F. None of the above (Four electrons are transferred).
2Mg → 2Mg^(2+) + 4e^(-)
O_2 + 2H_2O + 4e^(-) → 4OH^(-)
2Mg + O_2 + 2H_2O + 4e^(-) → 2Mg^(2+) + 4OH^(-) + 4e^(-)
2Mg + O_2 + 2H_2O → 2Mg^(2+) + 4OH^(-)
This is a redox reaction in which two atoms of Mg transfer four electrons to one molecule of O_2.
Answer : The correct option is, (A) 0
Explanation :
The given chemical reaction is:
[tex]2Mg(s)+O_2(g)+2H_2O(l)\rightarrow 2Mg^{2+}(aq)+4OH^-(aq)[/tex]
This chemical reaction is a balanced chemical reaction because in this reaction the number of atoms of individual elements present on reactant and product and charges are completely balanced.
In the reaction, (+4) charge present on magnesium will be balanced by the (-4) charge present on hydroxide ion.
So, zero (0) number of electrons are transferred that means there is no electrons are transferred.
Hence, the correct option is, (A) 0
