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(A) 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(l) (B) C2H3O2-(aq) + H3O+(aq) → HC2H3O2(aq) + H2O(l) (C) 4 H+(aq) + 4 Co2+(aq) + O2(g) + 24 NH3(aq) → 4 Co(NH3)63+(aq) + 2 H2O(l) (D) CaCO3(s) → CaO(s) + CO2(g) (E) 2 H2O2(l) → O2(g) + 2 H2O(l) The reaction in which a single species is both oxidized and reduced

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Answer:

The reaction (E) 2 H₂O₂ (l) → O₂ g) + 2 H₂O (l) has a single species that is both oxidized and reduced.

Explanation:

Given the reaction (E):

2 H₂O₂ (l) → O₂ g) + 2 H₂O (l)

In hydrogen peroxide, oxygen has an oxidation state of -1. We can see that the reaction is balanced.

The products of the reaction are:

O₂ (the oxidation state of the Oxygen is 0)

H₂O (the oxidation state of the Oxygen is -2)

Hence, 1 mol of Oxygen changes its oxidation state from -1 to 0 (oxidation) and 1 mol of Oxygen changes its oxidation state from -1 to -2 (reduction).

The reaction (E) has a single species that is both oxidized and reduced.

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