 of them are being used up the by the hydrogen. This is not even
so this is why redox reactions must be balanced.
To balance redox reactions there are a few
steps to follow.
- Write down the complete reaction
- Assign oxidation number to each element
- Determine which element is being reduced
and draw a line below the reaction to its pair on the products side
- Detemine which element is being oxidized
and draw a line above the reaction to its pair on the products side
- Write the number of electrons being
reduced on the line drawn in step 3
- Write the number of electrons being
oxidized on the line drawn in step 4
- Determine the least common multiple of
the numbers written in steps 5 & 6
- Take the least common multiple
(determined in step 7) and divide it by the number of electrons being
reduced (determined in step 5) and that number is the coefficient for
the substances that the line connects
- Take the least common multiple
(determined in step 7) and divide it by the number of electrons being
oxidized (determined in step 6) and that number is the coefficient for
the substances that the line connects
- Check the equation to make sure it is
balanced and if it isn't then balance it through the normal methods
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