[biricikelagozlum]

i need help balancing this equation and then answering a few questions.

Al + NaOH + H2O --> NaAlO2 + H2

a-) how many moles hydrogen can be produced from 16g Al?

b-) if 0.35 moles of hydrogen are actually produced, what is the % yield?

[Mitch]

Al + NaOH + H2O --> NaAlO2 + (3/2)H2

Does that work?

[Borek]

2Al + 2NaOH + 2H₂O -> 2NaAlO₂ + 3H₂

Oh, how easy it is to use UBBC codes exported from EBAS

And how easy it is to calculate soichiometry with EBAS

[Alberto_Kravina]

Al + NaOH + H2O --> NaAlO2 + H2

I think that the oxo-aluminate hydrolizes to a hydroxo-aluminate complex since there is water involved in the reaction....

something like: Al + 3 H₂O + NaOH ---> Na⁺ [Al(OH)₄] ^- + 3/2 H₂

...does anyone agree?

[Borek]

I believe we can discuss this problem, to death, as the equilibrium is multistate. Still, there is 1.5 mole of H₂ per mole of Al produced, and that's what counts for the OP question.

[biricikelagozlum]

thanks everyone i figured it out =)