Given the balanced equation representing a reaction:
\[ 4Al(s) + 3O_2(g) \rightarrow 2Al_2O_3(s) \]
As the aluminum loses 12 moles of electrons, the oxygen:
(1) gains 4 moles of electrons
(2) gains 12 moles of electrons
(3) loses 4 moles of electrons
(4) loses 12 moles of electrons
Answer (3)
Base on the question, which of the following that sates the balance of the reaction and as the aluminum loses 12 moles of electrons, what could be the oxygen, and base on my research, the possible answer among them is in number (2) gains 12 moles of electrons, I hope you are satisfied with my answer and feel free to ask for more
As aluminium loses 12 moles of electrons oxygen gain **12 moles of electrons.
Explanation ** 4Al + 3 O2 → **Al2O3 **** first write the ions of Aluminium and oxygen
** that is, Aluminium ion is = Al^3+ oxygen ion is = O^2- therefore one atom of Al loses 3 electrons moles while one atom of O gain 2 electrons moles from equation above there a total of number of Al atom are 4 =( 1 x4=4) atoms while Oxygen atoms are 6= ( 3 x2=6) atoms
therefore the total number of Moles of Al lost is = 3 x 4 = 12 moles of electrons
total number of moles of O gained = 2 x6 = 12 moles of electrons
In the given reaction, aluminum loses 12 moles of electrons while oxygen gains 12 moles of electrons. The correct answer to the options provided is (2) gains 12 moles of electrons. This reflects the principle that in redox reactions, the total number of electrons lost must equal the total number of electrons gained.
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