Identify the species undergoing oxidation and reduction. a. `H_(2)S(g)+Cl_(2)(g)rarr2HCl(g)+S(s)` b. `3Fe_(3)O_(4)(s)+8Al(s)rarr9Fe(s)+4Al_(2)O_(3)(s)` c. `2Na(s)+H_(2)(g)+H_(2)(g)rarr2NaH(s)`

Identify the species undergoing oxidation and reduction. a. `H_(2)S(g)

1.	Identify the species undergoing oxidation and reduction. a. `H_(2)S(g)+Cl_(2)(g)rarr2HCl(g)+S(s)` b. `3Fe_(3)O_(4)(s)+8Al(s)rarr9Fe(s)+4Al_(2)O_(3)(s)` c. `2Na(s)+H_(2)(g)+H_(2)(g)rarr2NaH(s)`
Answer» Correct Answer - A a. `H_(2)S` is oxidised because a more electronegative element `Cl_(2)` is added to `H`. Alternatively, a more electropositive element `H` has been removed from S. `Cl_(2)` is reduced due to addition of `H` to it. b. `Al` is oxidised because oxygen is added to it. `Fe_(3)O_(4)` (ferrous ferric oxide) is reduced beacuse oxygen has been removed from it. c. `2overset(0)Na(s)+overset(0)H_(2)(g)rarr2overset(0)Naoverset(-1)H(s)` `2Naimplies2oveset(+1)Na+2e^(-)`(oxidation) `H_(2)+2e^(-)rarr2H^(ө)`(reduction) Therefore, `Na` is oxidised to the concept of electronegativity, the more electronegative element `H` is added to `Na`, so `Na` is oxidised and `H_(2)` is reduced.

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Identify the species undergoing oxidation and reduction. a. `H_(2)S(g)+Cl_(2)(g)rarr2HCl(g)+S(s)` b. `3Fe_(3)O_(4)(s)+8Al(s)rarr9Fe(s)+4Al_(2)O_(3)(s)` c. `2Na(s)+H_(2)(g)+H_(2)(g)rarr2NaH(s)`

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