Final answer:
Electrolysis of hydrogen peroxide typically yields oxygen and water with the balanced chemical equation 2 H₂O₂ (aq) → O₂ (g) + 2 H₂O (l). Therefore, for electrolysis of hydrogen peroxide, one would expect twice as much oxygen as hydrogen, if hydrogen were produced at all, since hydrogen gas is not a primary product in this reaction. So, the correct option is C.
Step-by-step explanation:
When you perform the electrolysis of hydrogen peroxide (H₂O₂), it's essential to consider the stoichiometry of the reaction. Electrolysis involves the breaking down of a compound by electrical energy. For water (H₂O), the well-known electrolysis reaction produces hydrogen (H₂) and oxygen (O₂) gases. However, for hydrogen peroxide, the equation looks slightly different. Hydrogen peroxide decomposes into water (H₂O) and oxygen gas (O₂) according to the balanced chemical equation:
2 H₂O₂ (aq) → O₂ (g) + 2 H₂O (l)
This indicates that for every 2 molecules of hydrogen peroxide that decompose, you will get 1 molecule of oxygen gas and 2 molecules (or equivalent volume) of water. Considering the reaction from the standpoint of gases produced, you would receive half as much oxygen as there would be water produced if it were in gaseous form, which is not the immediate product of this reaction. Therefore, the correct expectation for the electrolysis of hydrogen peroxide outcome would be (c) twice as much oxygen as hydrogen, should any hydrogen be produced. However, it is critical to realize that the usual electrolysis of hydrogen peroxide doesn't yield hydrogen gas directly, unlike the electrolysis of water. Instead, it mainly decomposes into water and oxygen. Only if a subsequent process separated the produced water into hydrogen and oxygen, following the typical 2:1 diatomic hydrogen to oxygen ratio, would you see hydrogen gas as a product.