Hydrogen peroxide (#H_2O_2#) decomposes to form water and oxygen. How do you write the balanced equation for this reaction?

Answer 1

#2H_2O_2(l) rightleftharpoons 2H_2O(l) + O_2(g)#

This is in fact a disproportionation reaction in that oxygen in peroxide (#-I# oxidation state) has given water (#-II# oxidation state for oxygen) and zerovalent oxygen gas (#0# oxidation state for oxygen).
Often a #Mn^(2+)# salt is added to catalyze this reaction.
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Answer 2

The balanced equation for the decomposition of hydrogen peroxide (H2O2) into water (H2O) and oxygen (O2) is:

2 H2O2 (aq) -> 2 H2O (l) + O2 (g)

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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