Aluminium metal can reduce the hydrogen ions in a solution of hydrochloric acid to hydrogen gas, according to the equation:2Al(s) + 6H+(aq) -gt; 2Al3+(aq) + 3H2(g)a) Write half equations for the oxidation and reduction processes involved in this reaction.b) Use these half equations to explain why six hydrogen ions are reduced for every two aluminium atoms oxidised.I can do part a alright but I don't know how to answer part b and it seems so simple but I just don't get it! Any help will be appreciated and thanks in advance :)!
A) Aluminium is oxidized: Al - Al3+ + 3e- Hydrogen is reduced: 2H+ + 2e- - H2 Now, you have to balance to number of electrons, aluminium gives three, hydrogen takes two, so the least common factor is sixHence: 2Al - 2Al3+ + 6e- 6H+ + 6e- - 3H2 From the above two equations, you have see that for every two aluminium atoms, six hydrogen ions are reducedI really hope I helped
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