Question

Al(s) + NaOH(aq) + H2O(l) =​

Answer 1

Answer:

Al(s) + NaOH(aq) + H2O(l) → NaAlO2(aq) + H2(g)

For this reaction, water is contributed as a reagent. This is a redox reaction. Aluminium is oxidized to its +3 oxidation state and oxidation number of hydrogen atom is increased from +1 to 0.

Answer 2

Because Al is an amphoteric metal, it can react with both acidic and basic species. When it comes to reactions, Aluminum does not react with water under normal conditions because an impermeable protective layer of aluminium hydroxide forms within seconds or is already present. The creation of a protective layer is inhibited by adding sodium hydroxide. The amphoteric (capable of acting as either an acid or a base) aluminium hydroxide $Al(OH)_{3}$ enters the solution with the synthesis of aluminates$Al(OH)_{4}$. 

$2Al +6H_{2}O\to 2Al(OH)_{3} +3H_{2}$

$Al(OH)_{3} +NaOH\to Na^{+}+[Al(OH)_{4}^{-}]$

 The aluminium disintegrates totally. 

Hence, the chemical equation is as follows-

$Al(s)+NaOH(aq)+H_{2} O(l) \to Na[Al(OH)_{4}] +H_{2}$

However, the chemical equation, after balancing, looks like this: 

$2Al(s)+2NaOH(aq)+6H_{2} O(l)\to2Na[Al(OH)_{4}] +3H_{2}$